CHEM 110L - Experiment 10 It's Back... Titration
pdf
School
University of Phoenix *
*We aren’t endorsed by this school
Course
110
Subject
Chemistry
Date
Apr 3, 2024
Type
Pages
2
Uploaded by HighnessRockOryx35
Experiment 10 It’s Back… Titration Total Points: 40 Student’s Name:
Lab Section: NOTE: You must show your work for all calculations; no work, no credit. Mass of Na
2
S
2
O
3
______2.503g_______ (2 pts) Molarity of Na
2
S
2
O
3
_____0.010073M_________ (Show your calculation) 2.503g x 1mol Na2S2O3/248.18g/1L = 0.010073 (1 pt) Density of Bleach _____0.10262_________ g/mL (Show your calculation) 31.625g-21.363g/100mL = 0.10262 Initial Samples 20 mL Diluted Bleach Treated with KI Volume of Na
2
S
2
O
3 Used During Sample Titration (3 pts) Titrant Added (mL) to: After Starch Added Titrant Added (mL) to: Total Volume Color: Brown Initial Buret Volume, mL Light Orange/ Dark Yellow Dark Blue End Point: Colorless (mL) Sample 1 0 10.15 18.86 29.01 Sample 2 0 8.820 8.080 16.90 1.
Calculate the following for each trial. Make sure to show all your work to receive credit. a.
(2 pts) Moles of Na
2
S
2
O
3 used to titrate the bleach solution. S1: 0.010073M x 0.2901L = 0.00292 moles S2: 0.010073M x 0.1690L = 0.001702 moles b.
(2 pts) Moles of I
2
formed by reaction with bleach. S1: 0.00292mol/2 = 0.001461 moles S2: 0.001702mol/2 = 8.512E-4 moles c.
(4 pts) Molarity of OCl
-
present in the bleach solution. (Remember to account for the dilution of the original sample.) S1: (0.001461mol)(1mol OCl-/1mol I2)/(0.02L)(10)= 0.73054M S2: (8.512E-4)(1mol OCl-/1mol I2)/(0.02L)(10)= 0.42558M d.
(2 pts) Grams of NaOCl present in the bleach (in g/mL): S1: (0.73054M)(74.44g/mol) = 54.382g/L -> 0.054382g/mL S2: (0.42558M)(74.44g/mol)= 31.680g/L -> 0.031680g/mL e.
(2 pts) Percent NaOCl present in the bleach: S1: (0.054382g/mL)/(0.10262g/mL) x 100 = 52.99% S2: (0.031680g/mL)/(0.10262g/mL) x 100 = 30.87%
Experiment 10 It’s Back… Titration Total Points: 40 2.
(6 pts) Use the following equation to answer the following questions: I
2
-starch complex
(aq)
+ 2 S
2
O
2-
3(aq)
→
starch + 2 I
-
(aq)
+ S
4
O
6
2-
(aq) What is being reduced? ____Iodine I2_____________________________ What is the oxidizing agent? ______Iodine I2_______________________ How many electrons are being gamed by each iodine atom? _1 e-__ Post-lab Questions NOTE: You must show your work for all calculations; no work, no credit. 1.
(6 pts) Balance the redox reaction first (it is in basic medium). OCl
-
(aq)
+ CrO
2
-
(aq)
→
Cl
-
(aq)
+ CrO
4
2-
(aq)
2OH- + 3ClO- + 2CrO
2
2- →
3Cl- + 2CrO
4
2- + H2O 2.
(4 pts) A titration experiment is set up to use 0.777M bleach (NaOCl) to analyze CrO
2
-
. If 50.0 mL of the CrO
2
-
(aq)
solution required 12.27 mL of bleach to react to completion, what would you calculation as the molarity of the CrO
2
-
solution? 0.777M x 0.1227L = 0.93379 mol NaCl 2mol/3mol x 0.93379 mol NaCl = 0.635586 mol/0.50L = 0.127M 3.
(6 pts) Excess I
2
can be used to determine vitamin C levels in solution. Vitamin C (ascorbic acid) reacts in the following manner: C
6
H
8
O
6(aq)
+ I
2
→
C
6
H
6
O
6(aq)
+ 2 H
+
(aq)
+ 2 I
-
(aq)
The I
2
that did not
react with ascorbic acid is then determined in a thiosulfate reaction as you did in this experiment. If 22.07 mL of 0.8310 M I
2
was added to a sample containing vitamin C, the unused I
2
required 20.00 mL of 0.143 M S
2
O
3
2-
to react. How many moles of vitamin C were originally present? I2 + 2 S2O3 -> 2I + S4O6 I2= 0.8310M x 0.2207L = 0.1834017 mol S203= 0.143M x 0.2000L = 0.0286mol /2mol = 0.0143mol 0.1834017mol –
0.0143mol = 0.1691017 moles of Vitamin C
Your preview ends here
Eager to read complete document? Join bartleby learn and gain access to the full version
- Access to all documents
- Unlimited textbook solutions
- 24/7 expert homework help
Related Documents
Related Questions
The flask contains 10.0 mL of HCl and a few drops of
phenolphthalein indicator. The buret contains
0.140 M NAOH. It requires 16.4 mL of the NAOH solution
to reach the end point of the titration.
What is the initial concentration of HCl?
concentration:
M HCI
about us
careers
privacy policy
terms of use
contact us
help
docx
DII
F5
PrtScn 8
Home
F9
End
F10
PgUp
F11
F4
F6
F7
arrow_forward
Calculate the Molarity
arrow_forward
3. A student titrates 20.0 ml of an acid solution with 0.500 M NaOH and gets the graph shown below. Determine the concentration of the acid.
arrow_forward
Hello,Can you help me with number 4, 5 ,6 and 7 please?
arrow_forward
A 10.0 mL sample of H₂SO4 is titrated
with 0.685 M NaOH. The initial buret
volume is 0.10 mL and the final buret
volume is 28.92 mL. What is the
concentration (mol/L) of the H₂SO4
sample? Answer to 3 decimal places with
no units.
Your Answer:
Answer
arrow_forward
From the titrations below, calculate the molarity of the NaOH solution in each of the f ollowing? Make sure you balance the equations.
a) NaOH + HCl → NaCl + H2O 32.00 ml of NaOH is required to completely react with 25.00 ml of 0.150 M HCl. ___________
b) NaOH + H2SO4 → Na2SO4 + H2O 42.00 ml of NaOH is required to completely react with 18.00 ml of 0.10M H 2SO4 . __________
arrow_forward
Titration Calculation Practice 4
1. Nitrous acid has a Ka of 4.0 x 104. Calculate the pH at the following places on a titration curve
when 40.00 mL of 0.125 M NANO2 is titrated against 0.200 M HC1.
a. the initial pH
b. the pH at the point when 12.50 mL acid has been added
c. the pH at the point when 15.00 mL acid has been added
arrow_forward
It’s a 4 part question
arrow_forward
25
arrow_forward
55 ml of Na2CO3 solution was titrated with 1.2 M of HCI according to the following reaction
Na2CO3 + 2HCI
2NACI + H2CO3
If 27 ml of HCI are required to completely reacts with Na2CO3 solution
Calculate the molarity of Na2CO3 solution
Select one:
O a. 2.5 M
O b. 0.3 M
O c. 1.8 M
O d. 0.6 M
O e. 0.9 M
arrow_forward
Use the reported molarity For vinegar ( average value) To calculate the percent by mass of HC2H302 and vinegar. Assume the density of the solution is 1.036 g/ml
arrow_forward
Can you please do number 14 III. Can you tell us how to get the volume. I want to know how to calculate the volume in this titration of ch3nh2. See pic.. This is not a graded question as it is a practice question . I am 60 years old and helping my son prepare for the AP exam in a few months. We do questions at the back of the textbook by Zumdahl and Zumdahl
arrow_forward
A 25 ml of Na2CO3 solution was titrated with 0.5 M of
HCl according to the following reaction
Na2CO3 + 2HCI → 2NACI + H2CO3
If 18 ml of HCl are required to completely reacts with NagCO3 solution
Calculate the molarity (The concentration) of Na2CO3
solution
Select one:
a. 0.52 M
b. 0.36 M
c. 0.18 M
d. 0.12 M
arrow_forward
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
QUESTION 5
In an experiment, it requires 35 ml of NaOH to titrate 0.35 g of dissolved KHP (molecular weight = 204.22 g/mol)
to the phenolphthalein end point. Calculate the concentration of NaOH in mol/L .
Оa.4.896 М
O b.0.4896 M
Ос. 0.490 М
O d. 0.0490 M
O e. 1.714 M
arrow_forward
Solid iron(III) hydroxide is added to 635 mL of 0.280 M HCl. The resulting solution is acidic and titrated with 1294 mL of 0.111 M NaOH. What mass of iron(III) hydroxide was added to the HCl?
_____ g
Thanks!
arrow_forward
based on the data tables provided, what is % CH3COOH in vinegar
arrow_forward
If 25.0 mL of 0.451 M NaOH solution is titrated with 0.253 M H2SO4, the flask at the endpoint will contain (besides the indicator phenolphthalein) as the principal components:
Select one:
a. sodium hydroxide, sulfuric acid, and water
b. dissolved sodium sulfate and water
c. sodium hydroxide, sodium sulfate, and water
d. dissolved sodium sulfate, sulfuric acid, and water
e. precipitated sodium sulfate and water
arrow_forward
The graph below represents the titration curve of a
A.
1 M strong acid with 1 M strong base
B.
1 M weak base with 1 M strong acid
C.
1 M strong base with 1 M strong acid
D.
1 M weak base with 1 M weak acid
E.
1 M weak acid with 1 M strong base
arrow_forward
A 30.00 mL sample of a 0.064 M weak acid solution is titrated with 0.068 M strong base. What is the pH after the addition of 12.65 mL of the base? Ka for the acid is 9.16x106.
REPORT YOUR ANSWER TO 2 DECIMAL PLACES. DO NOT INCLUDE UNITS.
Type your answer...
arrow_forward
Suppose a student performed a similar standardization titration experiment. Below is the calculated concentration of NaOH from each of their titrations.
Titration #1
Titration #2
Titration #3
The concentration of NaOH (M)
0.9554
0.9540
0.9551
Using the 3 concentrations, calculate the average concentration of the student's NaOH solution and calculate the ± error in parts per thousand (ppt). Show the complete calculation. Express your final answer in the form of average (with units) ± error in ppt.
arrow_forward
SEE MORE QUESTIONS
Recommended textbooks for you

Chemistry: An Atoms First Approach
Chemistry
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Cengage Learning

Chemistry & Chemical Reactivity
Chemistry
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning

Chemistry for Engineering Students
Chemistry
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Cengage Learning
Related Questions
- The flask contains 10.0 mL of HCl and a few drops of phenolphthalein indicator. The buret contains 0.140 M NAOH. It requires 16.4 mL of the NAOH solution to reach the end point of the titration. What is the initial concentration of HCl? concentration: M HCI about us careers privacy policy terms of use contact us help docx DII F5 PrtScn 8 Home F9 End F10 PgUp F11 F4 F6 F7arrow_forwardCalculate the Molarityarrow_forward3. A student titrates 20.0 ml of an acid solution with 0.500 M NaOH and gets the graph shown below. Determine the concentration of the acid.arrow_forward
- Hello,Can you help me with number 4, 5 ,6 and 7 please?arrow_forwardA 10.0 mL sample of H₂SO4 is titrated with 0.685 M NaOH. The initial buret volume is 0.10 mL and the final buret volume is 28.92 mL. What is the concentration (mol/L) of the H₂SO4 sample? Answer to 3 decimal places with no units. Your Answer: Answerarrow_forwardFrom the titrations below, calculate the molarity of the NaOH solution in each of the f ollowing? Make sure you balance the equations. a) NaOH + HCl → NaCl + H2O 32.00 ml of NaOH is required to completely react with 25.00 ml of 0.150 M HCl. ___________ b) NaOH + H2SO4 → Na2SO4 + H2O 42.00 ml of NaOH is required to completely react with 18.00 ml of 0.10M H 2SO4 . __________arrow_forward
- Titration Calculation Practice 4 1. Nitrous acid has a Ka of 4.0 x 104. Calculate the pH at the following places on a titration curve when 40.00 mL of 0.125 M NANO2 is titrated against 0.200 M HC1. a. the initial pH b. the pH at the point when 12.50 mL acid has been added c. the pH at the point when 15.00 mL acid has been addedarrow_forwardIt’s a 4 part questionarrow_forward25arrow_forward
- 55 ml of Na2CO3 solution was titrated with 1.2 M of HCI according to the following reaction Na2CO3 + 2HCI 2NACI + H2CO3 If 27 ml of HCI are required to completely reacts with Na2CO3 solution Calculate the molarity of Na2CO3 solution Select one: O a. 2.5 M O b. 0.3 M O c. 1.8 M O d. 0.6 M O e. 0.9 Marrow_forwardUse the reported molarity For vinegar ( average value) To calculate the percent by mass of HC2H302 and vinegar. Assume the density of the solution is 1.036 g/mlarrow_forwardCan you please do number 14 III. Can you tell us how to get the volume. I want to know how to calculate the volume in this titration of ch3nh2. See pic.. This is not a graded question as it is a practice question . I am 60 years old and helping my son prepare for the AP exam in a few months. We do questions at the back of the textbook by Zumdahl and Zumdahlarrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- Chemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
- Chemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning

Chemistry: An Atoms First Approach
Chemistry
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Cengage Learning

Chemistry & Chemical Reactivity
Chemistry
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning

Chemistry for Engineering Students
Chemistry
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Cengage Learning