Notes On A Macro Porous Strong Base Anion Exchange Resin...

Notes On A Macro Porous Strong Base Anion Exchange Resin...
3.0 MATERIALS AND METHODS
3.1 Materials
3.1.2 DOWEX TAN 1
DOWEX TAN 1 is a macro porous strong base anion exchange resin with quaternary amine
functionally designed for the removal of large natural organic compounds (NOM) from drinking
water to reduce color and THM precursors. The resin was obtained from DOW chemicals. The
resins are opaque white beads with particle size ranging from 0.3 to 1.2 mm and total exchange
capacity is greater than 0.7meq/ml.
3.1.2 IRA–67
Weak base anion exchanger IRA67 was obtained from (company name)...............................
...............................................................................................................
3.1.3 Chemicals, Glass wares and Plastic wares
Table .... Contains lists out some silent details of chemicals, reagents and other materials used in for
the study.
Table .... Different chemicals, reagents, glass wares and plastic wares used in study
S.No. Chemical/Reagent/Glassware/Plasticware Sources
1.
2.
3.
4.
5.
6.
3.1.4 Instruments used: The following instruments are used for the studies.
3.1.4.1 Spectrophotometer: A double beam UV–Visible/NIR spectrophotometer modal DR–5000
from Hach (USA) was used for determination of phosphate in aqueous samples estimation.
3.1.4.2 Deionized water unit: De–ionized water used in the study was obtained from MilliQ Water
Purification System (Elix 3 UV Water Purification System, Millipore) was used for distilled water.
3.1.4.3 Shaker: A Platform shaker from Sara Instruments (Roorkee) was used in the study in order to
create turbulence and also to achieve
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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

Why We Absorb Bath Bombs
Bubbling Bath Bombs
Hypothesis
What makes bath bombs fizz and bubble? Will a bath bomb containing lime juice rather than citric
acid dissolve faster? I think there is a chemical reaction within the bath bomb that makes it fizz, but
I am not sure what things are reacting. I also think that if I substitute lime juice for citric acid in one
half of the bath bomb, the half with citric acid will dissolve quicker. This is because it is pure citric
acid, unlike lime juice which has other things as well as citric acid in it.
Research
Bath bombs are composed of several ingredients that are molded into a shape. They begin to fizz
and dissolve once they touch water. Bath bombs come in a large variety of different colors, scents,
shapes, and sizes. ... Show more content on Helpwriting.net ...
water, 2 tsp. coconut oil, about 15 drops essential oil, and a few drops of food coloring (depending
on the color I wanted), ¼ cup Epsom salt, 5 bowls, and molds to put the mixture into. To create the
different halves, I took half of each ingredient into separate bowls and added either ¼ cup lime juice
or ¼ cup citric acid. First, I combined the baking soda, corn starch, and Epsom salt into a bowl. If I
was using the citric acid, I combined that into the same bowl. Next, I combined my water, coconut
oil, essential oil (optional), and food coloring (optional) into a different bowl. If I was using the lime
juice instead of the citric acid, I would combine it into this bowl. It is very important you keep your
wet and dry ingredients separate. Then, I slowly put a few drops of the wet mixture into the dry
mixture and stirred. You want to put a few drops, then stir; add a few more, and stir again. You must
do this step slowly to prevent any reactions happening between the citric acid and the baking soda.
During this step, I discovered that the side with lime juice was much moister than the other side
with citric acid. This made it difficult to mold the halves together because a slight reaction was
occurring when I put them together. Next, I put the different mixtures into half a mold and stuck the
halves together into the freezer for 2 hours. Then, I took the bath bomb and put it into a bowl full of
warm water. Finally, I watched the reaction and recorded my

Titration Investigation Essay examples
Titration Investigation
Aim:
The aim of my investigation is to determine the solubility of calcium Hydroxide solution with the
aid of the titration process.
Titration can be defined as the method of determining the concentration of a substance in solution
by adding to it a standard reagent of known concentration in carefully measured amounts until a
reaction of definite and known proportion is completed, as shown by a color change or by electrical
measurement, and then calculating the unknown concentration.
An example could be, a given volume of a solution of unknown acidity may be titrated with a base
of known concentration until complete neutralization has occurred. This point is ... Show more
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From the pH at the equivalence point, the dissociation constant of the acidic or basic group can be
determined (see chemical equilibrium). If a compound contains several different acidic or basic
groups, the titration curve will show several sigmoid–shaped curves like steps and the dissociation
constant of each group can be obtained from the pH at its corresponding equivalence point.
I have now explained the basis of the Titration methodology; I will now have to choose the
appropriate compounds in order to make sure that the experiment is carried out in the appropriate
manner. I will now display a table containing the different compunds for my availability:
Strong acid
Weak acid
Strong alkali
Weak alkali
Hydrochloric acid
Ethanoic acid

Sodium Hydroxide
Ammonia solution
Nitric acid
Ethandioic acid
Potassium Hydroxide
Sodium Catbonate
Sulphuric acid
Calcium Hydroxide
Sodium Hydrogen Carbonate
This table will aid us into the right choice of indicator. The reason for doing so is that some aspects
of the Titration process have to be very accurate. Depending upon the strength of an alkali and acid
the right indicator is chosen:
* A Titration between a strong acid and a weak alkali requires a methyl orange

Weak Acid Lab Report
The statement, the stronger acid has a higher pH than the weak acid , is proven to be false. pH is a
measurement of the concentrations of hydrogen and hydroxide ions. To defined the pH we used the
formula –log10[H+]. With this example H+= 1.0e^–2 equal the pH of 2 and H+=1.0e^–4 equal the
pH of 4, we can see that the lower the pH values the concentration of hydrogen ions is higher when
the pH goes up compare to when H+ decrease. HCl is a strong acid in which it completely ionize in
water and become H+. when HCl mix with water the pH is lower because the concentration of the
H+ increase. A weak acid like CH3COOH ionize partially in water and get a less concentration of
the H+ ions.
In an aqueous solution, the strong acid reacts with magnesium faster than the weak acid. The
equation for magnesium is 2H+ +Mg –––> Mg2+ H2 .When the magnesium react with the strong
acid the magnesium become completely ionize that you can tell by the bubble. Since the stronger
acid react much faster the bubble form showing that there was more hydrogen ions in the solution.
On the other hand the weaker acid take longer to react because it concentration is lower than the
strong acid. ... Show more content on Helpwriting.net ...
The equation of the two reaction we tested is CH3COOH + NaHCO3 –––> CH3COONa + H2O +
CO2 and NaHCO3 + HCl –––> NaCl + H2O + CO2. In the weak reaction, acetic acid and an acetate
ion is input to the product. The more hydrogen ion and acetate ion added to the product the
concentration of the carbon dioxide increased due to the reaction of the two solution. on the other
hand when strong acid such as HCl is mix with baking soda, less carbon dioxide gas is produce
because NaCl ionized in the

Acid Base Balance Case Study
Maintenance of acid and based balance in the body is essential for normal function of biological
processes, mainly because of the dependence of pH level for enzyme function. The body
concentration of acids and bases is controlled so that the pH of extracellular body fluids is
maintained within the range of 7.35 to 7.45. The body maintain this balance by a mechanism that
generate buffer and eliminate acids and bases. A base is an ion or molecule that can accept or
combine with a hydrogen ion and an acid is a molecule that can release a hydrogen. (Grossman,
Port, 2014). Acids and bases exist as a buffer system. For example, a mixture of a weak acid can
reversibly become base or a mixture of a weak base can reversibly become acid. There are two type
of acid–base imbalance; metabolic and respiratory.
Metabolic imbalance is a disorder that produce an alteration in the plasma bicarbonate concentration
from the addition to or the loss from the extracellular fluid of nonvolatile acid or alkali. A reduction
in pH because of a decrease in bicarbonate is called metabolic alkalosis. Respiratory imbalance
involves an alteration in partial pressure of carbon dioxide due to an increase or decrease in alveolar
ventilation. Respiratory acidosis is the result of a decrease in pH, ... Show more content on
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One hot afternoon in a small market community, she grabbed some fruit juice from a street vendor.
Several hours later, she developed abdominal cramping and diarrhea. The diarrhea became so severe
that she missed three days of the tour and stayed in her hotel room. By the end of her illness, she felt
weak and tired. Her head ached, but the mild fever had disappeared, and she was able to join her
new friends for the rest of the tour. Based on the information collected, and the symptoms displayed,
Shauna is experiencing metabolic

Henderson Hasselbalch Lab Report
In the first experiment my partner and I selected to produce a buffer that contained 35mL of .1M
sodium acetate with 10 mL of .2M acetic acid with the excepted pH of the solution to be 5. We used
C1V1=C2V2 to first calculate the theoretical concentration of both the weak acid and the weak base
in the buffer solution. Then using the theoretical concentration and the Henderson– Hasselbalch
equation we were able to calculate the excepted pH. After calculating the pH we then measured the
experimental pH of the produced buffer and found it to be 4.9. This showcased that there was a
difference of 2% between the theoretical pH and the experimental pH. We further measured the
buffering capacity of three different samples one being the buffer that ... Show more content on
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TLC showcased lysine being the unknown amino acid whereas titration showcased glycine as being
the unknown acid. In my opinion TLC is not accurate because as witnessed on the TLC plate there
are signs of contamination. Though titration may involve many tedious steps I believe that titration
has provided me with accurate answer. Some errors that may have occurred in the lab are not
switching the micropipette tip between the spotting of the amino acids. Also not wiping down the
pH meter correctly during measurement could have influenced the

Decipher Whether Acid Is Friend Or Foe?
The main purpose of this experiment is to decipher whether acid is friend or foe? Acid is a particular
substance with chemical properties including; turning litmus red, corroding metals, and neutralizing
alkalis (bases).
In the late 1800s, the Swedish scientist Svante Arrhenius suggested that acids are chemical
compounds that, when dissolved in water, give a solution with a hydrogen ion activity greater then
water, a pH less than 7.0. A base however is any compound that, when dissolved in water, gives a
solution with a hydrogen ion activity lower than that of water, a pH higher than 7.0. If mixed
together, the H ion and the OH ion would combine to then make H2O. This is called neutralization.
The neutralization reaction of an acid and a base will always result in water and a salt. Bases have a
slippery feel on fingers and taste bitter. They change litmus paper blue. Where as acids taste sour
and create a stinging feeling on the mucous membranes. The difference between acids and bases are
that acids are compounds that donate a hydrogen ion (H+) to another compound known as a base. ...
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When leaves of a plant are exposed to acid rain, the outer waxy layer of tissue is disintegrated. The
outer layer of tissue protects the plant from drying out, resulting in the disintegration of chloroplasts
that drive photosynthesis. When humans burn fossil fuels, sulfur dioxide (SO2) and nitrogen oxides
(NOx) are released into the atmosphere. These chemical gases react with water, oxygen, and other
substances to form mild solutions of sulfuric and nitric acid. This then creates acid

Explain Why The Ions That Are Responsible For A Strong Base
The ions that are responsible for making a solution of a base or an acid is H+ or a proton. The pH
scale measures the acidity or alkalinity of a solution. On the pH scale there are numbers that indicate
how strong or weak the acid or the base is. On the pH scale the numbers range from 0–14. 0 – 2
stands for a strong acidic, 3 – 5 for a weak acidic, 6 – 8 means the solution is neutral, 9 – 11 for a
weak base, and 12 – 14 for a strong base. There are three theories that are used to define a base and
an acid. The first theory is the " The Arrhenius Theory " this theory says an acid produces hydrogen
ions, H+ in water solution and a base produces hydroxide ions, OH− in water solution. The second
theory is " The Bronsted – Lowry Theory ". This

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 Lab
The purpose of a titration is to discover the concentration of the unknown acid or base. In this case,
the experiment uses a strong base to titrate the unknown acid. Once the titration is complete, the
data is plotted to create a graph that shows the equivalence point as well as the change in pH with
each volumetric addition of NaOH. The equivalence point in the graph is the point where the moles
of acid equal the moles of base added, which can be expressed as the equation MaVa = MbVb. On
any titration graph involving a monoprotic acid and a strong base, the equivalence point is the center
of the steepest part of the graph, also known as the inflection point. This point will be at pH 7 or
above, since the titrant is a strong base and the unknown ... Show more content on Helpwriting.net
...
The pKa is –log[Ka], and Ka is the equilibrium constant of a reaction. If there is a weak acid, it will
have a strong conjugate base which will bond with a hydronium ion, causing the reaction to move
towards the reactants which results in a lower Ka (or higher pKa). Therefore, the magnitude of the
pKa has an effect on the equivalence point. A higher pKa results in a higher pH of the solution. The
pKa also has several other implications. As the pKa increases, the initial pH increases as well. The
initial slope of the graph is almost horizontal for a smaller pKa; however, as the pKa increases, the
slope at the initial values increases as well. With further analysis, one can notice that the pH
increases steadily between 5 and 20ml for all eight graphs but are placed at different pHs. This
steady increase only lasts until the one drop of the titrant causes a jump from pHs. The range of the
jump from one pH to another decreses as the pKa of a reaction increases. In other words, the range
where the equivalence point occurs decreases. Despite the change in this range, the pKa (or Ka)
does not affect the equivalence point volume since the same amount of acid was used in each
experiment, which in turn means the same volume amount of NaOH is used as well. The changes in
the pKa display changes in the equivalence point, pH, and slopes of the curve, all which ultimately

Graded Assignment: Lab Report
Name: Date:
Graded Assignment
Lab Report
Answer each question, using complete sentences. When you have finished, submit this assignment
to your teacher by the due date for full credit.
(8 points)
Score
1. List the values for T–alkalinity for Sample A and Sample B.
List the ppm value for sodium carbonate for Sample A and Sample B.
Answer:
I am unable to answer this question because I don't think I have enough information. This is asking
for exact values and I don't have the data to answer it. I maybe overlooking the answer but I am
unable to figure this out.
(8 points)
Score
2. Write the equation for the dissolution of sodium carbonate in water as found in your laboratory
guide.
When sodium carbonate is dissolved in water, it doesn't

Describe The Relationship Between Acid And Carbonic Acid
The acid–balance must be regulated with a range of 7.35 and 7.45 in order for the body to function
normally. A pH of below 7.35 is considered acidic and a pH of above 7.45 is considered alkaline or
basic. Body acids exist in two forms; volatile and nonvolatile acids. Volatile acids can be eliminated
as CO2, usually known as carbonic acid, which is a weak acid. Nonvolatile acids can be eliminated
by the kidneys, example are sulfuric and phosphoric. These acids are strong compared to volatile
acids.
When there are changes in pH (can be an increase in hydrogen ion or decrease) there are different
buffer systems that can help to regulate the pH, such as; the carbonic acid–bicarbonate buffer,
protein buffer and renal buffer. Buffers absorb the excess hydrogen ion or hydroxyl ion and prevent
a ... Show more content on Helpwriting.net ...
The carbonic acid–bicarbonate buffer is a major extracellular buffer, that operates in both the lungs
and kidneys. The lungs acts as a second defense responding quickly by decreasing the amount of
carbonic acid by blowing off carbon dioxide and leaving water. The kidneys acts as a third defense
talking a little longer to respond (hours to days versus seconds to minutes with the lungs). The
kidneys reabsorb bicarbonate or regenerate bicarbonate from carbon dioxide and water. These two
systems work very effectively together because the lungs can adjust acid concentration rapidly by
ventilation and bicarbonate is easily absorbed or regenerated by kidneys tubules, although more
slowly. The way the renal and respiratory systems adjust to primary changes in pH are known as
compensation. The respiratory system compensates for changes in pH by increasing or decreasing
the concentration of carbon dioxide by changing ventilation. The renal system compensates by
producing more acidic or more alkaline urine. The protein buffer system is both extracellular and
intracellular,

Nucleic Acid Investigation
The purpose of the introductory activity was to analyze the pH of a mixture of a strong base and
weak acid. The purpose of the guided–inquiry lab was to analyze the concentration of sodium
carbonate by titrating the substance using a nitic acid solution.
Introductory Activity
5 mL of both 0.2 M ammonia and 0.1 M acetic acid were placed in separate test tubes and their pH
was determined with pH paper. A mixture was created by pouring both together and its final pH was
recorded. The strength of the acid and base was determined and whether the two had equal
concentration. Each indicator was researched (its colors when it's acidic/basic and its pH transition
range) and phenolphthalein was deemed suitable for this experiment. 5 mL of acetic acid was
poured into a test tube and 1–2 drops of phenolphthalein were added. The initial color was recorded.
10 mL of ammonia was obtained in a graduated cylinder and using the graduated pipet, the base was
added to the acid in 1 mL increments. Upon reaching the equivalence point, the indicator color and
the amount of base required to obtain this point were recorded. The relative concentrations of the
acid and base were then estimated.
Guided–Inquiry Design ... Show more content on Helpwriting.net ...
The indicator methyl red was deemed appropriate. A 60 mL Poorman's buret was placed on a
support stand above a beaker with a magnetic stirrer. The sides of the beaker and flask were rinsed
with water. 100 mL of nitric acid was collected and placed in the beaker below the buret.
Approximately 3 drops of methyl red indicator were added. After being rinsed with water and
sodium carbonate, the buret was filled with 60 mL of nitric acid. The beaker was placed 2 cm under
the buret. Then the sodium carbonate was titrated until the methyl red changed from red to yellow.
The final buret reading was recorded to determine the final volume of the base. The titration data
was used to graph a titration

Antacid Drops
The Effect of Antacid Brand on the Number of Drops It Takes to Neutralize a Solution of HCl
Problem: What brand of antacid requires the fewest number of drops to neutralize a solution of
HCl?
Hypothesis: If the number of drops of antacid required to neutralize a solution of HCl increases,
then the effectiveness of the antacid decreases.
Materials:
HCl
Milk of Magnesia
Mylanta
Care One Liquid Antacid
Universal Indicator with color chart
Pipette
Graduated Cylinder
Beaker
3 Test Tubes labeled A, B, C
Water
Procedures:
Fill the graduated cylinder with 10 ml of water and pour into the control beaker.
Measure and fill the graduated cylinder with 10 ml of HCl, and transfer to the test tube labeled A.
Repeat step 2 for test tube labeled B and C.
Add 3 drops of universal indicator to each of the test tube A, B and C.
Add as many drops of Milk of Magnesia as you need to test tube A, swirling around between drops,
until the color is neutral by comparing it to the control test tube of water.
Make sure to stop at the ... Show more content on Helpwriting.net ...
By comparison, the Mylanta had reached the 32 drops limit and failed to fully neutralize the same
amount of HCl solution. Since each H+ ion in HCl solution must be neutralized by an OH– ion from
the antacid to form H2O through neutralization reaction, therefore this is a clear evidence that the
original assumption of the more drops of antacid were needed to neutralize the acid, the less
effective the antacid is correct since it must contain less OH– ion. Therefore, the hypothesis was

proven correct.
Antacids are weak bases used to neutralize our stomach gastric acid, mainly composed of
hydrochloric acid or HCl, through neutralization reaction. Neutralization reaction is when the
reactants, acid and base, reacting with each other and produce a products of salt and water.
Base + Acid ––> Salt +

Acid-Base Titration Lab
The purpose of this lab is to determine a weak acid and its acid dissociation constant (Ka) through a
process of an acid–base titration. A sample of the unknown weak acid was made into a 100 mL
solution, where 20 mL was take out for titration; phenolphthalein was added in as the indicator.
NaOH, as the titrant, is dripped into the weak acid solution until a slight change in coloration (from
clear to pink) was noted. At this point in time, the titrated solution is diluted with 20 mL more of the
weak acid; the pH is then measured by a pH probe. This process was done a second time for
comparative accuracy. Throughout this lab, there were a few concepts that were used and applied.
This experiment revolved around a titration: the addition ... Show more content on Helpwriting.net
...
The solid given probably was not a pure Hydrogen sulfite ion based compound, therefore bringing
to question the possibility of other compounds inadvertently reacting in the titration. When the acid
was dissolved, some of the impurities might have followed suit and dissipated. If that were so, the
impurities could also take effect on the reaction when the titrant, NaOH, was introduced to the
solution. If the impurity was acidic in nature, it would require the solution to take in more titrant
than necessary for a indicator color change. This would also make the pH (and concurrently the
pKa) at midpoint slightly lower than actuality. Because there is a greater presence of acid, the pH
would be lower, and a lower pH, would mean a lower pKa. Consequently, the acid dissociation
constant would be larger than the accurate value. If the impurity was basic in nature, it would cause
the inverse: it would take less NaOH to titrate the solution until the indicator changes color. A more
basic solution would also make the pH of the solution at midpoint, slightly larger than the needed
value. Ergo, the Ka value would be smaller than that of HSO3–. Another lab error would be from
the usage of phenolphthalein: the indicator's color change is not an instant occurrence. As a result,
one would stop the release of the titrant a little bit of time after the reaction has reached the
equivalence point. This, in turn would mean an

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

What Do Acids And Bases Of Varying Ph Levels Have On The...
What effect do acids and bases of varying PH levels have on the efficiency of catalase? Catalysts are
an extremely important part of the experiment, but to understand catalyst you first must understand
Activation energy. Activation Energy is "the minimum amount of energy that is required to activate
atoms or molecules to a condition in which they can undergo chemical transformation or physical
transport." (Encyclopedia Britannica, "activation energy | chemistry"). A Catalyst is "is a substance
which speeds up a reaction, but is chemically unchanged at the end of the reaction. When the
reaction has finished, you would have exactly the same mass of catalyst as you had at the
beginning." A catalyst provides an "alternate route" for a reaction, one which has lower activation
energy, there for speeding up the reaction by requiring the reaction to need less energy to begin, but
only in specific conditions will they work to their full potential. (Clark, "The effect of catalysts on
rates of reaction") An enzyme is a "catalyst in living organisms, regulating the rate at which
chemical reactions proceed without it being altered in the process". Catalysts work optimally in
certain PHs, and can be altered when in temperatures and PH levels that are different then what they
are used to (http://www.britannica.com/science/enzyme). Acids and bases are both materials that can
inhibit the efficiency of a catalyst in a reaction. Materials can be considered acids or bases
depending on their

Nahco3 And Calorimetry
"In a chemical reaction, atoms rearrange and bond together in different ways to create new
substances". Concentration is involved with the amount of acid added to a certain amount of water.
Strength is used in acids to determine if they are weak or strong. A base can be defined as a
substance that can accept a hydrogen ion from another substance.An acid can be defined as a
substance that can donate a hydrogen ion, that is a proton, to another substance. Acids react with
most metals, and the most common way to identify an acid is color change. One safe way to test for
an acid is to place a few drops of solution on a compound that contains carbonate
When given similar looking substances, they can be distinguished by their chemical reactions.
Baking soda can be noticed when it is contained in acidic ingredients and starts to bubble. Its
chemical formula is NaHCO3. Baking powder is a combination of baking soda, calcium acid
phosphate (a weak acid), and cornstarch; used in bing to generate bubbles. Its chemical formula is
NaHCO3. When baking soda is reacted with red cabbage indicator, a color change usually occurs
from pink to green. The chemical equation between vinegar and baking soda is NaHCO3(s) +
CH3COOH(l) → CO2(g) + H2O(l) + Na+(aq) + CH3COO–(aq). ... Show more content on
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Its chemical formula is KC4H5O6. When water is dropped into cream of tartar there is no reaction.
But, when vinegar is dropped into it, it transforms into a cleaning agent. Cream of tartar is usually
used for cooking, but when mixed with vinegar, as stated previously, it becomes a cleaning agent.
Red cabbage indicator added to cream of tartar, results in a color change to pink. Red cabbage
indicator is commonly used to distinguish between acids and bases. Because cream of tartar is an
acid, it turns

Acid-Base Results
The purpose of this experiment was to test acid–base solutions to determine the absorbance intake
they had do to their different pH levels. To do this, four similar samples were recorded with a
different amount of NaOH added to each one, which would change the pH level from acidic to
basic. Acidic solutions take in less absorbance, while basic solutions will have the most absorbance,
as well as higher Ka and pKa values. The acidic solutions would have negative absorbance from
100% or higher transmittance, while the basic solutions would have low transmittance %, but very
high absorbance levels.
Introduction Acids–base indicators are organic weak acids or bases that change colors when they are
neutralized. A way for the color to be change ... Show more content on Helpwriting.net ...
However, the higher the transmittance percentage, the lower the absorbance for that solution will be.
The highest and lowest absorbance for each solution seems to be at 610nm wavelength. It should
also be noted that the pH levels in the four solutions are a big factor when finding the absorbance
and transmittance. The lower the pH, the lower the absorbance, but the higher the pH, the higher the
absorbance. It can be guessed that acid molecules do not take in light absorbance as well as base
molecules do. The calculations in table 1 help generate the graph shown in figure 4, by taking the y–
axis of the absorbance, and comparing the x–axis of the wavelength, to show comparison of the four
different pH levels. For table 2, the calculations found from the graph are put into the correct
category to represent the results found. The highlighted part of the graph shows the most important
info that helps solve for the other boxes. To find the pKa for samples 2 and 3, simply take the pH of
that sample and subtract it by the log of the sample absorbance, plus minimum absorbance over
maximum absorbance minus the sample absorbance. Sample 2 example: 7.1–LOG
((1.0554+0.0135)/(1.8085–1.0554))=6.95. To find the Ka of the sample, simply grab the answer for
pKa and plug it into the power of 10 to the negative. Ex: 10–6.95 = 1.13E–07. Finally, to

Determination Of An Unknown Concentration Of Vinegar Essay
An investigation was conducted to determine an unknown concentration of ethanoic acid in various
types of vinegar. Vinegar is a liquid that consists of around 4–8% ethanoic acid (CH3OOH), water
and other trace chemicals (Wikipedia, 2018). The vinegars used in this experiment were wine, white
wine and apple cider and they have 6%, 5% and 4% ethanoic acid concentrations respectively
(University of Sydney, n.d). Vinegar is produced by the fermentation of ethanol by acetic acid
bacteria. An acid is considered strong if they completely ionise in water to produce hydrogen ions
and have a low pH, an example of a strong acid is hydrochloric acid (HCl). Weak acids, however, do
not fully ionise and instead form an equilibrium mixture. Ethanoic acid ... Show more content on
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It occurs when enough base is added for a neutralisation reaction to occur. The equivalence point
between a weak acid and a strong base is pH 8.72. It must be attained precisely to produce accurate
results. This is done by slowly adding the titrant to the analyte. The end point of the experiment
refers to the point at which the indicator changes colour because of an indicator. The indicator
phenolphthalein has a pH range of 8.2 to 10.0 and is used to determine the endpoint as it shows
when enough of the base has been added to fully react with the acid. It remains colourless in an acid
and when neutral, however, when the solution becomes basic, it turns pink. When it turns a pale
pink, the endpoint has been reached and the amount of base can be determined, and the
concentration of acid can be found. However, if the solution is overly titrated, it will turn a bright
pink. This means that the results are no longer precise nor accurate. When the endpoint has been
reached, the amount of base used can be determined, and thus the concentration of the acid can be
found using

Tartaric Acid Lab Report
The experimental average 〖pk〗_a for the unknown weak acid was 4.075. The experimental
average K_a of the unknown weak acid was 8.424×〖10〗^(–5). The unknown acid was found to
be tartaric acid. Tartaric acid has a pK_a value of 2.89 and a K_a value of 1.288×〖10〗^(–3). The
experimental pK_a value had a percentage error of 41.0% when compared to the theoretical value of
pK_a of tartaric acid(equation 8). The experimental K_a value had a percentage error of 93.46%
when compared to the theoretical K_a of tartaric acid(equation 9). These large percentage errors
shows that the experimental values were not accurate. As more NaOH was added to the solution
containing tartaric acid, more of the conjugate base was formed and the pH of the solution will ...
A mass of the unknown acid was weighed out and dissolved in water. The molality of the solution
was calculated. This solution was then titrated using small amounts of the strong acid NaOH. As
more NaOH was added to the solution the more the pH increased. The volume added to solution
along with the new pH was using in the Henderson–Hasselbalch

Titration Lab
Titration is a technique that is used to determine and analyze the concentration of a substance. It is
based off of mole ratios between the two substances taking part in the lab. Burets are used in the
titration of substances, which are large glass tubes with a valve attached to the bottom to allow the
specially measured amount of substance into another. The amount of each substance must be very
precise and be recorded properly. The analysis of these reactions are usually simplified to a 1:1
ratio, just as this lab was. Three of the most commonly tested reactions include an acid–base
reaction, an oxidation reaction, and a water analysis. An acid–base reaction consists of finding the
amount of the acid or the base when mixed together, which is what the first part of this lab ... Show
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The process of titration is the adding of a base drop by drop into a flask of (in this case) 10.0 ml of
acid along with three drops of phenolphthalein. The solution must be swirled continuously
throughout the process until equilibrium is reached which will show a different color of solution
than the beginning. Phenolphthalein is an acid–base indicator commonly used in titrations. Its
molecular formula is C20H14O4 and it is a weak acid that can lose its H+ ions. In titrations, it turns
the solutions pink when the base is added. The first part of the lab is a forward titration, which was
explained above. The second part however, is what is called a back titration. A back titration is the
reaction of an unknown substance with a carefully measured known chemical. The known substance
is then analyzed to see exactly how much remains. Through stoichiometry, we can determine the
amount of the known substance that the unknown substance used during titration. The molecular
formula for Vitamin C, or ascorbic acid, is C6H8O6. Ascorbic acid is an organic compound derived
from glucose. The name "Ascorbic" means (a–) "no" and (scorbutus), a disease caused by not
having enough Vitamin C

Unknown Weak Acid Lab Report
The purpose of experiment ten was to collect data on an unknown weak acid by watching and
measuring the weak acid being neutralized. This was done by using a Vernier Probe and using the
data to figure out the identity of the unknown acid. A weak acid will have a strong conjugate base.
The pKa of a weak acid can be taken from the – log (ka) or by using pH. To find the pKa using the
graph of the pH in the experiment the equivalence point was found and ½ of this point is the pKa of
the unknown weak acid. To determine the molar mass of the unknown acid the moles of base has to
be determined along with the mass of the acid (Westfield, n.a). The equivalence point needed to
determine the pKa is the point of the titration curve where the pH begins

Determine The Identity Of An Unknown Weak Acid Lab Report
Determining the Identity of an Unknown weak acid (Vernier)
Formal Lab Report
Kelli McWatters
August 7, 2017
Chem 1121
Dr. Reed
Objective:
Observe and measure a weak acid neutralization and determine the unknown identity of an unknown
acid by titration.
Introduction:
Within an acid–base titration the titration curve resembles the strengths of the corresponding acids
and bases. A strong acid will correspond with a weak conjugate base, and a weak conjugate acid will
correspond with a strong base. This is based on the Bronsted–Lowry model. The weak acid will
donate protons to the hydroxide ion. Weak acids will have a low Ka value, the Ka value is the
tendency of the acid to dissociate: Ka= [H+] [A–] [HA] Ka is the acid dissociation constant and
[HA] is the concentration of the weak acid . Strong acids usually completely dissociate and has a Ka
value greater than 1. Weak acids don't dissociate completely and have a Ka value much smaller than
1. pKa values are often used for weak acids due to being able to work with whole numbers pKa =–
log Ka During a titration the pH of the solution will be monitored using a pH meter from that we get
a titration curve. The titration curve is then used to determine the equivalent molecular weight and
Ka value of the unknown weak acid, from that we are

6-2: Lab Assignment Ranking Salt Solutions by Ph Essay
Ranking Salt Solutions by pH
6–2: Ranking Salt Solutions by pH
In this assignment you will be asked to rank aqueous solutions of acids, bases, and salts in order of
increasing pH. This is most easily done by first identifying the strong acids that have the lowest pH,
the strong bases that have the highest pH, and the neutral solutions that have a pH near 7. The weak
acids will have a pH between 1 and 6 and the weak bases between 8 and 14. The exact order of
weak acids and weak bases is determined by comparing the ionization constants (Ka for the weak
acids and Kb for the weak bases). After ranking the pH of these solutions, you will then test your
predictions in the laboratory.
1. Arrange the ... Show more content on Helpwriting.net ...
Drag the 25 mL cylinder to the beaker on the stir plate and empty it into the beaker. Place the pH
probe in the beaker and record the pH in the data table. Drag the beaker to the red disposal bucket.
Double–click the bottle of NaHCO3 to move it to the Stockroom counter. Repeat steps 5 and 6 for
KNO3.
7. Click in the Stockroom. Double–click on the bottles of NH3 and H2SO4 to move them from the
shelf to the counter and return to the laboratory. Drag the bottle of NH3 to one of the three spotlights
on the lab bench. Place a beaker from the drawer on the stir plate. Drag the bottle of NH3 to the 5
mL graduated cylinder (the smallest one) by the sink and fill the cylinder by dropping the bottle on
the cylinder. Now drag the 5 mL graduated cylinder to the beaker on the stir plate and add the 5 mL
of NH3. Add 20 mL water to the beaker by filling and emptying the 10 mL cylinder into the beaker
twice. Place the pH probe in the beaker and record the pH in the data table. Drag the beaker to the
red disposal bucket. Double–click on the NH3 bottle to move it back to the counter.
8. Repeat step 7 with H2SO4, except that you should use a 10 mL graduated cylinder of H2SO4 and
adding 15 mL water.
9. Each of the other solutions is already approximately 0.1 M. With these solutions you can pour a
small

Extended Response Task: Acid And Bases
Extended Response Task– Acid and Bases
Introduction:
A buffer solution is a solution (consisting of a mixture of a weak acid and its conjugate base or a
weak base and its conjugate acid), which minimises changes in pH when small quantities of acids or
bases are added to it. In a way, it is used to consistently moderate the pH of a solution, and is
measured using the Acid Dissociation Constant.
General Formula:
HA⇋H^++A^–
NaA⇋N^++A^–
Where HA is a weak acid, N+ is a salt, and A– is a weak base.
Example of a basic buffer: 1.0 M of NH3 solution.
N〖H_3〗_((aq) )+H_2 O_((l) )⇌N〖H_4^+〗_((aq))+OH_((aq))^–
If enough NH4Cl is added to the solution for [NH4+] to reach 1.0 M, according to Le Chatelier's
Principle (that if a constraint is applied to a system in equilibrium, the equilibrium will shift so as to
tend to counteract the effect of the constraint), the ... Show more content on Helpwriting.net ...
When the blood reaches tissue where [O2] is low, the equilibrium shifts to the left per Le Chatelier's
principle, releasing O2.
If the [H+] is too high, the equilibrium cannot shift right enough in the lungs and cannot form
enough oxyhemoglobin. This condition is called acidosis, which causes headaches and fatigue from
the depletion of oxygen to the cells.
Acidosis can occur temporarily during exercise as the demand for energy exceeds the supply of
available oxygen to complete the oxidation of glucose to CO2. The glucose is converted to the
acidic metabolism product lactic acid.
As the tissues become starved for oxygen, lactic acid is produced to decrease the pH. This decrease
shifts the equilibrium to the left, delivering more O2 to the tissues. Moreover, it stimulates an
increase in breathing rate, eliminating CO2 whilst furnishing O2.
The Hb buffer system is effective in this scenario because it successfully delivered O2 to the tissues,
as depletion of oxygen in tissues make further activity impossible.

Analysis of Soda Ash and Volumetric Analysis of a...
Analysis of Soda Ash and Volumetric Analysis of a
Carbonate–Bicarbonate Mixture
Manalo, Ma. Cristina Joyce B.
Department of Chemical Engineering, Faculty of Engineering
University of Santo Tomas
Espana, Manila
A. Abstract
Crude sodium bicarbonate or commonly known as soda ash may contain amounts of impurities like
chlorides and hydroxides. The total acid neutralizing capacity of a soda ash sample, its alkalinity
value, was stated in terms of mass of sodium carbonate. In doing so, any sodium hydrogen
carbonate present in the sample was converted to its equivalent neutralizing capacity in terms of
sodium carbonate. A mass of the impure sample was dissolved and diluted in distilled water. 3 drops
of indicator was mixed and the ... Show more content on Helpwriting.net ...
Preparation of 0.10 M HCl 500 mL of distilled water was measured and put to a beaker. 4.2 mL of
concentrated HCl was added carefully and slowly to the beaker. The solution was stirred and then
transferred into a labelled storage bottle. b. Standardization of NaOH Two burets were prepared and
with one buret, 20 mL of the standard NaOH was transferred into a dry container. 3 drops of methyl
orange were added. The acid buret was filled with the acid to be standardized and the acid was
titrated with the base until the formation of an orange–colored solution. c. Analysis of the
Carbonate–Bicarbonate Mixture The electrode was rinsed with distilled water and was immersed
carefully into the specified buffer. The acid buret was filled up with the standard acid (HCl). The
initial volume of the acid was recorded. A 2.00 gram of solid sample was weighed and dissolved and
diluted with distilled water in a volumetric flask. A 50.0 mL aliquot was measured and 3 drops of
phenolphthalein were added. The electrode was immersed to the solution and was titrated with acid.
The volume of the HCl used to obtain a pink–colored solution was recorded. 3 drops of the methyl
orange were added to the same mixture. The volume of the acid used to obtain an orange–colored
solution was recorded. E. Results and Discussion I. Analysis of Soda Ash
Standardization of NaOH | Trial 1 | Trial 2 | Volume of NaOH | 20.0 mL | 20.0 mL | Final Volume of
HCl |

Alka Seltzer Lab Report
The buffer is a solution that minimises the changes in pH when small amounts of acid or base is
added.There are two types of buffer solutions.They can either be acidic or alkaline.An acidic buffer
is made by mixing equal amounts of a weak acid and its conjugate base.Similarly, an alkaline buffer
has equal amounts of weak base and its conjugate acid.
Alka seltzer acts as an antacid. It uses sodium hydrogen carbonate to neutralise excess hydrochloric
acid in the stomach and thus relieves heartburn.
Here, the bicarbonate reacts with a proton(from excess acid in the stomach)to release carbon
dioxide(H20 + co2).
It can also neutralise the hydroxide ions forming carbonate ion and a water molecule
HCO3–(aq) + OH–(aq) –> CO32–(aq) + H2O(l)
HCO3–(aq) + H+(aq) (–– removed HTML ––) CO2(g) + H2O(l) ... Show more content on
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When Alka seltzer tablet is dissolved in water, the sodium hydrogen carbonate and the citric acid
present in the tablet react together forming sodium citrate. This is a neutralisation reaction.This
sodium citrate is easily absorbed in the blood.Here, the sodium citrate behaves like an antacid.It is a
conjugate base of a weak acid(citric acid)
The buffer is a solution that minimises the changes in pH when small amounts of acid or base is
added.There are two types of buffer solutions.They can either be acidic or alkaline.An acidic buffer
is made by mixing equal amounts of a weak acid and its conjugate base.Similarly, an alkaline buffer
has equal amounts of weak base and its conjugate

Food Test Lab Report
In this lab, solutions are mixed with an indicator (red cabbage juice), which can be able to identify
whether it is an acid, base or neutral. Acids are aqueous solutions that contain H+ (hydrogen) ions.
When identifying acids, they relatively have a sour taste, like the citric acid which is found in fruits.
Some acids are safe to consume, however there are some acids like hydrochloric acid, nitric acid
and others that cannot be eaten, as they are highly corrosive. Acids are also electrolytes which
means they can conduct electricity. When it reacts with a base, it goes through a process of
neutralization where salt and water are formed. On the pH scale, acids have a pH of lower than 7,
with weak acids ranging from 1–3 and strong bases are 4–6. ... Show more content on
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Bases are characterized by their bitter taste and slippery, like soap. Just like acids, bases are
conductive, allowing electricity to pass through. Bases too can be eaten, but like acids, there are
bases where it cannot be eaten as it is corrosive. If eaten, bases can create damage to your stomach.
Some corrosive bases are lithium hydroxide, sodium hydroxide and more. Bases have a pH scale
greater than 7. Weak bases have a pH range of 8–10, where as the pH in strong bases are 11 and
higher. Solutions that are neutral have a pH scale of 7, which means that it has an equal amount of
hydrogen and hydroixide ions. It is not basic nor acidic, as it does not have any of properties that
acids and bases are identified with. An example of a neutral is sugar and distilled water. To
determine if a substance is acidic, basic or neutral, indicators are used. When added to a solution,
indicators are substances that change colours to categorize the solution as either an acid, base or
neutral. Some examples of indicators are phenolphthalein, litmus paper and the juice of red cabbage.
Phenolpthalein is a clear, colourless substance, changing into pink

The Effect Of Chemical Reactions On Temperature, Enthalpy,...
Discussion of Goals During this experiment we tested the amount of change in heat given off during
different chemical reactions. We created a calorimeter that we will use to test different reactions to
see how the heat energy was affected. After completing the experiments we were able to tell what
chemicals or metals would change the heat energy for every reaction we tested. Overall, this
experiment showed us what characteristics of chemical reactions affect the change in temperature,
enthalpy, and specific heat. Discussion of Results During the past four weeks we have been working
on identifying heat changes between an assortment of different chemicals and metals. We
constructed two calorimeters out of four Styrofoam cups, tape, ... Show more content on
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The cause of the large gap simply could have been a measuring mistake and or possibly an added
human error. After making our final tweaks to our calorimeters we moved on to experimenting with
the heat changes for several acids and a base mixture continuing from week one. We tested the same
base (Sodium Hydroxide) with three different acids (Acetic Acid, Nitric Acid, and Hydrochloric
Acid) all at one molarity; results are shown in Table 2. After testing our three experiments we
discovered a pattern with our acid and base reactions. Noticing that when we tested a stronger acid
with a base the reaction would give off higher heat energy readings; versus the weak acid we tested.
Which proves that there is a connection between chemical strength and heat energy. Leaving us with
the conclusion that the stronger the chemical used, the greater heat energy released from the reaction
that took place. Moving on with our project into week two we continued to test acids and bases; but,
we changed the acid and base molarity this time as seen in Table 3. The point of this experiment was
to see if the acid and base molarity (that we changed from 1, 3, and to 6 moles) would affect the
amount of heat energy given off. We tested the same Acetic Acid and NaOH. Measuring 50mL of
one mole NaOH and adding 50mL one mole Acetic Acid. We tested each experiment twice to make
sure we were accurate and checked for possible errors made. We did have one

Kickin Some Acids And Bases
Kickin' Some Acids and Bases
Katie Bachman, Kurt Wohlrab, Matthew Naumchik and Svetlana Griego
Chemistry 152–002
Brinkley
04–25–17
INTRODUCTION:
"Your research team has been called to the site of a former manufacturing facility that used acids
and bases in the dyeing of fabrics. The problem is that the drums of acids and bases are not labeled.
Your task is to identify whether your substance is an acid or a base. You then need to determine if it
is a strong acid, weak acid, strong base or weak base. In addition you should identify which acid or
base you have. Finally, you want to do further testing by performing a pH titration on each of your
unknowns. This will help you determine the concentration of your unknowns. ... Show more content
on Helpwriting.net ...
It weighs 56.105 g/mol when dry it resembles powder or crystals. It is white with a slight yellow tint
with lumps, rods, flakes, sticks or pellets for shape. Potassium Hydroxide does not have an odor to
it. With a boiling point, greater that 266oF and a melting point around 360 oC this substance is non–
combustible. This chemical has many uses including being used as a bleaching agent, functional
fluids, lubricants and solvents. This chemical can cause severe burns to the eyes, skin and mucous
membrane if it comes in contact. It is also dangerous because of its corrosive qualities. Sodium
Acetate is a weak base weighing 82.034 g/mol. It is a white powder or crystal substance with no
odor. It has a melting point of 324oC and is soluble in water and slightly soluble in alcohol. It is
used in anti–freeze, fuel, fuel additives as well as processing aids. It is combustible and decomposes
when heated or when coming in contact with strong acids. When this happens, toxic fumes are

Comparing The Determination Of Molarity Of Naoh By Titration
In this experiment we will be titrating the titrant sodium hydroxide against the analyte, which is the
substance being analyzed, hydrochloric acid. Titration is the process of analyzing base and acid
added together. The objective is to calculate the unknown concentration of hydrochloric acid with
the standardized solution of solid sodium hydroxide. The standardized solution is the known
concentration but since sodium hydroxide naturally reacts with air, we must first determine the true
concentration of NaOH by titrating against a weak acid, potassium hydrogen phthalate (KHP) that is
the known concentration. In the first experiment we will need to find the molarity of NaOH, which
is determined by multiplying the moles of KHP in volumetric

Buffers Lab
Buffers are solutions that resist change in pH when small amounts of strong acids or bases are added
to it. Adding a strong acid to a solution would decrease its pH as seen in fig 2 and adding weak base
would increase its pH as seen in fig. 3. One good use of buffers in a biology field is that buffers
control the pH in order for the cells to live in a livable environment. If the cell is too basic it releases
H+ ions into the cells and if its too acidic the buffer releases OH–. Therefore, buffers inside and
outside the cells help maintain the pH in the cytoplasm because if the pH is not applicable in the
cell, the cell dies. To recap buffers in the cells, help to maintain an ideal environment for
biochemical reactions to take place.
However, ... Show more content on Helpwriting.net ...
In part 1 of the experiment was where a stock solution was prepared using different quantities of
acid and base and comparing the predicted PH using the Henderson–hasselbach equation vs. the
measured pH using a pH probe. The Ph readings that was measured and graphed were pretty close
and off by approximately 0.03–0.08 points and we can say that is an accurate reading, meaning that
the probe was calibrated precisely in order to have a pH reading of the prepared solution as close as
possible to the predicted ph. When we used the hasselbach equation for the predicted pH we were
provided with a pKa of 7.18, looking at graph 1 at the intercept of each line, the pKa of the
measured pH is 7.195 and the predicted pH has a pKa value of 7.18, rounding those values to one
decimal place we get a pKa value of 7.2 for both and that is spot on compared to the provided pKa
for the Henderson–hasselbach equation. Looking at the graph, we can conclude that as pH increases
the concentration of acid/base increases

Buffers Lab Report
In this lab, the pH of seven different substances and solutions were tested both before and after the
addition of multiple drops of acid (HCl), or base (NaOH). Depending on the variation of the
affected pH from the original, the buffer range of the substance could be calculated by finding the
average pH fluctuation, both with the added acid and the added base. As shown in the graph above,
the buffer is labelled in dark blue, and the average pH fluctuation from the original was only 1.12.
This low pH variation characterizes a buffer, and therefore, the tested solutions and substances with
an average buffer range close to the buffer solution can also be considered buffers as well. For
example, both lemon juice (magenta) and baking soda (yellow) ... Show more content on
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Human blood, in fact, contains large amounts of both carbonic acid, a weak acid, and bicarbonate, a
base. Together, they help maintain the blood's pH of roughly 7.4. If the pH were to fall below 6.8 or
rise above 7.8, the organism affected can become sick or die. The bicarbonate neutralizes excess
acids in the blood while the carbonic acid neutralizes excess bases. Similarly, when we consume
antacids or milk of magnesia after eating a meal with particularly rich foods, the stomach must
produce gastric acid to digest the food. This acid can enter the lower end of the esophagus, causing
an uncomfortable burning sensation. To relieve this burning, one would take an antacid, which when
dissolved, the bases buffer the excess acid by binding to them. All throughout the biology and life
processes, even down to individual cells, chemical homeostasis must be maintained for optimal
function. Therefore, buffers are extremely useful and important to all aspects of life, as they regulate
the pH of solutions and aid in the consistency of organic

Ph Lab Report Essay
Objective
The objective of this lab is to determine the pH of common household items.
Introduction
This experiment involved determining if the liquids tested were acidic, a basic or neutral. An acid is
a chemical substance that turns litmus paper red, neutralizes alkalis, and dissolves metals. Bases are
chemical substances that change litmus paper blue, react with acids to form salts and encourage
certain chemical reactions.
Acids produce H+ ions in aqueous solutions while bases accept H+ ions as well as produce OH–
ions in aqueous solutions. In other words, acids are viewed as electron pair acceptors and bases as
electron pair donors. Every liquid has either acidic or basic properties. A liquid that is an acid will
taste sour and a liquid that is a ... Show more content on Helpwriting.net ...
Which ingredients contribute to each of the liquid's pH level?
Lemon Soda: Citric Acid
White Vinegar: Acetic Acid
Apple Juice: Ascorbic Acid
Shampoo: Citric Acid
Conditioner: Sodium Carbonate
Baking Soda: Sodium Bicarbonate
Real Life Applications:
Neutralization: Whenever you mix an acid with a base, they neutralize each other. If this is the case,
why is Alka–Seltzer used to treat stomach ashes? (Note: excess stomach acids cause stomach aches)
–Alka–Seltzer will neutralize any excess stomach acid, as a base.
2. Acid Rain: What is acid rain and how is it a problem to oceans, rivers, lakes, ponds.
–Acid rain is rain that contains elevated levels of hydrogen ions, due to pollination in the air. This
causes the perception to be unusually acidic. Acid rain has many harmful effects within the
ecosystem of oceans, rivers, lakes and ponds, because once the water becomes too strongly acidic,

certain species will start to die in said ecosystem. In this case, the species that will begin to die,
include fish. Acidic rain, along with snow and fog can also be considered dangerous to humans as
well, as it is known to cause respiratory

Investigation Of A Reagent Experiment Essay
[Cu(H2O)4]2+ (aq) + 4 NH3 (aq) [Cu(NH3)4]2+ (aq) + 4 H2O (l) Initial observations – 0.1 M
CuSO4: light blue, transparent, odourless liquid – NH3: colourless, transparent, strongly odorant
liquid – 1.0 M HCL: colourless, transparent, odorant liquid Experimental Observations – Addition
of 2 drops of concentrated NH3 to 1 mL 0.1 mol/L CuSO4 caused solution to become dark blue,
become translucent, and odourless – 24 drops of 1 mol/L HCl was added until colour changed to
light blue, odourless, transparent solution Discussion H2O is the molecule that caused the CuSO4
solution to be a light blue colour; without it, CuSO4 would be anhydrous and colourless. When NH3
was added to the CuSO4 solution the colour turned dark blue. According to Le Chateliers principle,
the reaction shifted towards the products. This is because the addition of a reagent causes the
reaction to produce more product and use up reagent. The single displacement of [Cu(H2O)4]2+ to
[Cu(NH3)4]2+ lead to excess production of [Cu(NH3)4]2+. The dark blue colour is explained by
the replacement of H2O by NH3, where NH3 allows for a greater absorption of yellow light than the
water molecule. The addition of H+ ions from HCl bonded with NH3 to make NH4, decreasing the
concentration of NH3 in the solution. This lead to the reaction shifting towards the reactants,
producing more NH3 and [Cu(H2O)4]2+ than [Cu(NH3)4]2+ and H2O, thus changing the colour to
light blue. If steps 2

Hot And Cold: An Investigation Of Enthalpy Changes Occurring
Hot and Cold: An Investigation of Enthalpy Changes Occurring During Various Types of Reactions
Hannah McCall
Chemistry 101 Laboratory, Section 005
Instructor: Lisi Wang
April 11, 2017
My signature indicates that this document represents my own work. Outside of shared data, the
information, thoughts and ideas are my own except as indicated in the references. I have submitted
an electronic copy through Blackboard to be scanned by TurnItIn.com. In addition, I have not given
aid to another student on this assignment.
Discussion and Scientific Explanations
Construction of Calorimeter After building the calorimeters, the formula (Heat Capacity) = ((Heat
lost by hot water) –(Heat gained by cold ... Show more content on Helpwriting.net ...
This is because the equation for the equation of this reaction is HCl + NH4 Thus, the enthalpy
changes for the reaction between 6M HCl and 1M NaOH had an enthalpy change of approximately
one sixth of the enthalpy change for the reaction between 1M HCl and 1M NaOH.
According to our results, again looking at Table 2, we can say that reacting a strong acid with a
weak base results in lower enthalpy change than reacting a strong acid with a strong base. This is
because the enthalpy changes during the reactions between HCl, a strong acid, and NH4OH, a weak
base, were –51.35 and –46.92 kJ/mole, while the enthalpy changes during the reactions between
HCl and NaOH, a strong base, were –61.87 and –65.16 kJ/mole. Although the difference between
these values is not that large, because the values for the respective reactions are consistent and have
little difference between them, we can conclude that the reaction between a strong acid and a strong
base has a greater magnitude of enthalpy change than the reaction between a strong acid and a weak
base.
According to our results, the reaction between a weak acid and a strong base results in a greater
magnitude of enthalpy change than the reaction between a strong acid and a strong base because the
enthalpy changes for the reactions between CH3COOH, a weak acid, and NaOH, a strong base, had
enthalpy changes of

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