Calculate the solubility of

PbSO4 whoseKsp = 2.0 x 10-14:

Oxidation Reduction Reactions(REDOX)

REDOX Reactions

•Chemical reactions in which electrons

are transferred

Oxidation•The act of losing

electrons

•Oxidation number increases

Reduction•The act of gaining

electrons

•Oxidation number decreases

REDOX Fact•You cannot have oxidation without

reduction or reduction without oxidation

Oxidizing Agent•A substance that oxidizes another

•The oxidizing agent will be reduced

Reducing Agent•A substance that

reduces another

•The reducing agent will be oxidized

Balancing REDOX Reactions

Balancing Redox Rxns1)Determine all ox #

2)Determine elements being oxidized & reduced

3)Divide rxn into half-rxns

4)Balance half-rxns

Balancing Half-Rxnsa)Balance redox elements

b)Balance ox # with e-

c)Balance e- between the two half-rxns

Balancing Half-Rxnsd)Balance total charge

with H+ or OH-

e)Balance H’s with waterf) Check balance with oxygen

Balancing Redox Rxns5) Add the two half-reactions

a)Cancel like substances from each side of the full reaction

b)Check work

Balance Redox Rxns:

MnO2 + Cl-1

Mn+2 + Cl2

in acid

Balance Redox Rxns:

Cr2O7-2 + NH3

Cr+3 + NO3-1

in base

Balance Redox Rxns:

MnO4-1 + N2O3

Mn+3 + N2O5

in base

Balance Redox Rxns:

HNO3 + Cu

N2O + Cu+2

in acid

Balance Redox Rxns:

SO2 + Pb(OH)2

SO3 + Pb

in base

Balance Redox Rxns:

MnO2 + P4

Mn2O7 + PH3

in acid

Balance Redox Rxns:

FeCl2 + KNO3

FeCl3 + KNO

in base

Balance Redox Rxns:

SnF2 + KIO4

KI + SnF4

in acid

Balance Redox Rxns:

IO3-1 + I-1

I3-1

in acid

Balance Redox Rxns:

PbBr4 + K2O

PbBr2 + O2

in acid

Balance Redox Rxns:

Ca + VO4-3

CaO + V+2

in acid

Balance Redox Rxns: Fe(OH)3 + Cr(OH)4

-1

Fe(OH)2 + CrO4-2

in base

Balance Redox Rxns:

Ni(OH)2 + N2H4

Ni + N2

in base

Balance Redox Rxns:

K3PO4 + Cr+2

P2O3 + K2CrO3

in acid

Balance Redox Rxns:

H2SO4 + Cr+2

SO + H2Cr2O7

in acid

Balance Redox Rxns:

PH3 + KMnO4

P2O5 + Mn2O3

in KOH