Determine an unknown volume of concentration reduction titration. The concentration of a hydrogen peroxide solution is determined by titrating it with a 0.1237 M solution of permanganate. The balanced net ionic equation for the reaction is shown below. 2 MnO4 (aq) + 5 H₂O₂(aq) +6 H30+ (aq)-2 Mn²+ (aq) + 5 O₂(g) +14 H₂0 (1) In one experiment, 16.36 mL of the 0.1237 M MnO4 solution is required to react completely with 20.00 mL of the hydrogen peroxide solution. Calculate the concentration of the hydrogen peroxide solution. M

Determine an unknown volume of concentration reduction titration. The concentration of a hydrogen peroxide solution is determined by titrating it with a 0.1237 M solution of permanganate. The balanced net ionic equation for the reaction is shown below. 2 MnO4 (aq) + 5 H₂O₂(aq) +6 H30+ (aq)-2 Mn²+ (aq) + 5 O₂(g) +14 H₂0 (1) In one experiment, 16.36 mL of the 0.1237 M MnO4 solution is required to react completely with 20.00 mL of the hydrogen peroxide solution. Calculate the concentration of the hydrogen peroxide solution. M

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

Similar questions

Write balanced half-reactions for the following redox reaction: 8 CO₂(aq) + AsH3(g)+8 OH¯(aq) → 4C₂0¾¯(aq) + H₂AsO 4(aq) + 4H₂O(1) reduction: 0 oxidation: ロ→ロ e X S
Balance the following oxidation-reduction reaction that occurs in an acidic solution using the half-reaction method. I(aq) + Clo-(ag) → I3¯(aq) + CI-(aq) HOW DO WE GET THERE? For the reduction half-reaction, which half-reaction correctly balances the elements on both sides? ClO (aq) + H2O(1) → CI-(aq) + 2 H*(aq) clo-(aq) → Cl-(aq) 2 H+(aq) + ClO-(aq) → Cl-(aq) + H20(I) Clo-(aq) → CI-(aq) + H20(1) Clo-(aq) → Cl(aq) + H20(1) + 2 H*(aq) Check Next (4 of 6)
Complete and balance the following redox equations using the smallest whole-number coefficients. The reaction takes place in a BASIC solution. Fe(OH)2 (s) + MnO4−(aq) → MnO2 (s) + Fe(OH)2 (s) In the balanced equation, 3 OH- are present on the product side. In the balanced equation, 5 molecules of water are present on the reagent side. In the balanced equation, 4 molecules of water are present on the product side. In the balanced equation, 5 molecules of water are present on the product side. In the balanced equation, 3 OH- are present on the reagent side. In the balanced equation, 4 molecules of water are present on the reagent side.
What type of reaction is the following reaction: M(s) + 2 LX(aq) → 2 L(s) + M(aq) O Combustion ● Redox Precipitation Surprised Acid-Base
Write balanced half-reactions for the following redox reaction: 3+ 3 Cl₂(g) +2 Cr³+ (aq) +7H₂O(1) → 6 Cl(aq) + Cr₂O² (aq) +14 H+ (aq) reduction: oxidation: ロ→ロ × S ?
Given the reaction: Mg(s) + 2 HCl(aq) → MgCl2(aq) + H2(g) Which species is the reducing agent? HCI H2 MgCl2 Mg
The following chemical reaction takes place in aqueous solution: AGNO3(aq)+KBr(aq) →AGB1(s)+KNO3(aq) Write the net ionic equation for this reaction.
Given the following half-reactions, 2 103 (aq) + 12H*(aq) + 10 e → 12(s) + 6H2O Fe2* (aq) → Fe3* (aq) + e" write the balanced overall reaction. 2103 - (aq) + 12 H* (aq) + Fe 2* (aq) → Fel2 (s) + 6 H2O o 2 103 (aq) + 10 Fe²* (aq) → l2 (s) + 10 Fe³+ (aq) 2 103 - (aq) + 12 H* (aq) + Fe 2* (aq) → 12 (s) + Fe3+ (aq) + 6 H20 2 103 - (aq) + 12 H* (aq) + 10 Fe 2* (aq) → 12 (s) + 10 Fe3+ (aq) + 6 H20
Consider the following redox reaction: Ag⁺(aq) + Fe²⁺(aq) ⇌ Ag(s) + Fe³⁺(aq). What quantity in moles of electrons are exchanged?
Sodium oxalate, Na2C2O4Na2C2O4, in solution is oxidized to CO2(g)CO2(g) by MnO−4MnO4− which is reduced to Mn2+Mn2+. A 50.3 −mL−mL volume of a solution of MnO−4MnO4− is required to titrate a 0.342 −g−g sample of sodium oxalate. This solution of MnO−4MnO4− is then used to analyze uranium-containing samples. A 4.60 −g−g sample of a uranium-containing material requires 33.0 mLmL of the solution for titration. The oxidation of the uranium can be represented by the change UO2+→UO2+2UO2+→UO22+. Part A Calculate the percentage of uranium in the sample.
The hydroperoxide ion, HO2–(aq), reacts with permanganate ion, MnO4–(aq) to produce MnO2(s) and oxygen gas. Balance the equation for the oxidation of hydroperoxide ion to O2(g) by permanganate ion in a basic solution.