Calculate the molar solubility of CuX(Ksp=1.27×10?36) in each of the following. |
Part A pure water Express your answer using three significant figures. Part B 0.25 M CuCl2 Express your answer using two significant figures.
Part C 0.23 M Na2X Express your answer using two significant figures. |
1) The dissociation of salt CuX in aqueous solution takes place as follows:
CuX(s) <--->Cu2+(aq) +X2-(aq)
Ksp1.27*10^-36
[Cu2+][X2-]
Let the molar solubility of CuX in pure water be S,
[Cu2+][X2-]
S
1.27*10^-36[Cu2+][X2-]
S^2
or, S1.127*10^-18M
part B) In 0.25M CuCl2 solution, CuCl2 <--->Cu2+(aq) +2Cl-
[Cu2+]0.25M+S
0.25M (as S<<<0.25M)
So,Ksp1.27*10^-36
[Cu2+][X2-]
(0.25M)*S
or ,Molar Solubility,S(1.27*10^-36)/0.25
5.08*10^-36M
part C) In 0.23M Na2X, Na2X <--->2Na+(aq) + X2-(aq)
[X2-]0.23+S
0.23M
(S<<<0.23M)
Ksp1.27*10^-36
[Cu2+][X2-]
(0.23M)*S
or ,Molar Solubility,S(1.27*10^-36)/0.23
5.522*10^-36M
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