A student measures the molar solubility of zinc sulfide in a water solution to be 4.32×10-13 M. Based on her data, the solubility product constant for this compound is
solubility of zinc sulfide (s) = 4.32*10^-13 M
ZnS(S) ------------> Zn^2+ (aq) + S^2- (aq)
s s
Ksp = [Zn^2+][S^2-]
Ksp = s*s
Ksp = s^2
Ksp = (4.32*10^-13)^2 = 1.86*10^-25 >>>>answer
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