The solubility of two slightly soluble salts of M2+ , MA and MZ2, are the same,
ID: 503575 • Letter: T
Question
The solubility of two slightly soluble salts of M2+ , MA and MZ2, are the same, 4×104 mol/L.
Which has the larger numerical value for the solubility product constant?
In a saturated solution of each salt in water, which has the higher concentration of M2+?
If you added an equal volume of a solution saturated in MA to one saturated in MZ2, what would be the equilibrium concentration of the cation, M2+?
MA has the larger numerical value for the solubility product constant. MZ2 has the larger numerical value for the solubility product constant. The numerical value for the solubility product constant is the same for two salts.Explanation / Answer
1) MA -----> M+2 + A-2
- s s
Ksp = s2 = (4x10-4)2
= 1.6x10-7
MZ2 ---- ---> M+2 + 2Z-
- s 2s
Ksp = s(2s)2
= 4s3
= 4 (4x10-4)3
= 256 x 10-12
=2.56x10-10
Thus MA has higher numercial value of Ksp than MZ2
2)The concentration of M+2 is same in both saturated solutions(shown above)
3)Bothe the salts are sparigly soluble salts. When both are added in the same solution, the solubility of each of them is decreased due to common ion effect.
Thus [M+2] decreases.
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