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Lab S. Acids and Bases: Titrations
Jayden Podmoroff 17122912
Partner: Miller
Lab performed: Feb 15, 2019
Chem 123 L22
TA: Sydney Fearnley
Lab Submitted: Feb 29, 2019
1
Introduction:
The purpose of this experiment was to perform different acid-base titrations and observe the use of
indicators in the titrations. Conducting this experiment will further the development skills in plotting
graphical data and graphical interpretation.
A titration is defined as a technique that uses a solution with a known concentration is used to find the
unknown concentration of another solution.
The titrations involved in Lab S are all acid-base titrations,
where two both a strong (HCl) and weak (CH
3
COOH) acid are titrated with a basic solution (NaOH) of
known concentration. The chemical reaction of the titration varies depending on whether the acid and
base involved is strong or weak. The reaction for strong acid and strong base titrations are given in
reaction (I) while the reaction for weak acid and strong base titrations are given in reaction (II).
1
The
corresponding reactions are given below.
1
H
3
O
+
+ OH
-
2H
2
O
(I)
HA + OH
-
A
-
+ H
2
O (II)
Once the acid has been fully neutralized by the base, the unknown concentration can be found using the
total volume of base added and the balanced chemical equation reaction of the titration.
The data obtained from a titration can be plotted as a graph into what is called a titration curve, where
pH is plotted as a function of volume of titrant added. The equivalence point can be found using a
titration curve graph by finding the average of the end point and start point, which is asked of Part A
(intersecting points between tangent lines and slope of pH jump).
2
Part B seeks to find the endpoint of different titrations with the use of indicators. Indicators are weak
acids or bases that are used to monitor the progress of a titration through colour change at certain pH
2
levels. The appropriate indicator must be used for the appropriate titration based off pH range in order
to yield accurate results. The change in colour occurs when the indicator changes into its conjugate acid
or base form through removal of a proton, using the equation (III) below.
3
HIn + OH
-
H
2
O + In
-
(III)
Colour I
Colour II
Procedure:
The procedure of Lab S given by the First Year Chemistry Lab Manual
4
was followed as described below.
Part A of Lab S required the use of a pH meter to find the equivalence point. First, the pH meter was
calibrated by following steps described in the lab manual. A burette was attached to a retort stand and
filled with an appropriate amount of standardized NaOH solution with concentration 0.105 M. 10.00 mL
of the hydrochloric acid solution was pipetted into a 100 mL beaker along with about 20 mL of distilled
water. The beaker was placed on a magnetic stirrer and a magnetic stirring flea was placed inside the
beaker. The initial pH of the solution was recorded using the pH meter.
The standardized NaOH solution was titrated very carefully with the HCl solution. The NaOH was added
in small increments ranging from 1 mL to 0.1 mL and the reading from the pH meter was recorded after
each corresponding addition. Smaller increments were used when finding the equivalence point of the
titration and larger increments were used nearing the end of the titration.
After completion of the titration, the exact same steps were repeated with the exception of using a
acetic acid solution instead of an HCl solution. 5.00 mL of acetic acid was pipetted into a 100 mL beaker
along with about 20 mL of distilled water to create the solution.
3
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Related Questions
In Experiment 4, we used titration to determine the total acid content of samples, which we reported in
terms of molarity. Reporting acidity through pH measurements is quite different, in that we can only
measure the amount of the acid in its ionized form. You were tasked to investigate a clear aqueous
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A. Calculate the molarity of the acid using the titration data.
B. If we assume that the titrated unknown is a strong acid, predict the pH of the sample.
C.…
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H2X is the base and HX is the conjugate acid
QUESTION 12
Which of the following could not be a Bronsted- Lowry Acid?
O NH4
O NH3
О Н20
BЕЗ
QUESTION 13
What volume of 0.0347 M Ba(OH)2 is needed to completely react wit
2 HC + Ba(OН)2
— ВаСl2 + 2 H20
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In the experiment, we used titration to determine the total acid content ofsamples, which we reported in terms of molarity. Reporting acidity through pHmeasurements is quite different, in that we can only measure the amount of theacid in its ionized form. You were tasked to investigate a clear aqueous solutionof an unknown monoprotic acid. You decided to use two methods togather data.Method 1 – TITRATION: A 10. mL aliquot of the sample was diluted with 25 mLdistilled water. Two drops of phenolphthalein were added and then it was titrated3.54 mL of 0.048 M standardized NaOH to the endpoint.Method 2 – pH STRIP: You took 1 mL of the sample and used a pH strip toestimate the pH, which turned out to be around 3.3. Another 1 mL of the samplewas diluted with 9 mL of water. The pH was taken again and is now around 3.8.a) Calculate the molarity of the acid using the titration data.b) If we assume that the titrated unknown is a strong acid, predict thepH of the sample.c) Using pH strip results,…
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Question Completion Status:
Using the data given, fill in the following table of ion concentrations and pH values. Remember that K = 1.0 × 10-
14
Solution
[H3O*]
[OH']
pH
1
3.67
6.3×10-5 M
3
7.6x10-6 M.
4.
3.8x10-14 M
6.00
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Calculate the pH at the equivalence point for the following titration: 0.35 M HCOOH versus
0.35 M NaOH.
points
Gui
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A) Please fill in the first blank with the word "acidic", "basic" or "nearly neutral".
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Hint: IF you need Ka to solve this problem, you must calculate it from the information provided
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When 0.77 M ammonium chloride salt hydrolyzes in water, the solution will be
with a pH =
Kb (NH3) = 1.8 x 105
%3D
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*Photo included below
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Let's determine the concentration and the pH of a H2CO3 solution that was prepared by using standard NaOH solution with a concentration of 0.125 M using the following data.
Trial 1
Trial 2
Trial 3
Volume of H2CO3
19.80 mL
20.05 mL
19.95 mL
Initial volume of NaOH (mL)
1.90
16.88
31.98
Final volume of NaOH (mL)
16.88
31.98
47.00
What is the Molarity and the pH of the H2CO3 ?
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Name:
Date:
Experiment # 11: Acid-Base Titration: Standardization of NaOH
Data and results
Data table *Remember to include units
Trial 1
Trial 2
Trial 3
Trial 4
Mass of KHC8H4O4 (KHP)
Initial buret reading (NaOH)
Final buret reading (NaOH)
Volume of NaOH used
Results table
Trial 1
Trial 2
Trial 3
Trial 4
Moles of KHP
Moles of NaOH
Volume of NaOH (L)
Molarity of NaOH
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Sample calculation:
In the space below show complete calculations for moles of KHP and molarity of NaOH using data from
TRIAL 2 only. Include formulas and units.
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Round your answer to1 decimal place.
pH =
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= 48
= 49
50
51
= 52
= 53
= 54
= 55
= 56
57
- 58
- 59
For a certain acid pK, = 6.79. Calculate the pH at which an aqueous solution of this acid would be 0.32% dissociated. Round your answer to 2 decimal places.
%3D
pH = 0
%3D
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