The generic metal hydroxide M(OH)2 has Ksp = 5.65×10−12. (NOTE: In this particular problem, because of the magnitude of the Ksp and the stoichiometry of the compound, the contribution of OH− from water can be ignored. However, this may not always be the case.) Part A What is the solubility of M(OH)2 in pure water? Express your answer with the appropriate units. Part B What is the solubility of M(OH)2 in a 0.202 M solution of M(NO3)2? Express your answer with the appropriate units.
PART(A)
M(OH)2 (s) M2+ (aq.) + 2 OH- (aq.)
S S 2S
Ksp = [M2+][OH-]2
Ksp = (S)(2S)2
5.65 * 10-12 = 4S3
S = Solubility of M(OH)2 = 1.12 * 10-4 M
PART (B)
M(OH)2 (s) M2+ (aq.) + 2 OH- (aq.)
M(NO3)2 (aq.) ------------> M2+ (aq.) + 2 NO3- (aq.)
0.202 0.202 2(0.202)
Ksp = [M2+][OH-]2
5.65 * 10-12 = (0.202)[OH-]2
[OH-]2 = 28.0 * 10-12
[OH-] = 5.29 * 10-6 M
So,
Solubility of M(OH)2 = (1/2)[OH-] = 2.64 * 10-6 M
The generic metal hydroxide M(OH)2 has Ksp = 5.65×10−12. (NOTE: In this particular problem, because of...
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The generic metal hydroxide M(OH)2 has Ksp = 5.45×10−18. (NOTE: In this particular problem, because of the magnitude of the Ksp and the stoichiometry of the compound, the contribution of OH− from water can be ignored. However, this may not always be the case.) Part A What is the solubility of M(OH)2 in pure water? Part B What is the solubility of M(OH)2 in a 0.202 M solution of M(NO3)2?
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Consider the dissolution of AB(s): AB(s)⇌A+(aq)+B−(aq) The generic metal hydroxide M(OH)2 has Ksp = 6.85×10−12. (NOTE: In this particular problem, because of the magnitude of the Ksp and the stoichiometry of the compound, the contribution of OH− from water can be ignored. However, this may not always be the case.) 1. Le Châtelier's principle tells us that an increase in either [A+] or [B−] will shift this equilibrium to the left, reducing the solubility of AB. In other words, AB...
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