A titration of 2.00 ml of hydrogen peroxide solution (Mw = 34.01 g / mol) used 35.57 ml of 0.1 N (0.02 M) potassium permanganate (Mw = 158.03 g / mol). a) Write down the coordinated redox reaction between hydrogen peroxide and potassium permanganate. b) How many moles of potassium permanganate does 1 mole of hydrogen peroxide correspond to? c) Based on the redox reaction, calculate the percentage of the sample that consists of hydrogen peroxide. d) Calculate the percentage of hydrogen peroxide in the solution when 1.00 ml of 0.1 N potassium permanganate corresponds to 1,701 mg of hydrogen peroxide

A titration of 2.00 ml of hydrogen peroxide solution (Mw = 34.01 g / mol) used 35.57 ml of 0.1 N (0.02 M) potassium permanganate (Mw = 158.03 g / mol). a) Write down the coordinated redox reaction between hydrogen peroxide and potassium permanganate. b) How many moles of potassium permanganate does 1 mole of hydrogen peroxide correspond to? c) Based on the redox reaction, calculate the percentage of the sample that consists of hydrogen peroxide. d) Calculate the percentage of hydrogen peroxide in the solution when 1.00 ml of 0.1 N potassium permanganate corresponds to 1,701 mg of hydrogen peroxide

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Related questions

Q: How many coulombs will it take to plate out 15 g of Fe from a solution of FeCl2?

Q: With respect to the following unbalanced redox equation that takes place in a basic environmnet,…

A: In the given question we have to balance the given chemical equation, Zn (s) + NO3- (aq) -->…

Q: (1) Identify each of the following half-reactions as either an oxidation half-reaction or a…

Q: or Questions 11-16: Balance the following oxidation-reduction reaction in acidic conditions using…

A: Redox reaction is the chemical reaction in which oxidation and reduction reactions take place…

Q: 1) Using the line notation and the half-reaction information provided, answer the following…

A: In this question, we have to find out the correct answer of all given problems by the help of "Redox…

Q: O Macmillan Learning Consider each of the following questions related to the Redox Titration Lab.…

A: 2KMnO4 + Na2C2O4 → K2C2O4 + 2NaMnO4• For Na2C2O4 solution,Concentration of Na2C2O4 solution =…

Q: What is the normality of a K,Cr20, solution prepared by dissolving 5.00 g of K2Cr20, in 200 mL of…

A: Given unbalanced equation is Cr2O7 -2 + SO3-2 → Cr+3 + SO4-2 Balance the reaction 1 Cr2O7…

Q: With respect to the following unbalanced redox equation that takes place in an acidic environment,…

A: Give reaction BrO3- (aq) + N2H4 (g) ---> Br- (aq) + N2 (g)

Q: How many g of Ag form when 10.0 A are passed through molten AgCl for 35.0 minutes?

A: Given: Time (t)=35 minutes=35×60 s=2100 sCurrent (I)=10.0 A To find: Mass of Ag

Q: In some old European churches, the stained-glass windows have so darkened from corrosion and age…

A: In some old European churches, the stained glass windows have so darkened from corrosion and age…

Q: Perform the steps above to balance the redox reaction (shown again below). Fill in each blank with…

Q: 2. Balance the following redox reactions that occur under basic conditions. -2 -2 a. SO3² (aq) + Cl₂…

A: The Redox reactions are those where reduction and oxidation occurs simultaneously. Oxidation is…

Q: Balance the reaction between Mn2+ and H3ASO4 to form MnO₂ and H3ASO3 in acidic solution. When you…

Q: What is the coefficient for the following reactants and products when the redox equation below is…

A: Balanced equation: balanced equation can be define as the reaction in which number of atoms of all…

Q: 0.11 mol sodium chloride and 0.122 mol magnesium chloride are added into water to make 1 L solution.…

A: A strong electrolyte is one which completely dissociates or ionizes in a given solution. On the…

Q: Fe3+ + 1e- → Fe2+ Eo = 0.77 V Sn4+ + 2e- → Sn2+ Eo = 0.15 V Fe2+ + 2e- → Fe…

Q: A solid sample containing some Fe2+ weighs 2.360 g. It required 36.44 mL 0.0244 M KMnO4 to titrate…

A: To calculate the moles of MnO4– used in the titration, we use the formula:Moles = Volume ×…

Q: a) (i) Write a half equation to show the conversion of MnO4 toMn2+. (ii) Write a half equation to…

A: Hello. Since your question has multiple parts, we will solve first question for you. If you want…

Q: A solid sample containing some Fe2+ weighs 2.360 g. It required 36.44 mL 0.0244 M KMnO4 to titrate…

A: Given : Mass of sample having Fe2+ used = 2.360 g Concentration of KMnO4 used = 0.0244 M And volume…

Q: Balance the following oxidation-reduction reaction in basic solution. Hint: Oxygen oxidation number…

A: Given: Cr2O72-(aq)+H2O2(aq)→Cr+3(aq)+O2(g) Calculation for oxidation state of Cr in Cr2O72-: let x…

Q: who are the reducing and oxidizing agent in the following reaction: H20 2 Cu(OH), + 4C,H¿0̟ → µ –…

A: In this question, we will determine the Oxidising agent and reducing agent. How we can determine the…

Q: A total of 1.707 F of electricity (1 F = 1 mol e¯) was required to electrodeposit all of the Zn and…

A: Answer:This question is based on Faraday's law of electrolysis. To deposit each mole of Zinc ion and…

Q: The solubility product for Cu(OH)₂(s) is 1.6x 10-19. Calculate the value of 8° for the following…

Q: 1.Which of the following would be the reason the following reaction occurs? Mg + Zn(NO33)22 --> Zn…

Question

A titration of 2.00 ml of hydrogen peroxide solution (Mw = 34.01 g / mol) used 35.57 ml of 0.1 N
(0.02 M) potassium permanganate (Mw = 158.03 g / mol).
a) Write down the coordinated redox reaction between hydrogen peroxide and potassium
permanganate.
b) How many moles of potassium permanganate does 1 mole of hydrogen peroxide correspond
to?
c) Based on the redox reaction, calculate the percentage of the sample that consists of hydrogen
peroxide.
d) Calculate the percentage of hydrogen peroxide in the solution when 1.00 ml of 0.1 N potassium
permanganate corresponds to 1,701 mg of hydrogen peroxide

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

Step 2

Step 3

Step 4

Trending now

This is a popular solution!

Step by step

Solved in 4 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

In the redox titrations using potassium permanganate and iron (II) ammonium sulfate hexahydrate, what indicator would you use?
17. When metallic lithium is a reactant in a synthesis reaction with oxygen gas to form an ionic compound, does the lithium act as an oxidizing agent or reducing agent? Justify your answer using half-reactions along with your explanation of terms. (3)
Consider the balanced redox reaction between silver and nitgric acid: 2H+ + Ag + NO3 -1 results in Ag + NO + H2O. If 42.50 mL of 12.0M nitric acid furnishes enough H+ to react with silver, how many grams of silver react?
I need help with all parts. Thanks
Write the balanced equations for the half reactions (ionic) and the overall net ionic equation for tritation of Mohr's salt Fe(NH4)2(SO4)2*6H2O with KMnO4. What is standardized molarity of a KMnO4 solution if 36.31ml are required to tritate 2.5010 g of Mohr's salt.
Can you please show me step by step how to do this question as I am very confused on these! :(
A solid sample containing some Fe2+ weighs 2.360 g. It required 36.44 mL 0.0244 M KMnO4 to titrate the Fe2+ in the dissolved sample to a pink end point. The balanced redox reaction is shown below. 8 H+ + MnO4ˉ + 5 Fe2+ ® Mn2+ + 5 Fe3+ + 4 H2O Calculate each of the following quantities. How many moles MnO4– were used in the titration? How many moles Fe 2+ are there in the sample? How many grams of Fe are there in the sample? What is the percentage of Fe (by mass) in the sample? Calculate the percentage of Fe in pure iron(II) ammonium sulfate hexahydrate: (NH4)2[Fe(SO4)2]• 6 H2O.
For Questions 11-16: Balance the following oxidation-reduction reaction in acidic conditions using the half reaction method by following the step described in each question. ??2?−27(??)+???2(??)⟶??+3(??)+??−3(??)Cr2O7−2(aq)+HNO2(aq)⟶Cr+3(aq)+NO3−(aq) Step 1: Assign the oxidation states of each ATOM in the reaction before and after the reaction takes place. Reactants: Cr = ["", "", "", "", "", "", "", "", "", "", "", "", "", "", ""] O = ["", "", "", "", "", "", "", "", "", "", "", "", "", "", ""] H = ["", "", "", "", "", "", "", "", "", "", "", "", "", "", ""] N = ["", "", "", "", "", "", "", "", "", "", "", "", "", "", ""] Products: Cr = ["", "", "", "", "", "", "", "", "", "", "", "", "", "", ""] O = ["", "", "", "", "", "",…