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  3. 4. calculate the equilibrium concentration of ag+

4. Calculate the equilibrium concentration of Ag+ (aq) in a solution that is initially 0.150 M...

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Chemistry

4. Calculate the equilibrium concentration of Ag+(aq) in a solution that is initially 0.150 M AgNO3 and0.500 M KCN. The formation constant for[Ag(CN)2]- (aq) is Kf= 1.0 x1021

a. 8.9 x 10-21 M

b. 2.3 x 10 -21 M

c. 4.3 x 10 -22 M

d. 7.5 x 10 -22 M

e. 3.8 x 10 -21 M

5. If a solution of Pb(NO3)2 (aq) is mixedwith a solution of NaBr(aq), what condition would causeprecipitation of PbBr2 (s) to occur?

a. When [Na+][NO3-] sp for PbBr2

b. When [Pb2+][Br -]2 sp for PbBr2

c. When [Pb2+][Br -] < Kspfor PbBr2

d. When [Pb2+][Br -]2 >Ksp for PbBr2

e. When [Pb2+][Br - ] > Kspfor PbBr2

Answer & Explanation Solved by verified expert
3.8 Ratings (440 Votes)

Ag+ (aq) + 2CN- (aq) = [Ag(CN)2]- (aq)

FORMATION CONSTANT K =[ [Ag(CN)2]- (aq)] /[ Ag+ (aq) ] [CN- (aq)]2

                                    Ag+ (aq)    + 2CN- (aq)    =        [Ag(CN)2]- (aq)

INTIAL CONCENTRATION         0.150 M                 0.500 M                         0

LET AT EQUILIBRIUM               (.150-X)               (.500-2X)                         X

X M Ag+ (aq) REACTES

FORMATION CONSTANT K =[ [Ag(CN)2]- (aq)] /[ Ag+ (aq) ] [CN- (aq)]2

       K = X / (.150-X ) (.500-X )2

NOW SOLVE THE EQUATION TO GET X

5. d. When [Pb2+][Br -]2 > Ksp for PbBr2
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