Question

Question 10 The equilibrium of a ZnS precipitate with an aqueous solution of Zn2+ where H2S gas is bubbled through the solution is described by the following chemical equation and equilibrium constant Zn(s) + 2H+ (aq) = Zn2+ (aq) + H250g) K25 t = 0.11 Given that the Zn ion concentration in the solution is 100 10-6 M with a pH of 4.0. if the partial pressure of H2S is 0 01 am then, the solution is undersaturated and a Zns precipitate can form the solution is overersaturated and a Zns precipitate can form the solution is saturated and a Zns precipitate is present the solution is overersaturated and a ZnS precipitate cannot form the solution is undersaturated and a Zns precipitate cannot form Submit un last checked at 5:35pm

Answer 1

ZnS(s) + 2H^+(aq) ------> Zn^2+ (aq) + H2S(g)    Kc = 0.11

PH = 4

-log[H^+] = 4

    [H^+] = 10^-4 M

PH2S = 0.01atm

[Zn^2+]   = 1*10^-6M

Qc   = [Zn^2+][H2S]/[H^+]^2

       = 10^-6*0.01/(10^-4)

        = 10^-4

Kc>Qc

The equilibrium shift to right side

The solution is unsaturated and a ZnS precipitate cannot form >>>>answer