Coarse Titration Lab

Coarse Titration Lab
Titration is a method used to determine an unknown concentration of a known solution. Through
this, we may know the chemical that can be dissolved, but not how much of the chemical could be
in a specific solution. The purpose of this lab is to be able to determine the concentration of a
hydrochloric acid solution using acid base titration in where hydrochloric acid solution is a strong
acid and sodium hydroxide is a strong base. In experiment 1, I perform a coarse titration. A coarse
titration is a method not very accurate in identifying the end point in the solution, but it does identify
the range of titrant volume in which the endpoint happen. In the coarse titration experiment I took a
certain amount of sodium hydroxide and added to the
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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

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

What Is An Unknown Titration Of Hydrochloric Acid
The purpose of this experiment is to determine an unknown concentration of acid (hydrochloric
acid) with a standard solution of a base (sodium carbonate) using titration method. The hypothesis
is; as we know the concentration of sodium carbonate (Na2CO3) we can obtain the concentration of
hydrochloric acid using the titration of a standard solution. Theoretical Principles behind Titration:
Titration is the slow addition of one solution of a known concentration (called a titrant) to a known
volume of another solution of unknown concentration until the reaction reaches neutralisation,
which is often indicated by a colour change. The solution called the titrant must satisfy the necessary
requirements to be a primary or secondary standard. In a broad sense, titration is a technique to
determine the concentration of an unknown solution. We can use the reaction to find out the
molarity of the solution by measuring the product(s) that is formed. In this experiment, we use a
known concentration (Na2CO3) to determine an unknown concentration of acid (HCl). This reaction
is neutralisation reaction, which we'll get water and salt as the products. Acid + Base Salt + Water
We can use a pH indicator, a chemical that changes colour depending on the pH, to show us when
the reaction has completely neutralised. This point, where all acid was consumed and there is no
excess of base, is called the equivalence point (end point). We can use this

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

Concentration Of Acid-Base Titration
Acid–Base titration is defined as using a solution of known concentration and volume to find the
concentration of a solution with known volume but unknown concentration. Acid–Base titration can
be used when mixing strong acids and strong bases because strong acids and bases neutralize each
other. Phenolphthalein indicators, substances that change color based on pH, can be used to
determine when the titration is complete and when both of the solutions are neutralized. In this
experiment, Acid–Base titration will be used to determine the concentration of 10mL of an HCl
solution by adding a known volume 0.1003 M NaOH solution using a buret. The chemical equation
for this reaction is NaOH(aq)+HCl(aq) → NaCl(aq)+H2O(l). Because the moles of NaOH equals
the moles of HCl, the number of moles of NaOH that are added to the solution in order to neutralize
it will equal the moles of HCl in the solution. The number of moles of NaOH added to the solution
will be used to determine the moles of HCl, which will then be used to determine the molarity of the
HCl solution by dividing the number of moles of HCl by the volume of HCl, according to the
formula: Moles/Volume=Molarity.
Results
The average HCl molarity was found to be 0.090 M. Our actual values were 0.091, 0.091, and
0.089. These molarities were found according to the formula mass/volume=molarity. For example,
0.089 was found by dividing the moles of NaOH added to the solution (8.9x10–4) by the volume of
HCl

Titration Research Paper
Quantitative Chemistry –Titration Determination of the Molarity of an Unknown Solution through
Acid–Base Titration Technique
1. Introduction
1.1 Aim
The aim of this investigation was to determine the precise molarity of two (NaOH(aq)) sodium
hydroxide solutions produced at the beginning of the experiment through the acid–base titration
technique.
1.2 Theoretical Background
Titration is a method commonly used in laboratory investigations to carry out chemical analysis.
The most frequent chemical analysis performed through titration is when determining the exact
concentration of a solution of unknown molarity. This technique is usually used in redox and acid–
base reactions. Redox reaction is when reduction – ... Show more content on Helpwriting.net ...
Therefore, after the titration was performed as explained on the previous paragraphs, the data
needed to calculate the molarity of NaOH(aq) was obtained.
1.3 Preliminary calculations
1.3.1 The first important value to be obtained from the investigation was the volume of NaOH(aq)
used. This was done by the following equation: eq.3 – for 1st solution produced
Average volume volume of 2nd trial – volume of 1st trial2= V1 eq.4 – for 2nd solution produced
Average volume volume of 2nd trial – volume of 1st trial2= V2
1.3.2 The next step when determining the molarity of NaOH(aq) was to calculate the moles of
HCl(aq) by using the volume HCl(aq) provided on the lab scripts and the molarity obtained from the
bottle of HCl(aq) used during the investigation. The eq.5 and eq.6 below was used to calculate: eq.5
– moles1 = V1 (dm3) × molarity (M) eq.6 – moles2 = V2 (dm3) × molarity (M)
1.3.3 The third important equation, for both solutions, worth noting are the number of moles of
NaOH(aq) present in the reaction. This was obtained by using ratio of the moles of NaOH(aq) :
HCl(aq) used during the investigation. This can be recalled by eq.2 eq.2 – HCl(aq) + NaOH(aq)
NaCl(aq) + H2O(l) 1 : 1
1.3.4 Hence, moles of both solutions of NaOH(aq) will be the same as the number of moles of
HCl(aq) since the mole ratio is 1:1. That is for every one mole of HCl(aq)

Titration Of A Concentration And The Acid Base Titration
Summary
The purpose of this experiment was to find the molarity of a concentration and the acid–base
titration. In part A of this experiment, the molarity of an assigned concentration which was 0.040,
was found using formulas that represent molarity. Part B of this experiment, which was titration of
an acid and base, was found by a series of steps that involved dropping Sodium Hydroxide from a
buret into vinegar, until the perfect shade of pale pink occurred. With the Phenolphthalein, too much
acid causes the base to turn a dark pink. The molarity was then found of the titration. So the end
results will determine M HCH3O2.
Introduction A solution is a homogenous mixture of a solvent and one or more solutes. The
substance that dissolves in the solute is the solvent, and the solute is what gets dissolved. Solutions
can vary in concentration in great ratio differences. It is very important to be able to correctly
prepare solutions. There is always a proper amount of solution to be made to have a desired amount
of produced. So in the medical world, too much solute will most likely have harmful effects like
overdosing and too little could result in ineffective treatment. Also the money spent on solutions
could also be another reason for correct preparation of solutions, because the success of the drug has
an effect on future sales and profit. Solutions that are dilute, are weak, and solutions that are
concentrated are strong. A precise means of describing concentration is 1.

Titration Laboratory
Colegio Católico Notre Dame
Caguas, P.R
Laboratory:
Titration of an Acid with a Base
Tristian Pérez Rivera
12–136
AP Chemistry
Professor Judith Martínez PhD
Objective * The purpose of this laboratory is to recreate and understand what titration is.
Hypothesis
* If the experiment works correctly, we should determine the amount of a substance by adding a
carefully measured volume of a solution with known concentration until the reaction of both is
complete.
Materials
* Computer
Pre–lab
1. How will you know when your titration is finished? I will know that the titration is finished when
the color of the indicator changes, meaning that the equivalence point has been reached.
2. Draw and label the pH scale below with acid, base, ... Show more content on Helpwriting.net ...
Phenolphthalein changes from white to pink at a pH of 8.2–10.0. Bromothymol blue changes from
yellow to blue at a pH of 6.0–7.6. In my case, I used Bromothymol blue for all because the
equivalence point for a strong acid being titrated by a strong base is at a point near the neutral
position.
6. (a) Why is it important for the buret to be clean before using? How do you clean a buret?
It is important to clean the buret thoroughly before using it because it will help for the buret to
perform better and will minimize or even prevent error in the experiment.
(b) Why are air bubbles in the buret tip a possible source of error in a titration experiment? How do
you remove air bubbles from the buret tip? Air bubbles in the buret tip can cause error in a titration
experiment because it can cause the reader to read an inaccurate value of the volume in the buret.
One can remove air bubbles by draining several milliliters of the titrant into a waste beaker.

7. Predict the products of these reactions.
(a) HNO3 (aq) +KOH (aq) KNO3 (aq) + H2O (l)
(b) HCl (aq) + Ca (OH) 2(aq) CaCl2 (aq) + 2H2O (l)
(c) NH3 (aq) + H2SO4 (aq) HSO4– (aq) + NH4+ (aq)
8. For the reactions (a) and (b) in question 8, how many moles of the base are required to neutralize
one mole of the acid? How many mL of 0.100 M base are required to neutralize 10.00 mL of 0.100
M acid?
(a) It takes 10.0mL of the 0.100M base to neutralize the 10.0mL of the 0.100M acid

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

M1: Standard Solution And Titration
M1– Standard solution and titration
In the experiment, Sodium Carbonate (Na2C03) was mixed with Hydrochloric acid (HCL) to make
a standard solution.
The concentration of the sodium carbonate was known and the volume of hydrochloric acid was
known however, the concentration of hydrochloric acid was unknown which is why we did the
experiment to fine the concentration of the acid.
In this experiment, when adding the hydrochloric acid (2HCL) to the sodium carbonate (Na2CO3),
we got sodium chloride (NaCl) + carbon dioxide (CO2) and water (H20).
Sodium is a metal in group 1 in the periodic table, the sodium ion has a charge of
+1; this means that one electron is lost from the outer shell of sodium with the electronic
configuration of 2,8,1.
Chlorine

Explain Why Are Three Replicate Titrations
1. Why are three replicate titrations done for each sample? The more times an experiment is done,
the more reliable the answer becomes. Therefore, three replications are done in order to reduce the
error. 2. What other household products could be analyzed by titrations (suggest three)? We could
analyze other household products, for example, drain cleaner, milk of magnesium, and citrus fruits.
3. Why is it necessary to add an indicator? Describe how an indicator works. A chemical indicator is
a substance that indicates the presence or absence of certain conditions. A common indicator is
Phenolphthalein. It remains colorless in acidic solutions and turns pink in basic solutions. Because
both acidic and basic solutions are colorless,

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
content on Helpwriting.net ...
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

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

Antacid Titration Lab Report
Neutralization of an acid using a base
Introduction: Last week I had a chicken cheese burrito and got a massive heart burn. My mom gave
me some tums and the heartburn went away. This made me think about antacids and how much of
the table is actually useful? The reaction of NaOH when titrating with KHP or an CaCO3 (Antacid)
could be expressed with the equation (KHP) – NaOH(aq) + KHC8H4O4(aq) = KNaC8H4O4(aq) +
H2O(l) and CaCO3 + NaOH = Na2CO3 + Ca(OH)2
Research Questions: How much of an antacid is in an antacid tablet?
Variables: The dependent variable would be the antacid tablets. As it is crushed and put with the
acid. The independent variable would be the amount of NaOh used to titrate.
Materials:
Safety: When dealing ... Show more content on Helpwriting.net ...
When titrating the process was quite long since we used a little bit extra Acid to dissolve the tums
tablet. I believe that the mass of the tum size definitely had an impact on the amount of NaOH
required.
Conclusion: The calculations of three tablets' antacid property roughly 500mg had variables that
ended up resulting through the data results that the amount of CaCO3 in each pill is close to
advertised. The end result was an error of only 3.6% which is extremely close to the actual value.
The slight uncertainties gathered from tools and human errors would have definitely played a role in
increasing the percent error.
Further Investigation:
There are other experiments that can be done to understand the titration of KHP. We can titrate
larger amounts of KHP in water. The experiment would be undetermined of the different sized tums
tablets. We would be able to evaluate the different concentration of CaCO3 is the same for any tum
tablet regardless of size.
Calculations:
10.8mL NaOH = 0.1076 L NaOH
0.005 mol KHP/ 0.1076 L NaOH = 0.46M

Lab Report On Titration
Introduction: The Objective of the lab is to determine the mass percent of ascorbic acid in a vitamin
C tablet by titration with a sodium hydroxide solution of known concentration. A titration is a
procedure in which we measure the volume of a solution of a solution of known concentration that
is needed to completely react with volume of NaOH analyzing. A buret is used to measure the
amount of NaOH in titration and it is a piece of calibrated glassware used to accurately deliver
volumes of a liquid or a solution. To determine when the neutralization reaction is complete by
adding an acid–base indicator(Phenolphthalein) and it changes color at the end point. To calculate
the mass percent ascorbic acid in the sample by using mass of ascirvuc acid, gmass of sample,
g100%. Materials: Mortar
Pestle
Vitamin C tablet
2 Erlenmeyer flasks 250 mL
Balance
50 mL buret
Buret clamp
Support stand
250 mL beaker
Short –stem funnel
Sodium hydroxide(NaOH)
150 mL dry beaker
Stirring rod
Phenolphthalein solution Procedure: 1.Two 250 mL erlenmeyer flasks was labeled 1 and 2 and
weighted
2.Vitamin C tablet was crushed into powder and transferred roughly equal into the labeled
erlenmeyer flasks.
3.The mass of erlenmeyer flasks that contained the powder of vitamin c was measured.
4.The buret was mounted on the support stand by using the buret clamp.
5."Discarded solutions" was labeled on a 250 mL beaker.
6.The stopcock of the buret was

For this experiment, a titration was performed to determine the unknown concentration of a given
HCl sample by reacting it with a solution of sodium hydroxide. NaOH first had to be standardized
due to it being hygroscopic. A hygroscopic substance is one that readily attracts water from its
surroundings, through either absorption or adsorption.1 The titration of KHP with NaOH was the
standardization process which determined the actual concentration of NaOH. This value helped
determine the volume of NaOH seen within the second derivative curve to find the moles of NaOH.
The moles of NaOH were then used to find the moles of HCl by looking at a balanced chemical
equation. The moles were divided by the volume of unknown 1 HCl to get the actual concentration
of HCl. The pH of the solution as it was being titrated was monitored by a pH probe and the
LabQuest software. Phenolphthalein, a pH indicator, was also used to determine when the solutions
reached their endpoints.
A titration is the slow addition of one solution of a known concentration (called a titrant) to a known
volume of another solution of unknown concentration until the reaction reaches neutralization,
which is often indicated by a color change.2 Titrations were performed during this experiment by
using a burette, burette clamp, utility clamp, pH probe, ring stand, and Lab Quest. The amount of
titrant added to the analyte could be seen on the burette by looking at the values. When the stopcock
of the burette was

Lab Report : Ph Titration
pH Titration Practical Write Up:
Introduction:
This experiment includes a standard solution, which according to Lewis, R. and Evans, W. "is a
solution of known concentrations". They also stated that "the procedure in finding the concentration
of a solution is called volumetric analysis. It involves reacting a solution of known concentration
with one of the unknown concentration, in order to determine the equivalence point".
Titration is a technique where one reactant is slowly added to a second reagent until the equivalent
point is achieved. Chemical indicators are substances that change their colour at a specific ratio of
reactant concentrations, which is known as the end point. In a titration, a chemical indicator is
chosen so that the equivalence point and the end point are the same.
This experiment is an acid–base titration. "the (previously unknown) concentration of an acid can be
determined by titrating it with a standard alkaline solution. The acid is neutralized by the alkali"
(Lewis, R. & Evans, W., 2011).
Using a suitable indicator, which changed colour over an appropriate pH range at the end point, the
end point of an acid–alkali titration could be revealed. A different method of revealing the end point,
which was the method that was constructed, is to continuously monitor the pH value of the solution
during the titration, carrying on until well past the end point. In this experiment, there was a sudden
swing in the pH value at the end point. The approximate

Titration Lab
Titration can be used to standardize a solution. In this experiment, sodium hydroxide was used to
titrate KHP solution. Using the results of the titration, the exact concentration of NaOH was
calculated to three significant figures. As see in data table A.1, the volume of NaOH used in trial one
is 25.95 mL, and moles of KHP is 0.003501 mol. Using this information, the molarity of NaOH was
found by using the formula, Mass of sample x (1 mole/ atomic mass), in Table A.2. After plugging
in the appropriate values and taking the average of the three trials, the molarity of NaOH is
calculated to be 0.136 M. The calculated molarity has three sig–figs, which is more exact than the
0.1M solution that was provided. Therefore, the data supports the conclusion ... Show more content
on Helpwriting.net ...
To begin with, the unknown acid did not dissolve in the water completely. At first, this problem
caused the titration to be messed up. Next, a new trail was done by letting the acid settle to the
bottom, then taking the solution of without including any precipitate from the bottom of the beaker.
In addition, when the unknown acid dissolved in the water, a foggy solution was created. This
caused the titration to be tricky because it made it difficult to notice the change of color. Finally, the
NaOH that was used at first used in part B did not change color when it was added with the
indicator. This happened because the NaOH solution was prepared two weeks prior to this part of
the lab. The NaOH might have changed its properties as time went on, for instance, its concentration
might have changed. This problem was fixed by making a new NaOH solution. Other than that,
everything worked properly. However, one problem that might have occurred was overshooting the
solution. This could have been done by adding a large volume of the titrant to the solution, which
causes the pH of the solution to be messed up. Another problem that might have occurred was using
contaminated lab equipment. This problem would cause a base or an acid to change their pH leading
to errors during the lab. However, this problem was prevented by rinsing all glassware with
deionized

Titration Lab Report
Titration was performed over two weeks to determine the amount of acetic acid in vinegar. On the
first week, the purpose of the experiment is to standardize a 0.500 M of NaOH solution to be used in
week two. Since the stock solution was in 5.0 M NaOH, dilution of the solution was performed to
make 0.500 M NaOH solution. On the first week, 40 mL stock solution was diluted with 360 mL of
water to attain a 400 mL .500M NaOH. This method is considered imprecise because the
concentration of stock solution is only precise to 2 significant figures. In order to accurately and
precisely determine the concentration of NaOH, the primary standard KHP was used in the titration
of NaOH. In the first week, the 1.08 g of KHP was dissolved with 25 mL ... Show more content on
Helpwriting.net ...
One of the biggest systemic error is that the substance used in week 1 was not actually KHP. Since
the primary standard was wrong, the substance will require either a greater amount of titrant than
expected. Instead of titrating about 10.47 mL of NaOH to react with 1.08 g KHP, over 15mL of
NaOH was needed. This systemic error makes the calculation of the molarity of NaOH highly
inaccurate because the balanced equation with new substance was not used. According to week 1
calculations, the molarity of NaOH is reported as 0. This error mean the standardization of .500 M
NaOH has failed. Although the accuracy may be off, the preciseness of the titration over three trails
can be determined. The % RSD for the calculated NaOH concentration is 1.070%. Ideally, an
accurate titration will have a % RSD less than 0.2%. The reason for such high RSD % is due to the
many systemic errors with performing the titration. First, the mass of the KHP (not actually KHP)
was measured very imprecisely. As seen in both quick trial and the next 3 trials in table 1, the mass
of the substance was recorded as 1.072, 1.062, 1.075, and 1.068 respectively. If the mass of
substance used differ from the quick trial significantly, the estimation of end point will be less
accurate, making the titration more difficult. Therefore, it is important to use the same mass as the
quick trial in order to be more precise with getting the same

Introduction: Titration Is A Technique Used To Find The
Introduction: Titration is a technique used to find the concertation of an unknown acid, called the
analyte, through the use of a base with a known concentration, called the titrant. In this experiment
the analytes used were sulfuric and acetic acid and the titrant was sodium hydroxide. In order to find
the concertation of these acids, the acid and base were mixed until they reached the equivalence
point, or the point when the amount of titrant is equal to the amount of the analyte needed to fulfill
the mole to mole ratio necessary complete neutralization. When the equivalence point was reached
the phenolphthalein indicator made the solution turn light pink and this signified the endpoint of the
acid–base titration. Before the titration of ... Show more content on Helpwriting.net ...
After 5mL of the sodium hydroxide was used in the titration the remaining amount of sodium
hydroxide was added into the Erlenmeyer flask very slowly until the solution reached the
equivalence point, then the indictor turned a light pink color and the endpoint was reached. When
the solution turned a light pink color the stopcock was closed and the Volume was recorded.
1. Volume = Volume(Final)–Volume(Initial)
The Erlenmeyer flask was cleaned, the buret was refilled with the sodium hydroxide solution, and
the experiment was repeated again.
For the titration of acetic acid 2mL of acetic acid solution was measured and put inside of the
Erlenmeyer flask. The acetic acid was then diluted with 50mL of distilled water. Three drops of
phenolphthalein indicator were then added to the acetic acid solution. Then, the titrant (sodium
hydroxide solution) in the buret was added into the Erlenmeyer flask very slowly until the solution
reached the equivalence point. At the endpoint when the solution turned pink the stopcock was
closed and the Volume was recorded. The Erlenmeyer flask was cleaned, the buret was refilled with
the titrant, and the experiment was repeated again.
For the titration of acetic acid 2mL of sulfuric acid solution was measured and put inside of the
Erlenmeyer flask. The sulfuric acid was then diluted with 50mL of distilled water. Three drops of
phenolphthalein indicator were then added to the sulfuric acid

Discussion Of Potato Titration
The purpose of the iodimetric back titration, a form of redox titration, experiment is to determine the
weigh percentage of ascorbic acid in Vitamin C tablets. The experiment is performed by titrating
iodine solution that contains the dissolved ascorbic acid with sodium thiosulfate. The results of the
titration was inconclusive, and the weight percentage of the ascorbic acid could not be determined.
Several sources of error could explain the variation of titrated volume of sodium thiosulfate. These
sources of error include oxidation of sodium thiosulfate, the oxidation of ascorbic acid, the
instability of the iodide solution, and the starch indicator. Most of the sources of error are problems
with samples and solution being oxidized by the atmosphere. The results of the current experiment
is dependent on correcting the sources of error. To decrease the oxidation by air, prompt titrations
are needed and glassware that are light sensitive are needed to ensure that the sodium thiosulfate
solution does not oxidize.
Introduction The experiment is a redox titration process. A redox titration involves an oxidation–
reduction reaction between an analyte and the titrate (Harris, 2016, p. 374). Iodine is commonly
used in a redox titration as it is a versatile redox reagent. Therefore, iodine can be a moderately
weak oxidizing agent or a moderately weak reducing agents depending in the presence of strong
oxidants or reducing agents.
This versatility allows iodine to be

Acid-Base Titration Lab
Abstract
By using acid–base titration, we determined the suitability of phenolphthalein and methyl red as
acid base indicators. We found that the equivalence point of the titration of hydrochloric acid with
sodium hydroxide was not within the ph range of phenolphthalein's color range. The titration of
acetic acid with sodium hydroxide resulted in an equivalence point out of the range of methyl red.
And the titration of ammonia with hydrochloric acid had an equivalence point that was also out of
the range of phenolphthalein.. The methyl red indicator and the phenolphthalein indicator were
unsuitable because their pH ranges for their color changes did not cover the equivalence points of
the trials in which they were used. However, the ... Show more content on Helpwriting.net ...
Results
Part I: Data and Calculations
Table 2: Titration Data Table
Trial 1 – HCl and NaOH (Strong–Acid + Strong–Base)
Trial 2 – CH3COOH and NaOH (Weak–Acid + Strong–Base)
Trial 3 – NH3 and HCl (Weak–Base + Strong–Acid)
(*) marks equivalence range
Trial 1Trial 2Trial 3
Titrant Volume (mL)
pHTitrant Volume (mL)pHTitrant Volume (mL)pH
0.001.70.003.10.0010.4
5.001.75.004.05.009.7
10.001.710.004.410.009.3

15.001.815.004.815.008.9
20.002.020.005.120.007.9*
21.002.121.005.321.006.0
22.002.122.005.421.503.8
23.002.223.005.522.003.1
24.002.224.005.722.502.9
25.002.325.006.2*23.002.7
26.002.425.506.723.502.6*
27.002.726.009.824.002.5
28.003.026.5010.524.502.4
29.003.3*27.0011.2*25.002.4
30.003.827.5011.426.002.3
30.509.428.0011.627.002.2
31.0010.3*29.0011.728.002.2
31.5010.830.0011.830.002.1
32.0011.031.0011.835.002.0
33.0011.232.0011.840.001.9
35.0011.534.0011.9
40.0011.835.0011.9
40.0012.0
Table 3: Equivalence Point values.
Equivalence Point
Titration of HCl with NaOH7.0

Titration of CH3COOH with NaOH8.6
Titration of NH3 with HCl 5.5
1)Initial pH
See Table 2.
2)Final pH
See Table 2.
3)Equivalence Range
Using Graph 1: The Volume of Titrant Added in order to reach the Endpoint and the Corresponding
pH Values, observe the vertical line of each titration and see the points in which the horizontal lines
intersect it. These points give the

Titration Of Hcl Lab Report
For this experiment, a series of strong acid–strong base titrations were performed to determine the
unknown solution concentration of HCl. KHP was first titrated with NaOH in order to create a
standardized solution of NaOH. This solution was used to titrate a known volume of the unknown 1
HCl solution. The results were then used to determine the exact concentration of the original HCl
sample. One thing that could be changed during this lab is to use a more neutralized sample of
deionized water. Throughout the rinsing process of the pH probe, the deionized water's pH reading
would be more basic instead of neutral. Therefore, when testing the pH of the analyte, the results
were slightly basic rather than having a pH of zero. This could have resulted in the pH of the
solutions being slightly off when it came to the LabQuest readings.
The volumes of NaOH titrated at the endpoint and equivalence point related to one another
throughout the experiment. The volume was always greater at the endpoint than at the equivalence
point. For the titration of HCl and NaOH, the amount of NaOH added at the endpoint was 9.00 mL
and the 2nd derivative curve amount was 9.033 mL. Throughout Trial 2 and titrations of KHP and
NaOH, this same trend was seen. The most accurate volume amount of NaOH was determined by
looking at the equivalence point. This is the point where all of the H+ was neutralized by OH–. The
endpoint is where the indicator, phenolphthalein, changed color based on pH. The color

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
Helpwriting.net ...
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

Titration Lab
Titration is the slow adding of one solution of a known concentration (called a titrant) to a known
volume of another solution of unknown concentration until the reaction reaches neutralization which
is indicated by color change (1). We take the solution of known concentration and carefully mix it
with unknown concentration until the solution is concentrated. The main goal of this experiment was
to prepare a standard solution of oxalic acid and use it to standardize an unknown sodium hydroxide
solution. And finally to determine the molar mass of unknown solid acid by titration with
standardized NaOH solution. By weighting a sample prepare a solution of an acid of known
concentration. Make it up to a known volume in a volumetric flask. We use ... Show more content
The molarity of NaOH was 0.2089 mol per liter. Molarity of acid was 0.0766 mol per liter. Percent
difference for NaOH solution titration was 0.21 %. And the percent difference for acid was 0.39%.
The molar mass of unknown acid was 190.68 grams per mol. The source of error could be the use of
more volume of NaOH solution and acid solution during the titration. Yes, the results are reasonable.
If the experiment were to be repeated, careful adding of the solution during titration would result in
better percent difference. Also careful reading of the volume

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

Analysis Lab Report Titration
From the data collected during this experiment, results concluded that the average concentration of
the unknown solution of NaOH (aq) (Unknown A) was 0.0755 M. When compared to the true
concentration of NaOH, 0.075M, I would say that our experiment and results were accurate being
that the average concentration of NaOH found was just 0.0005M more than the true concentration of
NaOH. I would also say that our results were precise because without including our titration 1
(which was our baseline), our titration 2 and titration 3 had a 0.0006M difference. Additionally, our
average percent error was determined to be 0.67% therefore proving that our results not only were
accurate but also precise.
In order to find the initial concentration of the NaOH base, we first collecting the initial and final
HCl buret readings for all three titrations. The final HCl buret reading was found once the titration
had ended. The end of the titration was easily recognized and determined when the color of the
NaOH base and 2 drops of 1% phenolphthalein indicator mixture changed from a pink solution to a
clear, colorless solution when enough HCl acid was added. After collecting the initial and final HCl
buret readings, we then determined the volume of HCl added by subtracting the initial ... Show more
content on Helpwriting.net ...
Finally, we were then able to solve for the initial concentration of NaOH in each titration by
converting the 20.0 mL NaOH solution used from mL to L, and then plugging it into the molarity
equation along with the mols of NaOH we determined. The initial concentration of NaOH was
found to be 0.0780M in titration 1, 0.0739M in titration 2, and 0.0745M in titration 3. The average
concentration of NaOH was then determined by adding up the initial concentrations of titration 1, 2,
and 3 and then dividing the sum by 3. The average concentration of NaOH was calculated to be
0.0755

Iron Titration Essay
Iron Titration Practical
Introduction into Treating Anaemia with Iron Tablets
Anemia, which is a condition that develops when there is a lack of red blood cells or isn't enough
healthy cells to support the body.
The symptoms are:
 Extreme fatigue
 Pale skin.
 Weakness.
 Shortness of breath.
 Chest pain.
 Headache.
 Dizziness or light–headedness.
Causes of Anaemia can vary depending on the person. Iron Deficiency Anaemia can be caused by
bleeding, for example if a person has lost blood due to injury. The body may also not manufacture
enough healthy red blood cells to support the body. This can be due to not having a healthy or
balanced diet, also if you have a disease that limits the amount of nutrients your body absorbs can be
a cause of Anaemia. (NHS, 2012)
The aim of this Titration is to calculate the amount of IRON in the tablets to see if how much they
are actually benefiting people with Anaemia.
What are the hazards? Who might be harmed and how? What are you already doing? Do you need
to do anything else to control this risk? Action by who? Action by when? Done
Slips and trips Staff and visitors may be injured if they trip over objects or slip on spillages. Rules
are in place to prevent any accidents from tripping or slipping by having all bags under the desks or
away from work bench. You could have a selected room or store where bags can be kept while
experiments for practical's are in progress. Staff and Students Start of Experiment

Titration Lab Report Discussion
Titration what is that you may be asking yourself. Well a titration is a method of analyzing that will
allow you determines the endpoint of a reaction and therefore the quantity of the reactants in the
flask A buret is used to deliver the second reactant to the flask and an indicator or pH Meter is used
to detect the endpoint of the reaction. Also just so you know a titrant is the know solution that is
added and a the analyte is the unkown solution until the reactanc is complete.
In order to do a titration you will need special glassware, burets
Flasks, Beakers, & Graduated Cylinders. Also you will need Pipets,
Repipets, and Volumetric Flasks
Also during a titration lab you will need to know what an equivalance point is in order to complete
the lab. An equivalnce point is when or stoichiometric point, of a chemical reaction is the point at
which chemically equivalent quantities of acid and base have been mixed. In other words, the moles
of acid are equivalent to the moles of base. It can be found by means of an indicator, most often
phenolphthalein. You can find find an equivalance point by being precise and not going to fast it is
recommended that you should do it slowly. ... Show more content on Helpwriting.net ...
We will first start by making a standard solution of NaOH. One way to prepare a standard solution is
to dissolve an accurately massed amount of the substance and dilute it to a measured volume. So
then the concentration can be calculated

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

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 more content
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

Back Titration Lab Report
Abstract The concentration of ethanol in vodka was determined by back titration. A known amount
of excess potassium chromate was added to the vodka sample to convert ethanol into acetic acid by
oxidation. The amount of leftover chromate was determined by titration with iron (II) solution,
prepared from dissolution of ferrous ammonium sulfate. Using the amount of chromate added to the
vodka solution, the amount of chromate reacted was determined and used to find the amount of
ethanol in the sample. A potentiometer in the mV mode was used to create first and second
derivative curves for determining end points. The concentration of ethanol determined was 39.91%,
with standard deviation of 0.13%. The percent error was 0.22%, with the true concentration being
40.00%.
Introduction The consumption of alcoholic beverages, which has increased, has been presenting
several health complications in recent years. The center for disease control explained that the act of
drinking in order to become intoxicated has become more popular recently, and that this has led to
increases in alcohol poisoning, high blood pressure, stroke, liver disease, and neurological damage,
as well as both intentional and unintentional injuries [1]. Although alcoholic beverages contain
many different ingredients, the most significant is ethanol, as it is most commonly responsible for
the health problems mentioned above. This study's primary focus was to identify the concentration
of ethanol in an unknown

In this lab, a titration was performed in order to calculate find the concentration of hydrochloric
acid. In the first part of the lab, the hydrochloric acid was then titrated with sodium hydroxide to
obtain the concentration of the hydrochloric acid. In the second part of the lab, a base and/or antacid
was over titrated with hydrochloric acid. It was then back–titrated using sodium hydroxide solution
to determine how much hydrochloric acid was needed to neutralize the titration. Throughout the first
exercise, the neutralization reaction was performed using both NaOH and HCl. The known
concentration of NaOH from lab 15 was then used again and titrated it into the HCl. This formed
water and sodium chloride. The known concentration of the NaOH and volume is used to determine
the concentration of the HCl. The indicator was phenolphthalein and it was used to titrate sodium
chloride and hydrochloric acid to their equivalence point, which was indicated with a pink color
change. In the second part, a sample was collected in an Erlenmeyer flask and was then titrated with
a buret. The second part of the lab was used to observe the pH of an antacid tablet. an antacid
solution was created by crushing antacids in with an HCl solution and added methyl orange. The
methyl orange is used as an indicator where acids are titrated into a basic solution. The HCl that was
used in the buret had a known concentration, so we were able to use the volume of the known
concentration HCl solution to

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

Oxidation Titration
Introduction/Theoretical Background: A common task in chemistry is the determination of a
substance present in a product. If the product contains a substance that can be oxidized, then it is
possible to determine the number of moles of that substance by titrating the sample with a solution
of a strong oxidizing agent. In this lab, a solution of KMnO4, an oxidizing agent, will be
standardized by titration with a solution containing a known concentration of iron (II) ions, (Fe+).
The concentration of oxalic acid solution will be determined by titration with the MnO4– solution
that had been standardized first. The purpose of this lab is to standardize a solution of potassium
permanganate by redox titration with a standard solution of ... Show more content on
Helpwriting.net ...
Add 20 mL of distilled water to each flask and swirl.
5. Warm the first flask to about 85°C on the hot plate.
6. Immediately titrate this solution with the standardized MnO4 solution from Part 1. Record both
the initial and final buret readings in the Part 2 Data Table.
7. Repeat steps 5 and 6 with the second flask.
Data Table:
| Trial 1 | Trial 2 | Trial 3 | Volume of Fe2+ solution titrated | 10 mL | 10 mL | 10 mL | Initial volume
of MnO4– solution | 3.5 mL | 14.5 mL | 24.8 mL | Final volume of MnO4– solution | 14.5 mL | 24.8
mL | 35.32 mL | Volume of MnO4– added | 11 mL | 10.3 mL | 10.52 mL |
| Trial 1 | Trial 2 | Volume of H2C2O4 solution titrated | 25 mL | 25 mL | Initial volume of MnO4–
solution | 2 mL | 15 mL | Final volume of MnO4– solution | 15 mL | 28 mL | Volume of MnO4–
added | 13 mL | 13 mL |
Calculations:
Balancing:
Reduction: 8H+ + MnO4– + 5e– –> Mn2+ + 4H2O
Oxidation : Fe2+ –> Fe3+ + e–
8H+ + MnO4– + 5e– –> Mn2+ + 4H2O
5Fe2+ –> 5Fe3+ + 5e–
Balanced overall: 8H+(aq) +MnO4–(aq) + 5Fe2+(aq) –> 5Fe3+(aq) + Mn2+(aq) + 4H2O(l)
Normality:

Number of electrons transferred = number of equivalents = 5
Equivalent weight: (39.10g/mol + 54.94g/mol + 4*16.00g/mol)/5 = 31.61g/mol Normality = 5M = 5
* .020M = .100N
Volumes: Trial 1:
FeSO4: 24.60mL – 14.76mL = 9.84mL
KMnO4: 26.20mL – 9.18mL = 17.02mL
Trial 2:
FeSO4: 34.59mL –

Using Acid Base Titration Methods
Abstract
The purpose of this experiment was to utilize acid–base titration methods to standardize NaOH, and
use the standardized NaOH to find the % KHP in an unknown mixture (unknown #46). The
standardization was precise, with the average molarity being 0.0917±0.3662 moles and each trial
varying by only 0.6621 %. The percent mass of KHP in the unknown sample was 55.75 % with a
percent variation between trials of 0.6621 %, which differed by the actual amount by 0.7883%;
showing the experiment was adequate.
Introduction
Potassium Hydrogen Phthalate (KHP) is an acidic salt compound with a molecular weight of 204.22
grams per mole. KHP is a white crystalline powder and is incompatible with strong oxidizing
agents. Titration is used as a method that allows scientists to determine the precise endpoint of a
reaction and is used to determine the precise quantity of reactant in the titration flask. The endpoint
of a reaction is the point at which the mixture is chemically balanced with equivalent quantities of
acid and base. Titration is used in a variety of fields. Titration is used for the mixing of drugs for
medical purposes as well as defines oils and fats in the food industry, etc. The analyte (titrand) is the
solution with an unknown molarity. The reagent (titrant) is the solution with a known molarity that
will react with the analyte. The molar amount of the titrant that is required for a

Titration Lab Report
As mentioned previously the purpose was to use the titration method in order to find molarity, to
find pH. The hypothesis is that very little amount of of HCI is needed to neutralize NaCl. This
would need to be tested through this lab, and will be confirmed through the different series of trials.
Throughout this we also checked our results and see our accuracy through the scientific process.
First in the procedures of this experiment, is we had to neutralize the unknown substance. We had a
beaker filled with 50 mL of sodium–hydroxide (NaOH) and buret full with 20 mL of hydrochloride
(HCl), Figures 2.3 and 2.4. After this we should pour by drop through the buret until the substance
turned a faint pink, Figure 1.2 and 2.2. This will happen because the indicator added to the beaker. If
the color becomes a dark pink the substance has become over–saturated, Figures 1.1 and 1.2. For
our results, which you can see in the table, it only took a few drops of HCI, more precisely 0.2 mL
for the mixture to neutralize, Figure 2.2. Although both of our trials were relatively similar, Jaime ...
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The first part of calculations was finding molarity, which has formula is, molarity equals moles
divided by liters. We already were given the number of moles for HCl. Our results goes as follows:
first trial is the molarity for HCl is 10, second is 9.9, third is 9.8, and fourth is 9.8. Then we
proceeded to the second part of the calculations. The second part is where we figure out the molarity
of NaOH, using the formula of MaVa=MbVb. Ma is the molarity of the acid solution, Va is the
volume of the acid solution, Mb is the molarity of the basic solution (This is the unknown variable
in which we will solve for.), and Vb the volume of the basic solution. After this we plugged–in all of
our information to the variables and solved for Mb. For trial one and three we got 0.1, for trial two
they got 0.3, and for trial four they got

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