Question

A solution has a [Ag+(aq)] of 0.01 M. The chloride concentration in solution is 1 x 10-5 M. Based on the following reaction, answer the following questions: AgCl(s) Ag+(aq) + Cl-(aq), Ksp = 1.7 x 10-10 Calculate the value of the current solubility product. Is the K value obtained greater or less than Ksp? Will a precipitate of AgCl form?

Answer 1

The value of current solubility product is calculated as below

K = (Ag+)( Cl-)

Ag+ = 0.01 M
Cl-= 1 x10^-5M

K is therefore = 1 x10^-5 x 0.01 = 1 x10 ^ -7 M

The K obtained is greater than Ksp

that is K> KSp
1x10^-7 > 1.7 x10 ^-10


will precipitation of AgCl form?

yes the precipitation of AgCl will be formed since K> KSP