Titration Lab Report
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School
Johns Hopkins University *
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Course
EN.030.206
Subject
Chemistry
Date
Apr 3, 2024
Type
Pages
5
Uploaded by PrivateAardvarkPerson480
Selene Barajas
Period 1
Question:
What is the concentration of acetic acid in each sample of vinegar?
Pre-Lab questions:
1)
NaOH is added to HCl until the color changes at a pH of 7.5. It is found that the
moles of acid equals the moles of base at a pH of 7.
a.
What is the titrant and analyte?
The titrant is the unknown concentration of chemicals. The analyte is a chemical of
known concentration that’s added to the titrant.
b.
What is the endpoint for the reaction?
The endpoint is when there is a color change as a result of the indicator added to the
solution which creates a color change based on the pH of the solution.
c.
What is the equivalent point
The equivalence point is when the moles of the titrant are equal to the moles of the
analyte.
2) Explain how rinsing the reservoir with water instead of the titrant before starting the
investigation will affect the calculated unknown molarity of the titrate. (Look in procedure
for answer)
By rinsing the reservoir with water instead of the titrant before starting the investigation will alter
the titrant concentration and result in inaccurate calculations.
3. Explain why there is a steep slope in a section of the titration curve and explain how it
can be used in calculations.
There is a steep slope in a section of the titrant curve because it shows the lowest
concentration, slowing down the reaction which results in a steep slope in the center of the
curve.
4. What types of data need to be collected to perform molarity calculations of the
unknown?
The types of data needed to perform molarity calculations of the unknown are the molarities and
volumes of the obscure corrosion. Also, necessary to have the initial and final volumes of the
equivalence point.
5. Why do you think it is important to know the exact concentration of acetic acid in apple
cider vinegar?
I think it is important to know the exact concentration of acetic acid in vinegar to be able to
calculate additional molarity.
3) Procedure
1)
calibrate the drop counter in order to get the volume of the titrant
2)
rinse the 10 mL cylinder, then place the drop counting onto it.
3)
We then need to add 10 mL of distilled water to the reservoir. 4
4)
We then open the valve in order to record the drops that are falling. 5
5)
We then need to record the volume of the water and the number of drops. 6
6)
We then need to create our NaOH solution.
4) Materials
Materials needed are a Labquest, Vernier Drop Counter, Vernier pH Sensor, Distilled water, Ring
stand, 0.03 M NaOH solution, reagent reservoir, Magnetic stirrer and bar, Utility clamp,
Unknown HCl Unknown acetic acid, beaker, Buret clamp, 3 beakers, 2 graduated cylinders, a
pipet, and two types of vinegar.
5) Safety Concerns
Some safety concerns are acids touching and damaging the skin, eyes, and other important body
parts. Therefore, it is important to wear our safety goggles when doing the lab. NaOH is also
poisonous if consumed, so it's recommended that we take these extra steps to help in our safety.
6) What data are you looking for?
The data we are looking for is the amount of acetic acid in the apple cider vinegar and the HCI
solution.
7) Data Table
Burette Data HCI
Trials
Initial
NaOH
volume
Final
NaOH
volume
Volume of
NaOH
added
Moles of
HCI
HCI
pH at
equivalen
ce point
1
30 mL
28 mL
2 mL
0.002
0.080 M
7.89 pH
2
25 mL
21 mL
4 mL
0.0004
0.080 M
8.05 pH
8) Calculations
9) Titration curve picture for each expt.
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Related Questions
STANDARDIZATION OF A SODIUM
HYDROXIDE SOLUTION
PRE-LABORATORY
EXPERIMENT 10
QUESTIONS
NAME
DATE
1. What is the purpose of this experiment?
2. A sample of KHP has a mass of 2.345 g is used for a titration, how many moles of KHP is this
sample?
3. How many moles of NaOH would be needed to reach the endpoint of this titration with sample of
KHP from the previous question?
4. If the initial volume of the NaOH in the burette was 0,50 mL
and the final volume is shown to the right, what is the volume of
NaOH used in this titration?
18
19
5. What is the concentration of the NaOH solution used in this titration?
EXPERIMENT 10
155
arrow_forward
QUESTION 9
Acid-Base Titration In this experiment, an indicator called phenolphthalein is used to signal the endpoint of the titration (when the acid has been fully neutralized by the
base). The indicator is colorless in acidic solution and pink in basic solution. During the titration, the pink color will appear and then disappear quickly with each addition
of base (titrant).
If a student is having trouble seeing the pink color in the sample flask, what can be done to help them see the color more clearly?
Experiment - Acid-Base Titration.pdf
O Remove safety goggles to get them out of the way.
O Add several more drops of indicator - the more the better!
O Place a piece of white paper or a white paper towel beneath the sample flask.
O Place something dark beneath the sample flask.
arrow_forward
EXPERIMENT 10
PRE-LABORATORY
QUESTIONS
STANDARDIZATION OF A SODIUM
HYDROXIDE SOLUTION
NAME
DATE
1. What is the purpose of this experiment?
2. A sample of KHP has a mass of 2.345 g is used for a titration, how many moles of KHP is this
sample?
3. How many moles of NaOH would be needed to reach the endpoint of this titration with sample of
KHP from the previous question?
4. If the initial volume of the NaOH in the burette was 0.50 mL
and the final volume is shown to the right, what is the volume of
NaOH used in this titration?
19
5. What is the concentration of the NaOH solution used in this titration?
EXPERIMENT 10
155
arrow_forward
A Question 13 (1 point) Retake question
*A buffer solution is prepared by adding 6.02 mL of 1.11 M HI to 192.0 mL of 0.11 M
methylammine solution. The buffer is allowed time to establish. Then, 0.005 mol of
a strong acid is added. What is the pH?
Round your answer to 2 decimal places.
Your Answer:
Answer
arrow_forward
II only
O both I & II
ОШ only
QUESTION 13
Consider an acid-base titration in which the base is dispensed from a burette into a flask containing an acid. If any drops of
the base adhere to the inner walls of the flask, but do not actually mix with the solution, the calculated acid concentration
would be
O the same as the actual value.
O lower than the actual value.
O higher than the actual value.
Need more information
Click Save and Submit to save and submit, Click Save All Answers to save all answers.
Save Al
arrow_forward
C. Titration of acid by a base
Standardization of NaOH
Volume of NaOH
Mass of KHP
Initial buret
Final buret
Trial
used
Molarity of NaOH
(g)
reading (mL)
reading (mL)
(mL)
(1)
(2)
(3)
(4)
(5)
1.2075
0.7
25
24.3
0.243
(6)
(7)
(8)
(9)
(10)
1.2062
16.4
40.9
24.49
0.2412
arrow_forward
7) What is the molarity of a 12.46 mL sulfuric acid solution if 18.22 mL of 0.100 M potassium hydroxide is required to reach the endpoint as indicated by a titration .
arrow_forward
based on the data tables provided, what is % CH3COOH in vinegar
arrow_forward
In titration, what solution is placed inside the burette?
Group of answer choices
stock solution
analyte
diluted solution
titrant
arrow_forward
O II only
QUESTION 5
In the experiment "Preparation and Standardization of a Sodium Hydroxide Solution", why was the burette rinsed with
NaOH before filling it to "zero" for the titration?
To remove any residual liquids from the burette
O To check that the burette works properly
To remove any air bubbles and fill the tip of the burette
All of the above
QUESTION 6
Save A
Click Save and Submit to save and submit. Click Save All Answers to save all ansuers.
arrow_forward
I need help with question 3?
arrow_forward
5
arrow_forward
1
2
3
4
Questions 1-4 refer to the same strong acid/strong base (SA/SB) titration.
A 25.00 mL solution of 0.200 M hydroiodic acid (HI) is being titrated with 0.200 M sodium hydroxide (NaOH). What is the initial solution pH (when 0.00 mL of titrant have been
added) (Two decimal places)
Type your answer...
Questions 1-4 refer to the same strong acid/strong base (SA/SB) titration.
A 25.00 mL solution of 0.200 M hydroiodic acid (HI) is being titrated with 0.200 M sodium hydroxide (NaOH). What is the solution pH (when 15.00 mL of titrant have been
added? (Two decimal places)
Type your answer...
Questions 1-4 refer to the same strong acid/strong base (SA/SB) titration.
A 25.00 mL solution of 0.200 M hydroiodic acid (HI) is being titrated with 0.200 M sodium hydroxide (NaOH). What is the solution pH at the equivalence point? (Two decimal
places)
Type your answer...
Questions 1-4 refer to the same strong acid/strong base (SA/SB) titration.
A 25.00 mL solution of 0.200 M hydroiodic acid (HI) is…
arrow_forward
YOU DON'T NEED TO ANSWER ALL THE QUESTIONS ALL I NEED HELP WITH IS QUESTIONS 4 and 5. I got d, e, e for the 1st 3 questions if that helps you, but you don't need to worry about questions 1-3 I just included them in case it helps you.
1.What reagent is used as the indicator for the neutralization?
a)citric acid
b)sodium hydroxide
c)sodium citrate
d)phenolphthalein
2.
What is the mole ratio of NaOH to citric acid for this neutralization reaction?
a)2 mole NaOH/1 mole citric acid
b)1 mole NaOH/1 mole citric acid
c)1 mole NaOH/2 mole citric acid
d)1 mole NaOH/3 mole citric acid
e)3 mole NaOH/1 mole citric acid
3.If 35.00 mL of 0.1104 M NaOH were used to reach the neutralization point, how many moles of NaOH were dispensed?
a)3.154 x 10-3 mol NaOH
b)1.104 x 10-4 mol NaOH
c)258.8 mol NaOH
d)3.864 x 10-3 mol NaOH
4. Using the above mole ratio, convert the moles of NaOH in the previous question to moles of citric acid.
a)1.288…
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How many mL of 16 N HCl is needed to make a 0.3 N solution from a 500 mL solution of 0.15 N HCl to be used as titrant?
This is titration
arrow_forward
QUESTION 8
A 0.9600 M NAOH solution was diluted with a factor of 4.
Then the diluted solution of NaOH was titrated against an unknown acld.
The volumes of NaOH(aq) titrated are shown in the table below.
Volumes of NaOH(aq):
Rough
titration
First
titration
Third
titration
Second
Third
titration
titration
Final burette reading:
(mL)
Initial burette reading:
(mL)
19.00
34.05
20.86
36.01
23.57
19.00
19.07
5.76
21.02
8.54
The molarity of the unknown acid is 0.08108 M and the volume of the unknown acid used in
each titration is 14.80 mL.
Was the unknown acid monoprotic, diprotic or triprotic? Show your calculations and
reasoning.
(i)
arrow_forward
Question: Comment on the solubility of the two dyes in water. In your answer consider intermolecular bonds and their relative strengths.
Solubility of dye C:
Solubility of dye D:
arrow_forward
Graph the data by plotting the pH (y-axis) versus the amount of citricacid solution added (x-axis). Make sure that you label the axes of thegraph
Titration Data
Titration of NaOH
Volume Citric Acid Solution Added (mL)
pH
0.0 mL (initial)
7.8
0.5 mL
7.8
1.0mL
7.2
1.5 mL
7.1
2.0 mL
6.9
2.5 mL
6.8
3.0 mL
6.7
3.5 mL
6.6
4.0 mL
6.5
4.5 mL
6.4
5.0 mL
6.2
5.5 mL
6.1
6.0 mL
5.9
6.5 mL
5.9
7.0 mL
5.8
arrow_forward
Suppose a student wants to determine the color change interval of an unknown indicator. Her results are given in the table.
Tube #
pH Unknown indicator
4
6.39
red
7.11
red
6.
7.87
purple
7
8.81
purple
8.
9.07
blue
9
10.10
blue
What is the interval of the unknown indicator?
The color change interval is between pH 7.11 and pH 7.87.
The color change interval is between pH 7.11 and pH 9.07.
The color change interval is between pH 9.07 and pH 10.10.
The color change interval is between pH 6.39 and pH 10.10.
O O
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1. At what point (how many milliters of added acid) was the solution in beaker “B” neutralized?
Neutralization of Acids and Bases
Test Data:
Table 2: Initial pH Test Results
Container
Substance in Container
pH using the pH meter
A
distilled water
6.8
B
0.5 g sodium bicarbonate with distilled water
7.5
C
vinegar
2.3
Table 3: Neutralization
Amount of Acid Added (mL)
pH using the pH Meter
1 mL
7.5
2 mL
7.3
3 mL
7.2
4 mL
7.2
5 mL
7.2
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Please answer the 3 boxes for ph
arrow_forward
Questions:
1. Why does the tip of your buret need to be free of air bubbles?
2. Explain why the volume of water did not need to be exactly measured or recorded.
3. Define the endpoint of a titration.
4. What is a standard solution? Why is a standard solution necessary for titration?
5. A student starts a titration without phenolphthalein in the Erlenmeyer flask. The student
realizes the mistake and adds the phenolphthalein during the titration. Once the
phenolphthalein is added, the solution in the Erlenmeyer flask remains colorless. Can the
results of this titration be used? Concisely explain.
6. Write a balanced equation for the neutralization of hydrobromic acid with potassium
hydroxide.
7. What is the molarity of a 12.46 mL sulfuric acid solution if 18.22 mL of 0.100 M potassium
hydroxide is required to reach the endpoint as indicated by a titration.
43
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3. Sprite does not contain phosphoric acid. Only sodas that are dark in color contain this acid. sodas such as Sprite contain citric acid, sugar, and carbonaled water Design a simple experiment to determine the concentration of citric acid in SpriteProvide a de tailed procedure
arrow_forward
When performing a titration in the lab, which equipment is not used?
1. burette
2. pipette
3. funnel
4. watch glass
5. Erlenmeyer flask
arrow_forward
Questions 11-14 refer to the same strong base/strong acid (SB/SA) titration.
A 15.00 mL solution of 0.100 M sodium hydroxide (NaOH) is being titrated with 0.250 M hydrobromic acid (HBr). What is the solution pH before the titration begins?
(Two decimal places)
Type your answer...
arrow_forward
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Related Questions
- STANDARDIZATION OF A SODIUM HYDROXIDE SOLUTION PRE-LABORATORY EXPERIMENT 10 QUESTIONS NAME DATE 1. What is the purpose of this experiment? 2. A sample of KHP has a mass of 2.345 g is used for a titration, how many moles of KHP is this sample? 3. How many moles of NaOH would be needed to reach the endpoint of this titration with sample of KHP from the previous question? 4. If the initial volume of the NaOH in the burette was 0,50 mL and the final volume is shown to the right, what is the volume of NaOH used in this titration? 18 19 5. What is the concentration of the NaOH solution used in this titration? EXPERIMENT 10 155arrow_forwardQUESTION 9 Acid-Base Titration In this experiment, an indicator called phenolphthalein is used to signal the endpoint of the titration (when the acid has been fully neutralized by the base). The indicator is colorless in acidic solution and pink in basic solution. During the titration, the pink color will appear and then disappear quickly with each addition of base (titrant). If a student is having trouble seeing the pink color in the sample flask, what can be done to help them see the color more clearly? Experiment - Acid-Base Titration.pdf O Remove safety goggles to get them out of the way. O Add several more drops of indicator - the more the better! O Place a piece of white paper or a white paper towel beneath the sample flask. O Place something dark beneath the sample flask.arrow_forwardEXPERIMENT 10 PRE-LABORATORY QUESTIONS STANDARDIZATION OF A SODIUM HYDROXIDE SOLUTION NAME DATE 1. What is the purpose of this experiment? 2. A sample of KHP has a mass of 2.345 g is used for a titration, how many moles of KHP is this sample? 3. How many moles of NaOH would be needed to reach the endpoint of this titration with sample of KHP from the previous question? 4. If the initial volume of the NaOH in the burette was 0.50 mL and the final volume is shown to the right, what is the volume of NaOH used in this titration? 19 5. What is the concentration of the NaOH solution used in this titration? EXPERIMENT 10 155arrow_forward
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- 7) What is the molarity of a 12.46 mL sulfuric acid solution if 18.22 mL of 0.100 M potassium hydroxide is required to reach the endpoint as indicated by a titration .arrow_forwardbased on the data tables provided, what is % CH3COOH in vinegararrow_forwardIn titration, what solution is placed inside the burette? Group of answer choices stock solution analyte diluted solution titrantarrow_forward
- O II only QUESTION 5 In the experiment "Preparation and Standardization of a Sodium Hydroxide Solution", why was the burette rinsed with NaOH before filling it to "zero" for the titration? To remove any residual liquids from the burette O To check that the burette works properly To remove any air bubbles and fill the tip of the burette All of the above QUESTION 6 Save A Click Save and Submit to save and submit. Click Save All Answers to save all ansuers.arrow_forwardI need help with question 3?arrow_forward5arrow_forward
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