Question

For your titrations of the hydrogen peroxide in a new bottle, record the following data in...

For your titrations of the hydrogen peroxide in a new bottle, record the following data in the table below. If you had to perform three fine titrations, disregard the one that was different.

initial volume of .2M KMnO4 in the burette (mL) 50.00
volume of hydrogen peroxide solution added to the flask (mL) 10.00
volume of .2M KMnO4 dispensed in the coarse titration (mL) 19.06
volume of .2M KMnO4 dispensed in the first fine titration (mL) 18.02
volume of .2M KMnO4 dispensed in the second fine titration (mL) 18.01

Data Analysis

For your titrations of the hydrogen peroxide in a new bottle, calculate the molarity of the new hydrogen peroxide solution using the average volume of permanganate solution dispensed in the fine titrations. If you had to perform three fine titrations, disregard the one that was different.

Calculate the mass percent of the hydrogen peroxide in the new bottle. The molar mass of H2O2 is 34.0147 g/mol and the density of the solution is 1.000 g/mL.

Experiment 2: Titrate the Hydrogen Peroxide in an Old Bottle

Lab Results

For your titrations of the hydrogen peroxide in a new bottle, record the following data in the table below. If you had to perform three fine titrations, disregard the one that was different.

initial volume of .2M KMnO4 in the burette (mL) 50.00
volume of hydrogen peroxide solution added to the flask (mL) 10.00
volume of .2M KMnO4 dispensed in the coarse titration (mL) 13.37
volume of .2M KMnO4 dispensed in the first fine titration (mL) 12.63
volume of .2M KMnO4 dispensed in the second fine titration (mL) 12.65

Data Analysis

For your titrations of the hydrogen peroxide in an old bottle, calculate the molarity of the old hydrogen peroxide solution using the average volume of permanganate solution dispensed in the fine titrations. If you had to perform three fine titrations, disregard the one that was different.

Calculate the mass percent of the hydrogen peroxide in the old bottle. The molar mass of H2O2 is 34.0147 g/mol and the density of the solution is 1.000 g/mL.

Homework Answers

Answer #1

Average volume of KMnO4 = (18.01+18.02)/2

= 18.015 ml

Molarity of KMnO4 = 0.2 M

Milli-Moles of KMnO4 = 0.2 * 18.015

Consider Molarity of H2O2 = x M

Following is the balanced reaction

2 KMnO4 + 5 H2O2 + 3 H2SO4 ----> 2 MnSO4 + K2SO4 + 5 O2 + 8 H2O

Hence ( Moles of KMnO4 )/2 = (Moles of H2O2 )/5

5* moles of KMnO4 = 2* Moles of H2O2

  5 * 0.2 * 18.015 = 2 * x *10

x= 0.9 M

Hence Molarity of H2O2 is 0.9M

Now mass%

1000 ml of H2O2 solution contain 0.9 moles of H2O2 . Hence wt of H2O2 =0.9 * 34 = 30.6 gm

wt of H2O2 sloution = 1000 gm

  

mass % of H2O2 = 3%

  

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Redox titrations are used to determine the amounts of oxidizing and reducing agents in solution. For...
Redox titrations are used to determine the amounts of oxidizing and reducing agents in solution. For example, a solution of hydrogen peroxide, H2O2, can be titrated against a solution of potassium permanganate, KMnO4. The following equation represents the reaction: 2KMnO4(aq)+H2O2(aq)+3H2SO4(aq)→3O2(g)+2MnSO4(aq)+K2SO4(aq)+4H2O(l) A certain amount of hydrogen peroxide was dissolved in 100. mL of water and then titrated with 1.68 M KMnO4. What mass of H2O2 was dissolved if the titration required 21.8 mL of the KMnO4 solution?
A volume of 60.0 mL of aqueous potassium hydroxide (KOH) was titrated against a standard solution...
A volume of 60.0 mL of aqueous potassium hydroxide (KOH) was titrated against a standard solution of sulfuric acid (H2SO4). What was the molarity of the KOH solution if 11.7 mL of 1.50 M H2SO4 was needed? The equation is 2KOH(aq)+H2SO4(aq)→K2SO4(aq)+2H2O(l) Express your answer with the appropriate units. Hints Part B Redox titrations are used to determine the amounts of oxidizing and reducing agents in solution. For example, a solution of hydrogen peroxide, H2O2, can be titrated against a solution...
2) The active agent in many hair bleaches is hydrogen peroxide. The amount of H2O2 in...
2) The active agent in many hair bleaches is hydrogen peroxide. The amount of H2O2 in 13.2−g of hair bleach was determined by titration with a standard potassium permanganate solution: 2 MnO4−(aq) + 5 H2O2(aq) + 6 H+(aq) → 5 O2(g) + 2 Mn2+(aq) + 8 H2O(l) (a) For the titration, how many moles of MnO4− were required if 32.3 mL of 0.195 M KMnO4 was needed to reach the end point? Write your answer to the correct number of...
Procedure Experiment 1: Standardize an NaOH Solution Using Benzoic Acid as Primary Standard Part 1: Prepare...
Procedure Experiment 1: Standardize an NaOH Solution Using Benzoic Acid as Primary Standard Part 1: Prepare the NaOH Solution Take a 250 mL volumetric flask from the Containers shelf and a balance from the Instruments shelf and place them on the workbench. Zero the mass of the volumetric flask on the balance. Take sodium hydroxide from the Materials shelf and add 1 g to the flask. Record the mass from the balance display. Place the volumetric flask on the workbench....
A new flow injection analysis enzymatic procedure for determining hydrogen peroxide in water was compared with...
A new flow injection analysis enzymatic procedure for determining hydrogen peroxide in water was compared with a conventional method involving redox titration with potassium permanganate by applying both methods to samples for peroxide for pharmaceutical use. The data below gives the amount of hydrogen peroxide found in mg ml-1. Each value is the mean of four replicate measurements. Sample No.                 Enzymatic Method                 Permanganate Method 1                                  31.1                                         32.6 2                                  29.6                                         31.0 3                                  31.0                                         30.3 Test whether the results obtained by the...
Below is the background info for the lab assignment. The 4 blank boxes are the questions...
Below is the background info for the lab assignment. The 4 blank boxes are the questions I would like answers too. The end point for the fine titration was 35.90 mL in the burette when the solution turned bright green again. And the coarse titration I got 35.36mL as the end point. 35.9 mL is exact in case you need that info. Thanks! Background In this lab, we will determine the amount of alcohol (ethanol), C2H5OH, in a commercial vodka...
1) Describe an example of each of the following that may be found of your kitchen:...
1) Describe an example of each of the following that may be found of your kitchen: Explain how your choice falls into this category, and if there is a chemical name or symbol for it, provide that as well. Provide a photo of your example with your ID card in it. a) a compound b) a heterogeneous mixture c) an element (symbol) Moving to the Caves… Lechuguilla Caves specifically. Check out this picture of crystals of gypsum left behind in...