Unknown Salt Essay

Unknown Salt Essay
The objective of the experiment was to identify the unknown salt that was given. The unknown salt
contained an anion and a cation labelled, 38A. A series of preliminary tests were first conducted in
order to help choose which confirmation tests should be used to identify the compound. The
preliminary tests included pH and solubility, and the behaviour of the salts with concentrated
sulfuric acid. The compound was found to have a slightly acidic pH, around 6.9 while being soluble
in water. The compound showed no change in properties after the addition of concentrated sulfuric
acid. The confirmation tests were then divided into two parts, one for the identification of the cation
and the other for the identification of the anion.
The anion tests ... Show more content on Helpwriting.net ...
The observation of chemical behaviours under specific conditions allowed for the use of process of
elimination. Given the observations found in the materials and methods section and the data found
in the lab manual1 it was found that the anion was not acetate or carbonate, but rather a halide,
specifically Br due to the brown–yellow hue of the organic layer. The observations for the cation test
along with the data from the lab manual1 showed that the unknown was from group II. Since the
flame test showed no observable difference this allowed for the conclusion that the cation was
Mg2+.
For the anion, the most difficult test was the acetate test as the test was concentration dependent and
it also relied on colour as its identifier. This was difficult to achieve as the concentration was hard to
keep constant, and the colour was difficult to pinpoint. Possible solutions include getting access to a
Drypette TM, a manual powder pipette that would dispel a more accurate sample of salt. This would
then make for a more reliable consideration of the color as an indicator of the presence of
... Get more on HelpWriting.net ...

Lipid Simulation
Firstly the shortcut simulation of BTX separation was conducted. The first shortcut column that
receives the feed is representative of the prefractionator, which is the left side of the dividing wall.
Therefore this first column is meant to do sloppy splits of the feed. In this case, the prefractionator is
expected to do a sharp split of Benzene and p–Xylene and a sloppy split of Toluene. For the
prefractionator (SRCT–1), the heavy key will be p–Xylene and light key will be Benzene. This is
because Benzene is the lightest component that is to be removed from the top of the column and p–
Xylene is the heaviest component that is to be removed from the bottom. Since a sloppy split of
Toluene is done, it is divided to the top and bottom of the shortcut ... Show more content on
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In this column, the main separation occurs between the heavy and middle components. Therefore,
p–Xylene is the heavy key and Toluene is the light key. Since the required purity of p–Xylene in the
bottoms is 92%, the remaining 8% must be made of Toluene. Therefore the mole fraction of light
key in the bottoms is specified to be 0.08. Since Toluene is meant to have 9% impurity and 4.5% is
already accounted by Benzene from the top part of the column, the mole fraction of p–Xylene in the
top can be estimated to be 0.045. This is done under the assumption that the molar flow rates of both
middle streams are the same. When SRCT2–Bottoms stream and SRCT3–Distillate stream is mixed
using a mixing unit, it showed the mole fraction of Toluene to be 0.9098. To make the shortcut
simulation to reach the specification, the light key in the SRCT–2 column and heavy key in the
SRCT–3 column was adjusted. After several trail and errors a mole fraction of 0.0505 for Benzene
in SRCT–2 and 0.0402 for p–Xylene in SRCT–3 column gave a mole fraction of 0.91 for toluene in
the side stream. The number of stages calculated by the SRCT–3 column was 29 and the optimal
feed stage was 18. The conditions at which SRCT3–Distillate and SRCT3–Bottoms are produced
can be seen on table 6. Figure 36 shows the SRCT–3 shortcut column. When SRCT2–Bottoms and
SRCT3–Distillate

Acid-Base Titration Lab
Authors: Quentin McCorvey, Scott McCartney, Craig Mathews, and Ross Mather. T.A. Maia
Popova, Professor Yasmin Jessa. 144 Section C. October 15, 2014.
Abstract:
While the goal of this lab was mainly to be able to perform an acid–base titration. Complete a
traditional titration and then and a pH electrode titration. Calculate the molarity of citric acid from
the titration volume of NaOH. Calculations should be fairly close in average and the ending point
should coincide with the equivalence point. All while effectively being able to compare and contrast
the two methods to detect the endpoints of an acid–base titration.
Introduction:
The goal of this lab is to understand the difference between polyprotic and monoprotic acids and to
be able to understand and perform an acid–base titration.
Method:
Traditional Titration ... Show more content on Helpwriting.net ...
After recording the volume of the NaOH. Obtain the 7–UP in an Erlenmeyer flask at about 40.0 mL
also containing 60.0 mL of water and 5 drops of indicator drops. After each trial repeat these steps.
Add the NaOH solution to the flask in 2 mL increments until a faint pink color appears and remains.
This is the endpoint of the titration. The titrant volume is the initial volume subtracted from the final
volume. After this is completed subtract 4 mL from the titrant volume and rapidly add that amount
to the new trial. Continue by adding NaOH drop wise into the flask until the faint pink color
persists. This should be done 3 times for a total of 4

Acid Concentration
Does the amount of active ingredient in different types of tablets decrease or increase per milligram
after its expiration date? Overtime, the concentration of acid in a low dose aspirin tablet increases,
as the concentration of acid in a high dose aspirin tablet decreases. However, due to various
experimental errors, the claim is not a strong and compelling one. What is assumed to have
happened is that both low dose aspirin tablets and high dose aspirin tablets increase in concentration
of acid as the expiration is surpassed.
Four different tablets (two new and two expired): Bayer High Dose 325 mg (exp unknown), Bayer
High Dose 325 mg (exp 8/18), Bayer Low Dose 81 mg Enteric (exp 4/11), and Bayer Low Dose 81
mg Enteric (exp 8/18) undergo the ... Show more content on Helpwriting.net ...
Firstly, the Bayer High Dose 325 mg tablets used as an "old and expired tablet" is unidentified in
expiration date, but the container seems to look very old. This means that it is uncertain whether the
tablets labeled as "old" are actually expired or not (Table 1, 2, and 3). Secondly, not all of the
powdered tablet is put into the beaker. Some remain on the papers while others fly out onto the
table. Because not all contents are present during the titration process, this could very well affect the
calculations measuring the mass of acid per

The Effect Of Ethanoic Acid On The Reaction Of Oxalic Acid
Discussion:
As it can be observed from the data in table 1 (refer to table 1) the concordant of the three titre
values was calculated to be 21.2mL. The results indicate the volume of the titrant, the approximately
0.1 mol sodium hydroxide, required to fully standardise against the primary standard oxalic acid
solution was 21.2mL. The sodium hydroxide was then used to neutralise against the 3g analyte, the
diluted vinegar solution. The data from table 2 depict that the volume of titrant required to neutralise
the analyte was 21.8mL. The results concluded the percentage (mass/mass) of ethanoic acid in
commercial vinegar to be 4.10% in equation 9 after determining the molarity of ethanoic acid prior.
The data collected from the experiment ... Show more content on Helpwriting.net ...
The use of an appropriate indicator is vital in performing a successful titration reaction because the
end point and equivalence point must be as close as possible. The indicator phenolphthalein was
chosen for both parts B and C as in both titrations it was a weak–acid and strong base titration.
Oxalic acid and acetic acid are both weak acids, whereas NaOH is a strong base. At equivalence
points, the resulting solutions contain CCOONa and only. Therefore, salt hydrolysis occurs in part B
and the PH at equivalence point is greater than 7. Phenolphthalein changes colour at PH rang of 8.2–
10.0. The end point of both titrations falls within the pH for colour change of phenolphthalein in the
titration. Additionally, the colour change of phenolphthalein is over a narrow PH range, when the
hydrogen ions equal the hydroxide ions it turns the indicator pink and producing a clear colour
change for easy visible recognition. This further supports why phenolphthalein is the most suitable
for both titrations.
There are predominantly two forms of errors which account for the precision and the accuracy of the
results– these are random errors and systematic errors.
Random errors: The precise data is an indication that the effect of random errors on the data
collected was minimum in part B. If there were any random errors that affected the precision of
results, then there would have been variation present in the results, thus

Essay on Laboratory Techniques and Measurements
Title
Laboratory Techniques and Measurements
Purpose
The purpose of this experiment is to determine mass, length, temperature, volume, and density of
objects and liquids using common measuring devices and algebraic formulas. The metric system, the
most common set of measurements used in science, which includes meters, liters, Celsius, and
grams will be used.
Procedure
The following items were used within the experiment:
(1) Metric ruler with centimeter (cm) and millimeter (mm), (1) table salt, (1) small number of ice
cubes, (1) piece of string, (1) isopropyl (rubbing) alcohol, (1) tap water, (1) distilled water, 25 mL,
(1) paper, 5 cm x 5 cm for weighing chemicals, (1) colored drink, (1) beaker, 100 mL, glass (1) ...
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(NH4OH was used instead of NH3 because it was not available.)
An empty and distilled cleaned pipet was used to drop substances on the paper.
Observations / Data Table 1
Chemicals Well # Reaction on White Paper Reaction on Black Paper
NaHCO3
(sodium bicarbonate) HCL
(Hydrochloric Acid) A1 Mixture absorbed within paper within seconds; Clear bubbles appeared
within the product; stained clear Clear bubbles within the product; Product was slow to absorb into
paper; once substance was absorbed, the paper stained green
HCL
(Hydrochloric Acid) BTB
(bromthymol blue)a A2 Mixture beads on paper; Appears orange; Slow to absorb mixture; color
changed green and dried yellow–tan with a green border
NH3
(Ammonia) BTB
(bromthymol blue) A3 Mixture absorbed within paper within seconds; appears blue Absorbed
immediately; Appears blue

HCL
(Hydrochloric Acid) Blue Dye A4 Mixture absorbed within paper within seconds; Substance appears
green Slow to absorb mixture; did not change color of paper; Dried Green and tan
Blue Dye NaOCl
(sodium hypochlorite) A5 Mixture absorbed within paper within seconds; Aquablue Slow to absorb
mixture; Green with yellow border
**Forgot to add 1 drop of HCl
NaOCl
(sodium hypochlorite) KI
(potassium iodide) A6 Mixture absorbed within paper within seconds; Yellow Slow to absorb
mixture; Yellow
Add 1 drop of

Acid-Base Titration Lab
The purpose of the Acid–Base Titration Lab was to determine the concentration of sodium
hydroxide by titration against a standard solution. A titration is a laboratory method used to
determine the concentration of an acid or a base in a solution by performing a neutralization reaction
with a standard solution. It detects the equivalence point between the acid and base where they
neutralize each other. The materials used in this procedure were HCL solution, water, ring stand,
burette, burette clamp, unknown concentration of NaOH, phenolphthalein, erlenmeyer flask, and
graduated cylinder. To start the procedure, obtain a burette, and rinse the burette with water and
check if the burette is able to release the solution. Next the ring stand must ... Show more content on
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Trial two started with 0 mL of NaOH and ended at 17.3 mL. On trial three NaOH started at 0 mL
and it ended at 21.5 mL. The molarity of HCL was 0.1 M and its volume was 20 mL. The average of
sodium hydroxide used was 19 mL. Using the dilution equation, 0.1 M of hydrochloric acid
multiplied by 20 mL of hydrochloric acid is 2. Taking 2 divided by 19 mL of sodium hydroxide
gives 0.105 M as the molarity for NaOH. The calculated unknown molarity of NaOH was 0.105 M.
This compares to the known theoretical molarity of NaOH which was 0.1 M. The molarity of
sodium hydroxide from the experiment is close to its theoretical hydroxide meaning the results of
the experiment were accurate. The final volumes of NaOH were also close to each other therefore
the results were both accurate and precise. Hydrochloric acid is an example of an strong acid and
sodium hydroxide is an example of a strong base. When a strong acid and a strong base react, the
neutralize each other. Carrying out a titration between a strong acid and a strong base is done to find
the equivalence point. The point at which chemically equal amounts of the acid and base have been
mixed and neutralized each other. Neutralization between a strong acid and base such as HCl and
NaOH will result in a solution with a pH of 7.0. If the final solution does not have a pH of 7.0 errors
that might have occurred include misjudging of color indicator, using a contaminated

Ph Lab
Name: Amra Aliyu
Lab partner: Jamie Liang
Lab: pH At The UN
Course: Chem 106
Date: 7/11/2015
INTRODUCTION pH is a scale that is used to determine the acidity or alkalinity of a solution. A
solution
with a pH less than 7 is considered acidic and a solution with a pH of more than 7 is considered
basic. In the first part of this lab we had to make several solutions and using a litmus paper
deduce it's pH number, this is done by analyzing its color, and determine if the solution is acidic
or basic. In the second part we had put a basic solution into several solutions to see if it would
have an effect on its pH. A more detailed information about the procedure can be found in
Cornerstone chemistry lab for Hunter college chemistry 106 students.
DESCRIPTION OF SUBSTANCE
.10M acetic acid– clear liquid
1.0M acetic acid– clear liquid
.5M hydrochloric acid– clear liquid.
1M nitric acid– clear liquid
1.0M sodium acetate– white ,solid
.1M Potassium dihydrogen phosphate– white powder
.5M potassium hydrogen phosphate– white powder
.2M ammonium chloride– white powder
1M sodium hydroxide– white solid
.01M sodium hydroxide– white solid ... Show more content on Helpwriting.net ...
Since we were dealing with a solid we knew that we had to prepare our solution. In doing so we
identified that the formula weight of the solid listed on its perspective bottle was 174.18 g/mol. We

set up a proportion (174.18 g/mol)*(0.05 mol/1L)*(1L/1000mL)*15mL), and determined that we
needed .1305 gram of the solid to be weighed out. After weighing out the calculated mass, we then
proceeded to place the solid into a clean beaker and then added 50mL of deionized water using a
graduated cylinder. The solution remained clear as the solid dissolved via mixing and swirling, and
we were certain that we had added the right amounts of solid and water, because when we tested the
pH value of the solution via a pH strip, we got a pH value of 8 due to the strip turning

ADI Molarity Lab Report
In the ADI Molarity Lab, the primary tasks was to use different values of moles of solute, volume of
solvent, and molarity to find the mathematical relationships between them. To find these
relationships, our group had to change the quantities of each of the variables and visually observe
the molarity within the solution. For instance when using Cobalt (II) Nitrate to find the relationship
between volume of the solution and the molarity of the solution; the group kept the amount of moles
of the solute at a constant of 1.00 moles because if it would have changed it would have caused
inaccurate data. We first set the volume of the solution to 0.2 liters. The molarity of the solution was
5.00 mol/L. Then we changed the volume of the solution ... Show more content on Helpwriting.net
...
We kept the volume at a constant 0.50 L and first set up the moles to 1.00 moles. The molarity of
Co(NO3)2 was 2.00 mol/L. When we decreased the number of solute moles to 0.50 moles, the
molarity of the solution was 1.00 mol/L. The quantitative data was collected and we concluded that
the relationship between the number of solute moles and the molarity of the solution was direct for
the reason that whenever the the moles increased, the molarity increased. However, when the moles
decreased the molarity decreases as well. We then combined the two relationships to conclude that
the derived unit for molarity is the number of moles/volume of the solution. We believe our claim is
right because it was not opinion based. Our theory is proven by facts and that is the simple reason.
To conclude, our claim is that the relationships consist of the following: number of moles of the
solute is directly proportionate to the molarity of the solution; the volume of the solution is inversely
proportionate to the molarity of the solution; and that the derived units for the molarity are number
of moles of the solute per the volume of the

Lab Report Titration
A titration is a common method used in the scientific labs for quantitative analysis of chemicals, we
use titrations to determine the unknown concentration of an identified analyte using a solution of
known concentration. Normally, the known solution (titrant) is put into a burette to a known
quantity of the unknown solution (analyte) until the reaction is complete. We can tell that the
reaction is complete by using an indicator which usually signals the end of the reaction by a colour
change, also known as the endpoint. Alternatively, pH meters can be used to record something
known as the pH difference; pH is a measure of hydrogen ion concentration of a solution. Solutions
with a high concentration of hydrogen ions have a low pH, while solutions ... Show more content on
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May fall, causing spillages and glassware breakages. Ensure chairs are well tucked underneath the
desks. Remove bags coats and any other personal belongings from the practical areas when doing
the practical as this may cause an obstruction to carrying out the experiment efficiently. Run cut
under cold water for 15 minutes until bleeding stops. Disinfect and use plaster. Seek medical
attention. Dispose broken glass with dustpan and brush.
Part One– Creating a standard solution of Na2CO3 (anhydrous sodium carbonate).
The equipment required to complete this practical was received from the lab technicians who had
already pre–rinsed the equipment with distilled water and dried in a drying cupboard.
EQUIPMENT:
Weighing Boat – to accurately weigh out the mass of the substance. It is made from plastic and
allows the powered substance to easily slide off leaving a minimum amount of residue on it.
250cm³ Volumetric (graduated) flask – to accurately measure out an amount of Na2CO3 solution,
the shape of the flask enabled the solution to be swirled and mixed more easily and efficiently ,
preventing any

Quantitative Analysis Of Mefenamic Acid And Redox Titration
Mefenamic Acid Introduction of titration method Titration is a lab method that used to determine a
quantitative analysis which used to know the concentration of a drug or compound, and this process
happen by use a reagent which is known its concentration and its volume to calculate the another
concentration or volume, this reagent called titrant and it may be acid or base. There are many types
of titration to determine different orders of drugs and compounds like (acid base titration– Redox
titration– Gas phase titration– Complexometric titration– Zeta potential titration). The most common
method for quantitative analysis is acid– base titration and redox titration. 1– Acid base titration is
the method which depends on the naturalization between acid and base in the flask then changes the
color of ph. indicator (ph.ph or methyl orange) till reach the endpoint. 2– Redox titration is the
method which relies on reduction–oxidation reaction between titrant and sample and we use a redox
indicator toll reach the indicator. 3– Gas phase titration this method of quantitative analysis is occurs
in gas phase. 4– Complexometric titration is depend on form a complex between titrant and sample
in which we are used a complexometric indicator which this indicator form a weak complex with
sample, then the titration happen till reach the endpoint. 5– Zeta potential titration we use this

Introduction To Identity The Unknow Acid Solution
The purpose of this experiment is to identity the unknow acid solution through determining the Ka
value of the reaction experimentally. The colors of unknown acid 3 matches the colors of test tube 1,
with thymol blue being light pink, malachite green being dark green and crystal violet being cyan.
Comparing it to other 3 test tubes, test tube 2 has a similar result. Both test tube 3 and 4 have higher
Ph than 1 and 2, since thymol blue is yellow and crystal violet is purple in test tube 3, rose and blue
in test tube 4. Crystal violet is green in test tube 2, which shows that it has a lower ph than test tube
1. So, the order of acidity from most acidic to least acidic is 2143. Dichloroacetic acid is the second
strongest in those 4 acids; this suggests that unknown acid 3 is dichloroacetic acid.
Discussion question:
Phenolphthalein is an indicator commonly used in acid–base titration. Explain how the equivalence
point of acid–base reaction can be determined using this indicator. State relevant reactions, pH
ranges and qualitative ... Show more content on Helpwriting.net ...
According to Le Chatelier's principle, the equilibrium shifts to the left, making Phenolphthalein
colorless. At a high ph level where the H3O– concentration is low, the equilibrium shifts to the right,
showing the pink color of Phenolphthalein. This allows it to be used in both weak acid–strong base
and strong acid–strong base titration. In a weak acid and strong base titration, the equivalence point
would be above 7 due to the reaction occur between the conjugated base and water. This often
makes the pH value detectable by Phenolphthalein. In a strong acid and strong base titration where
the equivalence point is 7, the spike of pH around equivalence point is huge and all indicators at this
range change color at the same volume of acid or base. Therefore, using Phenolphthalein in this case
won't cause major

Lab Report Ph Indicator Results
RESULTS
One drop of phenolphthalein indicator was added to each Well in row A and the color of each
solution was recorded in Data Table A. Wells A1 through A4 remained clear and transparent. A5
turned a murky pink. The A5 pencil mark on the paper below the Wells was still slightly visible. A6
turned a clear light pinkish purple.
The pH of each Well in row B1 to B6 was tested with a pH strip.
B1 turned the pH strip a dark pink or red rose color, the pH was recorded at one. B2 turned the pH
strip an orange color that had a pink hint to it, the pH was recorded at three. B3 turned the pH strip
an orange color with a darker ring of orange, almost red around it, the pH was recorded at four. B4
turned the pH strip a yellow color with a ring of ... Show more content on Helpwriting.net ...
The color in Well C1 was a transparent light pink rose color, the pH was estimated to be between
two and three. This estimate is slightly higher than that of the pH strip test. The color in Well C2
was a transparent redder pink, the pH was estimated to be around a two. This estimate is slightly
higher than that of the pH strip test. The color in Well C3 was transparent and was a similar color to
Well C1 but with lighter orange and pink, the pH was estimated to be around a three. This estimate
is slightly lower than that of the pH strip test. The color in Well C4 was a transparent light green, the
pH was estimated to be around a seven. The estimate of pH from the universal indicator is the same
as that of the pH strip test. The color in Well C5 was a transparent darker green with hints of blue,
the pH was estimated to be between a seven and an eight. The estimates are roughly the same,
between all three of the pH tests. The color in Well C6 was transparent was a dark blue, purplish
color, the pH was estimated to be a thirteen or a fourteen. This estimate is slightly higher than that of
the other tests, this could be due to numerous factors. One factor could be that the pH test simply did
not reach pH's of 13 and 14, like in the case of the pH strip test. Another factor is that the first
attempt at administering the indicator in Well C6, the drop from the pipette missed and hit

Titration Of A Strong Acid
It is believed that a strong acid that is titrated with a strong base will produce a resultant solution has
a pH that is slightly over 7. This is because strong acids have a lower pH and solutions that are less
basic than weak acids that have been titrated with strong bases. When a weak acid is titrated with a
strong base it will produce a resultant solution that is well above 7 because it starts off with a higher
pH. Acids and bases with high concentrations result in large changes in pH, while acids and bases
with low concentrations result in smaller changes in pH.
1. The titration curve would stop at the equivalence point. This is because the indicator changes the
solutions colour at this point.
2. In order to titrate with antacids (solid ... Show more content on Helpwriting.net ...
It would take less NaOH to neutralize CH3COOH compared with the amount of NaOH required to
neutralize HCl acid. This is because acetic acid is a weak acid has a stronger conjugate base. This
by–product helps to raise the pH to 7, a neutral level. HCl is a strong acid and has a weaker
conjugate base. This by–product is not very effective in helping to neutralize the acid. CH3COOH
also starts off with a higher pH since it is weaker; this means that it is closer to the neutral pH level
than HCl is.
6. The pH of HCl at equivalence point is less than the pH of CH3COOH at equivalence point. This
is because HCl starts at a lower pH level than CH3COOH, since it is a strong acid.
7. To classify an acid as either a strong acid or weak base you can test how they react with water. If
the acid is strong, it will ionize completely. If the acid is weak it will only partially ionize when
introduced to water.
9. If the acid is strong, the titration curve will have a lower equivalence point than a weak acid. If it
is a monoprotic acid, there will only be one equivalence point, while polyprotic titration curves will
include several equivalence

Mannitol Salt Agar Lab Report
Mannitol Salt Agar (MSA) differentiates halophile bacteria, and bacteria's ability to ferment
mannitol. Fermenting mannitol results with a yellow halo around colony from the acid produced
(staphylococcal species). MSA is composed of enzymatic digest of casein and animal tissue
(nitrogen, vitamin carbon source), D mannitol (carbohydrate), NaCl (7.5%, halophiles), phenol red
(indicator pH 6.8 turns yellow), and agar (coagulate), with a final pH of 7.4. Unknown 6 did not
grow since it is gram negative, and cannot tolerate the high salt concentration. Also there was no
yellow halo since the colony did not survive therefore could not metabolize mannitol. This is
because there is not a thick peptidoglycan wall; therefore the cell will go through ... Show more
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Durham tubes differentiate a microorganism's ability to ferment sugar (mannitol, dextrose, and
lactose) that may produce a gas, but acidic byproducts will turn solution yellow. Unknown 6 was
yellow in all three test tubes suggesting acidic conditions (fermentation occurred), however lactose
and mannitol were cloudy, dextrose remained clear. There was no gas present in any of the Durham
tube. Urease broth determines if a organism can hydrolyze urea with urease. It contains urea,
nutrients, pH buffers, phenol red (indicator). Unknown 6 tested negative because it remained yellow
and clear, therefore the pH did not rise, because no acid was produced from hydrolyzing urea. Sulfur
Indole Motility Media (SIM deep) differentiates microorganisms that reduce sulfur, produce indole,
and are motile. H2S is reduced by cysteine catabolism, or thiosulfate, and HCl, p–
dimethylaminobenzaldehyde, n–amyl alcohol (Kovac's reagent). SIM deep contains nutrients,
peptone (tryptophan), iron, sodium thiosulfate. Unknown 6 tested negative to sulfur reduction and
indole production, and remained yellow (after Kovac's reagent was added), and it is non–motile
since the agar remained clear. Kliger's Iron Agar (KIA) differentiates glucose, and lactose
fermentation to acids and gasses, specifically sulfur reducers. It contains small amounts of glucose
(to be exhausted), phenol red (indicate acid), lactose (secondary sugar). Fissures are the result of gas
byproducts. Unknown 6 fermented glucose, it failed to ferment lactose. It remained red with a
yellow butt, the surface was pink. It tested negative for H2S, or gas formation.Simmons Citrate Agar
tests an organism use of citrate as the only carbon source. Citrase hydrolyzes citrate into oxaloacetic
and acetic acid. Oxaloacetic acid is hydrolyzed into pyruvic acid and carbon dioxide. It contains
sodium citrate (carbon source), ammonium dihydrogen phosphate (nitrogen source), nutrients, and

Titration In The Medical Field
Today, in the real world, titration is used in the medical field to find the concentration of blood and
urine. It is also used to find a certain amount of a chemical in a food. A titration is a way to the
concentration of an unknown solution by using a solution with a known concentration. The
unknown solution is called an "analyte", while the known solution is called the "Titrant". The
glassware used in order to preform titrations is a buret or "burette". A burette is a glass cylinder with
a tap on one of the edges. It is used for measuring volumes of liquids, especially in titrations.
Standardization (sometimes referred to as standardisation) is a way of putting something or make
something into technical standards. Standardization is used when doing a titration since it finds out
the exact concentration of a solution that you want to use to find the concentration of the analyte.
An equivalence point in a titration is when the moles of the titrant equal the moles of a analyte. One
way to find the Equivalence point is through the pH indicator. This is an indicator that changes color
when there is a chemical change. An acid and base indicator changes color depending on what the
pH is. There are also Redox ... Show more content on Helpwriting.net ...
In order to find a standard solution you must first, add water from a cleaning bottle to dissolve it.
Second, you would need to use some of the water to rinse off all the substance off the watch glass.
This needs to be done at least two times. Then stir with a glass rod until all the of the solid substance
is dissolved, then put the solution to the volumetric flask. The laboratory method is when you drop
the titrant into the analyt. (basically titration). The results you get are titration, pH level, and the
moles. The equation to find molarity/concentration is: M1 x V1 = M2 V2. In conclusion, titration is
very useful in the modern day. It's also pretty

Red Cabbage Ph Indicator Lab
Science Essay:
Red Cabbage PH Indicator
Did you know that, instead having to buy expensive PH indicators, you can just use the juice from
red cabbages? In this experiment, I will see how red cabbage can go from side dish to science. My
hypothesis is that the color of red cabbage will change color based on a reaction with different
substances to indicate whether it is an acid or base. According to the page madsci.org, red cabbage
contains a pigment called 'anthocyanin.' this pigment "changes its structure and its reaction to light
depending on the acidity of its environment." For this experiment, I only needed a few typical
household items. This is a list of everything I used:
One small, red cabbage
Cheese grater
Boiling water
Four ... Show more content on Helpwriting.net ...
It is important that the liquid is allowed to cool to room temperature so that residual heat doesn't
affect the PH readings. Now I have a homemade PH Indicator!
Using an eyedropper, I added a few drops of the indicator into each of my substances and viewed
the color changes through the clear plastic cups. I used the chart below to determine each substances
PH level by matching its colour to the chart below. The lower the PH level the more acidic, so a
violet red color is highly acidic; whereas a yellow color is highly basic.
I tested a few of the most common substances used in daily life: milk, soda, lemon juice and bleach.
My results are the following: In my first test, I tried testing the PH level of milk. I first thought that
milk would be basic, but after dripping some of the cabbage mixture into it, I discovered that it was
light blue, which means that it was actually slightly acidic! After researching this, I found that this is
true because milk contains lactic acid, which is responsible for the sour flavor of sourdough breads.

Red Cabbage Ph Lab
Red Cabbage pH Mark Lab Work
The Goal of the investigation was to look for and understand the different chemicals (Acids, alkalis
and neutral) work and see a change in color.
Introduction:
The red cabbage mark shows how simple household product such as red cabbage can make a
suitable mark and be able find out if a chemical is either an Neutral, alkali or acid. Chemicals that
are acid reacts with an alkali neutralizing it making water and a salt. Acids commonly are sour
tasting. Acids change with metals, releasing hydrogen gas and leaving behind a salt. Acids conduct
electricity. Acids also readily give off hydrogen ions and have a pH level lower than 7. Simple
common acids are sulphuric, Nitric. The acid commonl used in car batteries are sulphoric acid with
electrolyte. ... Show more content on Helpwriting.net ...
Contact with any other chemical should be treated as this one.
8. All protective gear listed above should be used in the experiment in the same way.
9. Hair tied back.
10. Jewellery to be taken off
11. Results:
|Solution Name |Color of Indicator |Acid/Base/Neutral | Bleach |Green |Acid | |Baking soda
|Blur/Green |Base | |Distilled Water |Purple |Neutral | |Lemon Juice |Red/Fuschia |Acid |Purple
|Vinegar |Red/Fuschia |Acid |
Discussion:
The results found it the experiment adheres to the hypothesis. As shown in the Results above we
were able to find out the chemical compounds that were acidic, those that were alkalis and those that
were neutral. This was identified by using a known acid (Bleach) and a known base (Baking Soda).
We have also discovered that when mixing an acidic compound with the indicator it had an green or
a fuschia. When an alkalis compound was mixed with the indicator it would result in a green or a
reddish type of

Depletion Of The Reducing Agent Of Sodium Tioglycolates
This test utilizes a medium that has an oxygen gradient, meaning that most of the oxygen was at the
top of the tube, and the least amount of oxygen was at the bottom of the tube. To prepare this
medium, a reducing agent called Sodium thioglycolate was added, removing the free oxygen by
chemically binding with it. Thioglycolate broth, also called a reducing medium, eradicates the tube
of oxygen. Rasazarin is a pink dye that indicates oxygen depletion an indicator for oxygen
depletion. The test results determine oxygen requirements the organism requires.
1. Strict aerobes need oxygen to grow. Growth will only appear at the top of the tube.
2. Strict anaerobes require the complete absence of oxygen. Growth will only appear at the bottom
of the tube.
3. Facultative Anaerobes do not require oxygen, but develop best aerobically. Growth will be shown
throughout the tube, usually more at the top and minimizes as the microbe descends.
CATALASE TEST:
Some facultative aerobes have the enzyme called catalase, which catabolizes hydrogen peroxide
(H2O2) into harmless water plus oxygen. A chunk of the unknown colonies was transferred onto a
slide and added a drop of H2O2 onto the colony. A positive test result showed oxygen bubbles rising
up from the plate. That meant that the organism had the enzyme, resulting as catalase positive. A
negative result showed no appearance of bubbles.
OXIDASE TEST:
Some aerobes have the enzyme called cytochrome oxidase, which is a molecule that is a terminal
electron acceptor in the Electron Transport Chain (ETC). A Q–tip was used to pick up the unknown
organism and then administrated a drop of reagent, Dimethyl–p–phenylene diaminic hydrochloride.
Results were obtained within a minute duration. If purple was observed in less than a minute, it was
positive for oxidase. If there was no color change within a minute, it was negative.
OXIDATION–FERMENTATION (O–F) TEST FOR GLUCOSE
This test attempts to extrapolate a microbe's ability to ferment or oxidize glucose. The pH indicator
utilized in this test was Bromthymol blue, which is yellow when acid is present. The procedure
involved stabbing two O–F tubes of glucose. One tube needed a layer of sterile oil to create an
anaerobic environment

Ph Neutralization Investigation
In this experiment, the group was given two unknown solutions and were told to discover the pH of
each solution and if the two unknown solutions could be neutralized. The question they were solving
for was; "How do you determine whether two solutions are acids or bases and whether these two
solutions will neutralize each other and change their pH level?" The hypothesis the group decided
on was; "We predict that if the unknown solutions are acids they will turn the blue litmus paper red
and if they are basic, they will turn the red litmus paper blue. We predict that one of the two
unknown liquids will be acid and the other will be base, so if the two unknown solutions were put
together, they will neutralize each other and have a pH around 7." There was no other research done
on this project.
Materials: two pitchers, a bucket to pour out waste liquids, lemon concentrate, baking soda , 3
containers, rulers, sharpie markers, pH papers (litmus paper), paper towels, and a journal to record
the data. Procedures: (1) Gather materials (three containers, rulers, ... Show more content on
Helpwriting.net ...
Turned red litmus paper blue slowly, this means this solution is slightly basic.
Turned red litmus paper blue very slowly, and turned red litmus paper purple colored. This means
that the solution is slightly base because it turned red litmus paper blue.
One thing that caught the group off guard was the fizzing and bubbling that occurred right when the
solution in container B (slightly basic) interacted with the solution in container A (acidic). Our
hypothesis was partially right (valid) because the two solutions in container A and container B did
turn the litmus paper red and blue (red for container A and blue for container B). However, the two
liquids did not neutralize as the group expected it to in container C. Instead it was slightly more
basic (above 7 on the pH

Investigation Of A Titration Process
Purpose: The purpose of this lab was to determine how to use an indicator in a titration process, in
addition to using indicators to determine pH.
Materials:
DI water
Buret
Stand
Clamp
150ml beaker
Waste beaker
Vitamin c tablet
Vitamin c solution
Phenolphthalein
Acetic acid solution
Ammonium hydroxide solution
Ammonium chloride solution
Sodium acetate solution
Sodium carbonate solution
Glass stirring rod
Well plate
Mortar and pestle
Erlenmeyer flask
Weighing pan
Procedure: Vitamin C Titration
1. Set aside a waste beaker.
2. Acquire a vitamin C tablet and record its mass.
3. Use a mortar and pestle to crush the tablet.
4. Re–record the mass of the powder
5. Transfer the powder to an Erlenmeyer flask
6. Add 75mL of DI water to the flask
7. Add three drops of indicator to the flask.
8. Acquire 60mL of NaOH in a 150mL Beaker.
9. Record NaOH concentration
10. Fill a 50ml buret with NaOH and place buret in stand

11. Place Erlenmeyer flask under buret
12. Record initial buret reading
13. Titrate until color change sustains for greater than 30 seconds. If color change does not occur,
determine a suitable point to stop.
14. Record final buret reading.
15. Dispose of titration mixture with running water
16. Repeat steps 2–15 for second indicator.
17. Clean and rinse all glassware before putting away.
Acidity of Aqueous Solutions
1. Acquire well plate and vitamin c tablet solution, acetic acid, ammonium hydroxide solution,
ammonium chloride solution, sodium acetate

Lab Report On The Mass Of Actual Aspirin ( Acetylsalicylic...
Abstract: This experiment utilizes skills of titration in order to find the percent mass of actual aspirin
(acetylsalicylic acid) in store–bought aspirin. Two steps and two kinds of titrations are used. First,
approximately 0.1 M NaOH solution was standardized using titration with KHP. KHP was used
because it does not absorb moisture when it is stored, and it is soluble in water. The reaction that
takes place in this reaction is a 1:1 mole ratio reaction. The titration determines the volume of NaOH
solution needed to completely react with the known amount of KHP. This makes the calculation of
molarity of NaOH solution fairly easy. The average molarity calculated was 0.09897 M. The final
part of the experiment is a titration to indicate the amount of acetylsalicylic acid present in
approximately 0.5 g of store–bought aspirin. The volume of 0.09897 M NaOH solution indicated the
moles of NaOH that reacted with the aspirin. The reaction between NaOH and acetylsalicylic acid is
a 1:1 mole ratio reaction. The calculated mass of acetylsalicylic acid was 0.3963g. This was divided
by the initial amount of aspirin measured (0.4976g), and multiplied by 100 to give the percent mass.
This value is 79.66%. This particular experiment may not be very accurate. Specifically, only two
standardization trials were counted. This may cause a less accurate measurement of NaOH solution
molarity, ultimately leading to an inaccurate percent mass of acetylsalicylic acid.
Introduction

Methyl Orange Synthesis Lab Report
Experiment 11B consisted of synthesizing methyl orange, a synthetic dye, and testing this dye's
coloring quality and effectiveness as a pH indicator. Methyl orange is an acid–base indicator. In a
pH of greater than 4.4, it becomes a yellow solution with a negatively charged sulfonate ion. When
submerged into a solution with a pH less than 3.2, the dipolar red ion (helianthin) predominates.
Methyl orange is a type of azo dye, which is commonly found in food, fabric, paint, and other
brightly colored products. The general structure consists of the N5N functional group sandwiched
between two aromatic species. Azo dyes are brightly colored because of their extensive conjugated
system which gives rise to a strong chromophore. The exact color depends on both the nature of the
aromatic group and the substituents. Methyl orange is synthesized through an azo coupling reaction
between a diazonium ion and N,N–dimethylaniline. An electrophilic aromatic substitution causes
the positively charged diazonium ion to act as the electrophilic species. In the first step of azo
coupling the diazonium intermediate is synthesized. This process is called diazonation, in which the
diazonium intermediate is formed by the reaction between sulfanilic acid (an aromatic amine) ...
After this we added .5g of NaCl and allowed the solution to cool to room temperature then placed it
into an ice bath. The reaction mixture turned into a lighter shade of yellow and began to crystallize.
The crystals were filtered through a Buchner funnel and rinsed twice with saturated aqueous NaCl
solution. The reaction mixture was placed in a boiling water bath in order to dissolve most of the
dye and all the contaminating salts. It was then cooled in a ice bath and filtered using a Buchner
funnel. The product obtained was shiny and a metallic gray–gold color. The product weighed in at
.207g of methyl orange, giving us a percent yield of

Hydrochloric Acid Lab
bstract: This lab explored the effectiveness of various antacid tablets in regard to Sodium
Bicarbonate. The effectiveness of the antacid tablet was measured by how much NaOH was added
to the antacid and HCl solution, and the results indicated that the brand name product consumed
0.00391 mol of HCl compared to the off brand product that consumed 0.00250 mol of HCl which
shows that the name brand product was a better antacid. Introduction: In this experiment, two
different types of antacid tablets is used to determine which one is more effective. The two types
that are used are Tums and an off brand generic version of Tums from Walgreens. According to the
Tums antacid commercial, this antacid is advertised as being the best. Upon completion, ... Show
more content on Helpwriting.net ...
Add 5 mL of 0.1 of M hydrochloric acid to the buret for rinse. Discard the acid. Rinse the buret with
acid solution two more times. Add 0.1 M HCl solution to the same buret. Volume will need to be
adjusted to the zero mark. Add 5 mL of 0.1 of M hydrochloric acid to rinse another buret. Discard
the base. Add 0.1 M NaOH solution to the buret. Rinse the buret with the base solution two more
times. Volume will need to be adjusted to the zero mark. Clean the 125–mL Erlenmeyer flasks with
water. Use distilled or deionized water for a final rinse. Wet flasks can be used for titration. In a
clean 25 mL volumetric flask, measure out 0.0020 mole of acetic acid. Make sure to use all the
digits on the balance. Add water to line indicated on the flask. In 125–mL Erlenmeyer flask, add the
mixture and 3 drops of phenolphthalein indicator solution. Use sodium hydroxide to titrate the
solution until the color turns pink. Wait for at least 30 seconds to see if the pink color continues.
Record the volume of 0.1 M NaOH solution used. In 125–mL Erlenmeyer flask, rinse very well with
water. Use distilled or deionized water for a final rinse. Wet flasks can be used for titration. Titration
procedure should be repeated 2 more

How Does Red Cabbage Extract As An Indicator Used To...
Griffin
Dr. Burrell
Bio–111–900
April 10, 2016 Determining pH
Introduction:
In this Lab report we will be using Red Cabbage extract as an indicator to determine the pH of
substances. The purpose of this experiment is to see if and how base and acids react. Indicators are
chemicals that change color depending on the pH solution that they are dissolved in. This
experiment will determine which items we use to determine ph. The pH of a solution indicates its
acidity or alkalinity. There is a ph. scale that determines if the items such as lemons or bleach are an
acid or a base. I have chosen to use red cabbage in this experiment so that I can know the range of
the item that ... Show more content on Helpwriting.net ...
Buffer solutions needed are in test tubes. Then get seven test tubes and place them in a rack and
label them. Place 3 ml of buffer into the (test tube 1 should be put in 1). I then put the appreciate
amount in I each tube. Then added 1.5 mL of red cabbage juice to each tube. Then I covered the
tubes with Para film and mixed thoroughly and waited until I saw changes if there were any.
Results:
The results of my experiment were as follows the pH of 2 has a pink color and the ph. of 12 had a
blue color. As I go down the chart the pH turned darker as I got to 6 and higher. See the figure 1 for
the changes in the color as you go from a pH of 2 to 12. As I got to 10 it was still a green blue color.
Figure 1
Discussion:
I have found out that the any number below 7 is more acidic such as lemons and bananas. I have
found that in conducting this experiment that cabbage juice was more acidic when added to the Ph.
of 6 or less within the buffer solution. Greater with the more Alkaline. There is more acid which
makes the solution a red to pink color and then it goes to neutral then it go to green than to blue as
the level gets

Determining The Titration Of An Unknown Solution
This experiment explores techniques of a titration, where a solution of a known concentration is
used to determine the concentration of an unknown solution. Titrations are performed with a burette,
which was created by Francois Antonie Henri Descrozilles, which contains the titrant, and a glass
container such as a beaker or flask that contains the analyte.1 The titrant is solution of a known
concentration that is slowly added to the analyte which is solution that is being analyzed to
determine the unknown concentration of the solution. Inside the analyte is also an indicator that
changes color near the equivalence point of titration. Titration have a large variety of uses, such as
identifying the amount of binding proteins in the blood.2 The purpose of this experiment was to
become familiarize and learn how to properly use a burette, pH probe, and pH indicator to
effectively perform and examine a titration. ... Show more content on Helpwriting.net ...
Ultimately, the purpose of this experiment is to determine the unknown concentration of
hydrochloric acid, by performing a series of titrations between sodium hydroxide and potassium
phthalate in order to standardized the sodium hydroxide to be used to identify the concentration of
the hydrochloric acid.During each of the titrations, sodium hydroxide (NaOH) was used to titrate
potassium hydrogen phthalate (KHP); during each of the trials, sodium hydroxide was gradually
added to the KHP from the burette to the beaker. After each addition of sodium hydroxide, the pH
was recorded in order to form the titration curve, which can be seen in Graphs 1 and

Essay on Micro Unknown Lab Report
| Gram Negative Unknown | Biology 3444–006 | | Lena Wallace | 11/7/2011 |
|
Abstract:
The purpose of this lab was to identify an unknown bacteria culture using differential tests. The
identification of the unknown culture was accomplished by identifying the bacteria based on its
specific metabolic characteristics and morphology. It is suggested that culture 11 is a sample of
Enterobacter aerogenes.
Introduction:
This experiment was centered on metabolic and biochemical testing procedures. The rationale of
performing these tests was to distinguish six different microbes from one another and to compare
how their metabolic and biochemical processes differ from species to species to determine the
unknown sample. ... Show more content on Helpwriting.net ...
If the broth turns yellow, it means that acid was produced and reported as A. If the organism can
break down the amino acids be de–amination and ammonia is produced, this will raise the pH level
turning it pink. This alkaline result was reported as K.
The Methyl Red test is a differential test for bacterial respiration used to differentiate strains of
coliform bacteria capable of performing mixed acid fermentation that will lower the pH despite the
phosphate buffer (http://faculty.deanza.fhda.edu). Mixed acid fermentation is confirmed by using
methyl red as an indicator. It is red ant pH 4.4 and below, yellow at pH 6.2 and above, and orange in
between. Red is a positive result reported as (+), yellow is a negative result reported as (–), and
orange is negative or inconclusive.
The Voges–Proskauer test to detect organisms that are able to ferment glucose, but convert the
products to acetoin and 2,3–butanediol. This is deduced by the addition of Reagent A and Reagent
B, and the observation of the color change thereafter. Reagent A is a solution of –naphthol and
alcohol. Reagent A catalyzes the conversion of acetoin to diacetyl. Diacetyl thens react with
guanidine–containing compounds from the peptone to form a red color in the presence of –naphthol.
Reagent B is a solution of potassium hydroxide and water. It

Ph Buffer Using Cabbage Indicator
Lynne Andrew
NB 1110 / M 5 – 7:50
Lab 1
February 2, 2015
pH and Buffer – Using Red Cabbage Indicator to Measure pH
Introduction This experiment was performed to evaluate the following hypothesis: Red cabbage
indicator can be used as a measure of pH. According to Campbell, et al, in Biology: Concepts and
Connections, red cabbage contains a water–soluble pigment called anthocyanin that changes color
when it is mixed with an acid or a base. The pigment turns red in acidic environments with a pH less
than 7 and the pigment turns bluish–green in alkaline (basic) environments with a pH greater than 7
(2012). The pH indicating property of red cabbage indicator is well accepted in the scientific
community and is a useful standard for ... Show more content on Helpwriting.net ...
Acids were varying shades of red or pink and the bases were varying shades of green. The only
unexpected result was the variability of color change in the pH 12 buffer solution, though this was
attributed to the text, Table 2, stating the pigments are not stable at pH 12 (Pearson, 37). A weakness
of using red cabbage indicator to check the pH of an unknown solution or buffer is the subjectivity
of determining color. What one individual sees as pink. another person would see as light purple.
Color blind individuals would be at a significant disadvantage. Accuracy of pH is another
consideration, since in addition to the variability in shades of color the pH shown by the red cabbage
indicator is more of a ballpark estimate and limited to whole numbers. Using a pH meter, we can get
a significantly more accurate reading that is objective and not dependent on an individual's
interpretation of color or visible hue. In addition to the subjectivity of color, one would need to
ensure a consistent ration of indicator solution to test solution in order to not affect the shade of the
color change. Based on the data received and background information given, it is my opinion that
although red cabbage indicator solution can be used to determine pH levels, it is best used as a more
general indicator of whether a solution is an acid, base or neutral.

Essay On Titration Of Carbonate And Bicarbonate
Determine the total alkalinity of (=[HCO–3 +2[CO2–3]) by preforming a titration with the use of
HCl.
Determine the Bicarbonate content (HCO–3 + OH– → CO2–3 + H2O) by preforming a titration
with the use of NaOH to convert HCO3– to CO2–3.
Calculate the composition of carbonate and bicarbonate in the solution.
Introduction
Acid–base titrations are common laboratory practices that are used to determine the concentration of
either an acid or a base, by neutralizing the substance with a known concentration of an acid or base.
Crude sodium carbonate, also called soda ash, is commonly used as a commercial neutralizing
agent. In this experiment, we will determine the composition of an unknown solid, knowing only
that it contains sodium ... Show more content on Helpwriting.net ...
Using this, the concentration of carbonate can be determined from the total alkalinity (see Results).
Experimental Information
Procedure
At the start of the experiment all the following glassware was cleaned with DI water, and soap; then
dried to remove traces of DI water that remained. The glassware used was a 50mL buret, (3) 150 mL
volumetric flask, a 25mL glass pipet, and a 250mL volumetric flask. 2.5 grams of solid unknown
was added to the 250mL volumetric flask with the use of a funnel, and DI water was filled to the
mark on the 250mL volumetric flask, making sure to rinse the funnel, so the unknown residue
presented on the funnel can rinse down into the flask. After removing the funnel, we diluted to the
mark with DI water, and swirled the flask, until all of the powder was dissolved. This experiment
involved two different titrations. The first titration we observed was for total alkalinity (=[HCO–3
+2[CO2–3]) which was measured by titrating the mixture with 0.1 M HCl to a bromocresol green
end point. After 2L of 0.1M HCl were prepared, and divided among all groups. 25.00–mL aliquot of
unknown solution was pipetted into a 150mL volumetric flask, using bromocresol green as the
indicator, to observe the color change from a tinted light blue to a tinted light green, being the

Titration : Titration Of Hydrochloric Acid
Lab:Titration Analysis of Hydrochloric Acid
Title
In this lab a acid–base indicator phenolphthalein was used to determine endpoint of a reaction
HCl(aq) and KOH(aq). At the end point all of the HCl(aq) would have reacted with KOH(aq), and
the pH becomes 7. The phenolphthalein would changed colours from colourless to pink indication
when enough KOH(aq) was added. The purpose of numerous trials was to use the average volume
of the 3 trials with similar measurements.
Purpose
The purpose of this lab was to use process titration to find concentration of an aqueous solution of
Hcl(aq) , using KOH(aq) as the titrant.
Results
Table 1.0: Information gathered during the trial: The volume of KOH(aq),titrant, used in different
trial.
Trial
1
2 ... Show more content on Helpwriting.net ...
Write a discussion of error summarizing 2 sources of error, why are your results and the other group
different?
The first source of error that caused different results between group was that the groups misread the
colour of the indicator at exactly the equivalence point. The other group could have misjudged light
pink for clear and could've kept pouring the titrant till the color of the indicator changed dark pink
,which will result in a higher number of moles of the solution in your buret than in your flask. The
extra moles of titrant used would give incorrect measurement since the amount KOH used would to
titrate HCl would increase and giving a higher concentration for HCl. To avoid this source of error
groups should used pH meter instead of phenolphthalein.A pH meter giver reading from 1–14 and
doesn't require judgment. The group would know solution is basic when the reading is 7 and they
would stop pouring the titrant. This would avoid extra titrant in the solution and give a more
accurate concentration.
The second source of error that caused different results
Research

The method of titration was discovered in late 1800's by a french pioneer name Francois Antoine
Henri Descroizilles. Titration is a process used to find concentration of an unknown compound. This
process is used in labs to find information need in everyday life.For instance, titration is used during
blood test and urine test to determine the concentration

Titration Lab
Introduction This report, discusses how the concentration of a substance can be found through
titration. A titration is where a substance with a known concentration is tested with a substance that
has an unknown concentration to find that concentration (What Is a Titration). Titrations are very
important in the food industry. It is important to know the concentration of an ingredient or chemical
especially when it comes to nutrition facts and labels for a particular product. Scientists use
titrations to figure out the nutrients that are in food items. Titrations can determine the contents of
fats, carbohydrates and even proteins. This can help people know what is right to put in their bodies
and what is not. This can also prevent false advertisement ... Show more content on Helpwriting.net
...
When measuring out things such as the KHP, baking soda or even the vinegar trying to get the
substance to an exact number is bad. This could make a person measure poorly but making them see
what they want to see on a scale and not actually what they are seeing. Another weakness with
measuring is during this lab, it would have been helpful to clean the scale off and make sure there
were no leftovers on the scale that could make the measurements wrong. With weaknesses always
comes strengths. Some good things in this lab was doing the test at least three times. This allowed
the data to be more accurate than it would be with only one test. Another strength was being safe
while using chemicals that are more dangerous such as HCL. That helped these tests run smoothly.
Titrating can be very important in nutrition. Knowing what is on the market and food that is truthful
on the labels can help make people healthier. In this particular lab, the baking soda and HCL and
baking soda concentrations were off while the vinegar and the NaOH were very close to what they
should have been. This can suggest that if the baking soda and HCL were on the market they could
have been being falsely advertised. Titrations can help prevent these false advertisements from
reaching the buying and selling markets to help people stay healthier and happier. Research

Buffer Works Lab
The purpose of the experiment was to determine how a buffer works and how to use an acid–base
indicator. The way a buffer works was determined by observing the changes in pH of solutions of
different concentrations weak acids and their conjugate bases to determine how a buffer affects the
pH change. The solution of 10 mL of 0.20 M CH3COOH and 10 mL of 0.20 M CH3COONa had
slighter changes in pH than the solution of 10 mL of 0.0020 M CH3COOH and 10 mL of 0.0020 M
CH3COONa. Both of these solutions were buffers, shown because they had slighter changes in pH
than the solutions with only the weak acid or conjugate base and water. The determination of how
buffers work was also tested with observing that the solution of NaC4H3O4 and Na2C4H2O4 had
smaller

Bromothymol Blue Lab Report
The purpose of Experiment 3 was to determine the pKa of a common acid–base indicator and color
dye, bromothymol blue. Acid–base indicators are usually weak acid or base that change color with
various pH levels in a solution, giving one specific color for acidic solutions (HIn) and another color
for basic solutions (In^–). In the case of bromothymol blue, a weak acid, the reagent turns yellow in
the presence of an acidic solution and turns blue in the presence of a basic solution. As the pH of the
solution containing bromothymol blue changes, the equilibrium can either shift towards the
reactants (Hln) or the products (In^–). Since bromothymol blue is a weak acid, it's equilibrium
equation can be written as: Hln=H^++In^–. The solution color will change depending whether there
is more reactant or product present and additionally, whether it is more acidic or basic. Based ...
Dependent on the wavelength of light, absorbance is the extent to which a sample can absorb a light.
The acidic form of bromothymol blue will absorb light at a different wavelength compared to the
basic form due to the varying colors of the solutions. By collecting the various absorbance levels of
bromothymol blue, a spectrum can be created. A spectrum, a plot of absorbance versus wavelength,
can tell what wavelengths is absorbed or transmitted by the solution. Using a spectrum, the
wavelength at which absorbance is the greatest can be found, which not only gives information
about the electronic structure of compound but also at this point, the absorbance is the highest and
the rate of change of absorbance and wavelength will have the smallest difference. Using maximum
wavelength also assists in the Beer Law equation, A_λ=ε_λ b C. Beer's law is useful in this
experiment because it proves that absorbance is directly proportional to the concentration of the
solution of the

Titration Of An Unknown Solution
A titration is a method to determine the concentration of an unknown solution by using the known
concentration of another solution. An analyte is the concentration of an unknown solution . A titrant
is the concentration of a known solution. The glassware needed to perform a titration are a buret, a
flask, and an indicator of pH meter. The buret sends the second reactant to the flask. An indicator
detects the endpoint of this reaction. Standardization is the process in which you determine the
concentration of the titrant before performing the titration. One would need to make a standard
solution to be precise, and make sure the titration experiment is being done correct. The equivalence
point is point in the titration when the quantity of titrant is the right amount for the reaction with the
analyte. ... Show more content on Helpwriting.net ...
You prepare a standard solution by using the M1V1=M2V2 formula, and putting the information to
solve the equation. An indicator is going to have a reaction with hydroxide ions or hydrogen ions to
determine whether the substance is a base or acid. The role of an indicator in a titration is to
determine how many oxygen or hydroxide ions are in a solution. The laboratory method that is used
to titrate an unknown strong acid solution is a titration. When you drop NaOH ions the OH ions
unite with H ions creating water which leave less H ions in the solution making the solution less
acidic. The more NaOH ions you add the solution will eventually change color due to the indicator.
The data that should be collected during the titration in order to calculate the concentration of HCl
should be the number of moles, the volume of the solution, and the amount dropped to make the
solution less acidic. You calculate the molarity/ concentration of the unknown HCl solution by using
the formula

Sulphuric Acid Lab
From this lab experiment, I can conclude that the red cabbage solution is an effective indicator for
the acidic, basic and neutral chemical compounds. I learned that the universal indicator is also a
good solution for the three types of compounds. The colours are different depending on what
substance you are testing. The colours that we discovered in the pH scale are pink, red or orange. As
for bases the colour was either light or dark green sometimes yellow. The colours for neutral, were
violet or purple.In real life we are exposed to acids and bases everyday. For example, citric acid is in
lots of citrus foods such as lemons, oranges and grapefruits. It is also added to foods for flavouring,
non perishable, and cleaning supply. Citric acid creates a taste that is sweet and sour. ... Show more
content on Helpwriting.net ...
There is also acids in your stomach.The acid in your stomach helps digest food which in large
quantities causes indigestion to occur. If indigestion does occur, it is necessary to neutralize it with a
base. Nature also produces acids that are toxic to humans one that is known as sulphuric acid.
Sulphuric acid is extremely harmful if you are directly exposed to it. However it is very useful in
real life. For example, in car batteries, used in plant fertilizers. On the contrary, It is very dangerous
to the environment. There are many acids in the human body and many foods that we eat in our
daily lives. Bases on the other hand, are used also in our daily lives. For instance, baking soda is
used in baking, putting out small fires, cleaning and health purposes as well. It is used in baking
because it works as a rising

The Effect Of Temperature And Reactant Concentration On...
This experiment aimed to investigate the relationship between temperature and reactant
concentration on the rate of reaction for the hydrolysis of tert–Butyl Chloride, and to determine the
validity of the proposed mechanism for the reaction. It was hypothesised that measuring the kinetics
of this unimolecular substitution reaction would demonstrate the reaction rate for the hydrolysis of
tert–Butyl Chloride utilising acetone as the solvent which should increase with both its increased
concentration and temperature, to produce the product tert–Butyl alcohol.
When the solution of tert–butyl chloride in acetone is added to water in the presence of a base and a
universal indicator, its reaction to form tert–butyl alcohol is indicated by dramatic color change.
Bromothymol blue is an acid–base indicator which appears blue in an alkaline medium and yellow
in an acidic solution (Artxy, 2011). The solvolysis of tert–butyl chloride is revealed by the indicator
change from blue to yellow as hydrogen halide is produced during the reaction (Mostafa, 2009). The
solution is initially blue because of its Sodium Hydroxide (NaOH) content (alkaline), and the colour
change results as aqueous chlorine removes a proton from the transition state, while the generated
hydrogen ions neutralise the hydroxide ions of the NaOH, causing the change in the pH of the
system (Riley, 1977). This qualitatively determines that the rate of reaction is dependent on the
concentration of tert–butyl chloride.

Sodium Formula Lab Report
The Relative Formula Mass of an Unknown Acid
Table of contents
1.1 Aim of the experiment 2
1.2 Introduction 2 1.3 Equipments and apparatus 2
1.4 Safety precautions 2
2.1 Procedure 3
2.2 Apparatus setup 3
2.3 Analysis 4
3.1 Implementing ... Show more content on Helpwriting.net ...
There are two types of acids called organic acids and mineral acids. Organic acids, such as
methanoic acid, citric acid or latic acid, are obtained from plant and animal sources. From the other
side, mineral acids (hydrochloric acid, nitric acid or sulphuric acid) are made from minerals. They
are much more reactive with bases than organic acids.
1.3 Equipments and apparatus
1. burette
2. 25 cm3 pipette
3. pipette filler
4. stand and clamp
5. funnel
6. 500 cm3 beaker

7. 250 cm3 conical flask
8. phenolphthalein indicator
9. wash bottle/deionised water
10. 250 cm3 of the unknown acid solution
11. 250 cm3 of 0.100 M sodium hydroxide solution
12. A sheet of paper to record the results of the titration
13. A white tile
1.4 Safety precautions
You must be careful throughout preparing the solution and the titration process. Some chemicals can
pose a risk. In this case an alkali (sodium hydroxide) is corrosive chemical. In contact with skin it
will cause burn and damage eyes. From the label of the unknown acid you can deduce that it is a
toxic substance which is poisonous and can kill you. The care must be also taken while using
phenolphthalein indicator. Its pH value is 9.5 which mean it is an alkali. This chemical also may
cause damage to your body. During

6.03 Synthesis Lab Report
This lab could have contained errors. The errors could have happened when performing the lab.
Some of the possible errors in this lab are:
There might have been some mistakes made while transferring the ingredients from the beaker and
the funnel to the flask and the burret.
The antacid tablets were not crushed properly, resulting in big crumbs of the tablet which will affect
the dissolving process of the lab.
There might have been more KOH solution added to the flask resulting in the observations to be
wrong.
The mixture might have contained more or less than 5 drops of bromophenol blue, which might
have resulted in the indication of the lab.
Not enough attention paid when the solution was changing colours.
The buret might have been leaky resulting in more KOH dropped in the erlenmeyer flask.
Conclusion: ... Show more content on Helpwriting.net ...
The lab checked for neutralization and check if it did not neutralize too much or too little. There
were two commonly sold brands examined in this lab which were the Tums and Rolaids. The
crushed tablets were dissolved in 0.10 M HCl with a pH indicator bromophenol blue and a solution
of KOH was added to it in order to neutralize the solution. The solution turned light blue when it
was neutralized. Both the tablets were neutralized and titrated in the same way. From the
observations above; Rolaids was better because it had better neutralizing ability per each dollar
spent than the Tums. As the Rolaids were 4.07g/$ and the Tums were 4.01g/$ as seen from the
observations above. So, the better buy is the Rolaids out of the two as the neutralization ability per
dollar spent in the Rolaids is better than the

Acid-Base Titration Lab Report
Mariam Sy May 8, 2014
Acid– Base Titration Lab Write–up
Introduction:
Titration is the process of adding measured volumes of a base or acid with a known concentration to
an acid or base with an unknown concentration in order to determine the unknown concentration.
Volume measurements play an important role in titration. It involves measuring the exact volume of
a solution with a known concentration that will react with a measured volume of a solution that has
an unknown concentration. The solution that has a known concentration is called a standard
solution. Acid– base titration is based on neutralization that occurs in the reaction. If a base is added
to an acid until the acid is neutralized, then the moles of base and the moles of acid will be equal. In
other words, the moles of H+ ions must equal the number of moles of OH– ions. The following
equation can be used to calculate the unknown molarity of an acidic or basic solution: (Molarity of
the acid) * (Volume of the acid) = (Molarity of the Base) * (Volume of the Base) or MaVa = MbVb.
Equivalence point is when there is enough of the standard solution to neutralize the unknown
solution.
The endpoint is when the indicator changes color. The difference between the equivalence point and
the endpoint is that the equivalence point is when the pH of the solution is 7 which means that it is
neutral. However, the endpoint is when the indicator turns either white which shows that the
solution is acidic or pink which

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