Question

PbCl(aq) =Pb2+ (aq) + 2Cl(aq), K3 = 1.87x10-10, and

AgCl(aq) = Ag+ (aq) + Cl- (aq), K4 = 1.23x10-4,
what is the equilibrium constant Kfinal for the following reaction?
PbCl2 (aq) + 2Ag+ (aq)
2AgCl(aq) + Pb2+ (aq)
A. 1.87x10-10
B. 1.23x10-4
C. 2.36x10-14
D. 4.74x10-14

Answer 1

The equilibrium constant, Kfinal, for the reaction can be determined by multiplying the equilibrium constants for the individual reactions that make up the overall reaction.

Step-by-step explanation:

The equilibrium constant, Kfinal, for the reaction can be determined by multiplying the equilibrium constants for the individual reactions that make up the overall reaction. In this case, the individual reactions are:

1. PbCl(aq) = Pb2+ (aq) + 2Cl(aq), with equilibrium constant K3 = 1.87x10-10
2. AgCl(aq) = Ag+ (aq) + Cl- (aq), with equilibrium constant K4 = 1.23x10-4

To find the equilibrium constant for the overall reaction, we multiply K3 and K4:

Kfinal = K3 * K4 = (1.87x10-10) * (1.23x10-4) = 2.3001x10-14, which is closest to answer choice D, 4.74x10-14.