🏷️ LIMITED TIME OFFER: GET 20% OFF GRADE+ YEARLY SUBSCRIPTION →
Log in
Chemistry
2
answers
2
watching
1,184
views
28 Jun 2020

What is the coefficient for hydroxide, and how many electrons are transferred after balancing the reaction?

Pb(OH)4 2- + ClO- → PbO2 + Cl- + OH- + H2O

Booster class
AP Chemistry
Skill
Solve problems involving galvanic (voltaic) and electrolytic cells
Watch
2
answers
2
watching
1,184
views

For unlimited access to Homework Help, a Homework+ subscription is required.

Avatar image
Read by 23 people

Unlock all answers

Get 1 free homework help answer.
Already have an account? Log in
Share
1 Sep 2020
Already have an account? Log in
Share
discord banner image
Join us on Discord
Chemistry Study Group
Join now

Related textbook solutions

Basic Chemistry
5 Edition,
Timberlake
ISBN: 9780134138046
Principles of Chemistry Molecular Approach
4th Edition,
Tro
ISBN: 9780134112831
Principles of Chemistry Molecular Approach
3rd Edition, 2014
Tro
ISBN: 9780321971944
Chemistry: Structure and Properties
2nd Edition,
Tro
ISBN: 9780134293936
Chemistry: A Molecular Approach
3rd Edition,
Tro
ISBN: 9780321809247
Chemistry: A Molecular Approach
5th Edition,
Tro
ISBN: 9780134874371
Principles of Chemistry: A Molecular Approach
4th Edition,
Tro
ISBN: 9780134895741
Chemistry: The Central Science
14th Edition, 2017
Brown
ISBN: 9780134414232

Related questions

Complete and balance the following equations, and identify the oxidation and reducing agents:

a) Cr2O72-(aq) + I- (aq) → 2Cr +3 + IO3- (acidic solution)

b) MnO4-(aq) + CH3OH(aq) →Mn2+(aq) + HCOOH(aq) (acidic solution)

c) I2(s) + ClO- (aq) → IO3- (aq) +Cl- (aq) (acidic solution)

d) As2O3 (s) + 2NO3-(aq) → 2H3AsO4 +N2O3 (acidic solution)

e) MnO4- + H2O +Br- → 2MnO2 + 2OH- + BrO3- (basic solution)

f) Pb(OH)42- (aq) + ClO- (aq) → PbO2(s) + Cl – (aq) (basic solution)

One Class Solution:-

  1. Cr2O72- + I- + → Cr +3 + IO3- (acidic solution)

+6 +3

Cr2O72-→ Cr +3 REDUCTION

-1 +5

I-→ IO3- OXIDATION

Cr2O72- +14 H+ +6 e- → 2Cr +3 + 7H2O

I- + 3H2O → IO3- + 6H++ 6e-

Cr2O72- + 14 H++ I- + 3H2O → 2Cr +3 + IO3- + 6H+ + 7H2O

+6OH- → 6OH-

Cr2O72- + 8H++ I- + 3H2O → 2Cr +3 + IO3- + 7H2O

b)MnO4- + CH3OH →Mn2+ + HCOOH (acidic solution)

+7 +2

MnO4- →Mn2+ REDUCTION

-2 +2

CH3OH → HCOOH OXIDATION

MnO4- + 8H+ + 5e- → Mn2+ + 4H2O ∕. 4

CH3OH + H2O → HCOOH + 4H+ +4 e- ∕ .5

4MnO4- + 32H+ + 20e-+ 5CH3OH + 5H2O→ 4Mn2+ + 5HCOOH + 20H+ +20 e- + 16H2O

+20OH- → 20OH-

4MnO4- + 12H+ + 5CH3OH + → 4Mn2+ + 5HCOOH + 11H2O

c)I2 + OCl- → IO3- + Cl- (acidic solution)

0 +5

I2→ IO3- OXIDATION

+1 -1

OCl- → Cl- REDUCTION

0 +5

I2 + 3H2O → 2IO3- + 6H+ + 5e- / 2

+1 -1

ClO- + H+ + 2 e-→ Cl- + H2O /5

2I2 + 6H2O + 5ClO- + 5H+ + 10 e- → 4IO3- + 12H+ + 10e- + 5Cl- + 5H2O

+5H+ → +5H+

2I2 + 6H2O + 5ClO- → 4IO3- + 7H+ + 5Cl- + 5H2O

d)As2O3 + NO3-→ H3AsO4 + N2O3 (acidic solution)

+3 +5

As2O3→2H3AsO4 OXIDATION

+5 +3

2NO3-→ N2O3 REDUCTION

As2O3 + 5H2O → 2H3AsO4 + 4H++ 4e- /4

2NO3- + 6H+ +4e- → N2O3 + 3H2O /4

As2O3 + 2NO3- + 6H+ +4e- +5H2O → 2H3AsO4 + 4H++ 4e- + N2O3 + 3H2O

+4 OH → +4OH

As2O3 + 2NO3- + 2H+ +2H2O → 2H3AsO4 + N2O3

e)MnO4- + Br- → MnO2 + BrO3- (basic solution)

+7 +4

MnO4- + 2H2O +3e- → MnO2 + 4OH- /2

-1 +5

Br- + 6OH- → BrO3-+ 3H2O + 6e- /1

2MnO4- + 4H2O +6e- + Br- + 6OH- → 2MnO2 + 8OH-+ BrO3-+ 3H2O + 6e-

+ 6 H+ → + 6 H+

2MnO4- + H2O +Br- → 2MnO2 + 2OH-+ BrO3-

f) Pb(OH)42- + ClO- → PbO2 + Cl –

+2 +4

Pb(OH)42- → PbO2 + H2O +2 e- oxidation/1

+1 -1

ClO- + H2O +2 e- → Cl – +2 OH- reduction /1

Pb(OH)42- + ClO- + H2O + 2 e- → PbO2 + H2O + Cl – + 2OH- + 2 e-

+H+ → +H+

Pb(OH)42- + ClO- → PbO2 + Cl – + 2OH-+H2O

Redox Reactions -- Electrons Transferred

Balance each of the following equations occuring in basic aqueous solution.
In each case enter the number (n) of electrons transferred from the reducing agent to the oxidizing agent for the conventionally balanced equation (full reaction).

Pb(OH)3- + OCl- --> PbO2 + Cl- Br2 + Cr(OH)3 --> Br- + CrO42- Be + SO32- --> S2O32- + Be2O32- Al + NO3- --> NH3 + Al(OH)4-

Show transcribed image text

Balance the following redox reaction if it occurs in basic solution. What are the coefficients in front of Cr(OH)4- and ClO- in the balanced reaction?

Cr(OH)4-(aq) + ClO-(aq) ? CrO42-(aq) + Cl-(aq)

Balance the following redox reaction if it occurs in basic solution. What are the coefficients in front of Cr(OH)4- and ClO- in the balanced reaction?

Cr(OH)4-(aq) + ClO-(aq) ? CrO42-(aq) + Cl-(aq)

Cr(OH)4- = 6, ClO- = 5
Cr(OH)4- = 1, ClO- = 2
Cr(OH)4- = 2, ClO- = 6
Cr(OH)4- = 1, ClO- = 1
Cr(OH)4- = 2, ClO- = 3

Weekly leaderboard

Home
Homework Help 3,900,000
Chemistry 830,000
Start filling in the gaps now
Log in