Which of the following compounds will have the highest molar solubility in pure

Question

Which of the following compounds will have the highest molar solubility in pure water? A) MgC_2O_4, K_sp = 8.5 times 10^-5 B) CuCN, K_sp = 3.2 times 10^-20 C) Agl, K_sp = 8.5 times 10^-17 D) AgN_3, K_sp = 2.8 times 10^-12 E) NiCO_3, K_sp = 6.6 times 10^-9 Consider the dissolution of FeS in water (K_sp = 6.0 times 10^-19): FeS(s) + H_2O(aq) reversiblearrow Fe^2+(aq) + HS^- (aq) + OH^-(aq) How is the solubility of FeS affected by the addition of aqueous KOH to the system? A. The solubility will increase B. The solubility will decrease C. The solubility will be unchanged D. The amount of KOH added must be known before its effect can be predicted E. The pK_a of H_2S is needed before a reliable prediction can be made The molar solubility of MnS is 1.7 times 10^-7M in pure water. Calculate the K_sp for MnS. A) 6.80 times 10^-5 B) 1.6 times 10^-35 C) 2.9 times 10^-14 D) 2.6 times 10^-24 E) 8.0 times 10^-13

Explanation / Answer

1) All salts are of the type AB

AB (s) <----------> A+ (aq) + B- (aq)

- s s

Ksp = s2

and solubility of salt s = (Ksp)1/2

Thus the salt with highest Ksp value will have highest solubility.

Thus OPTION A , MgC2O4 with Ksp of 8.5x10-5 has highest ksp value and thus highest molar solubility.

2) In Ksp equilibrium OH- ions are on the right side , product side.

If OH- ions are added , that is kOH addition , the product concentration increase, thus the equilibrium shifts left side.

Which means solubility decreases.

Option B

3) the equilibrium is

MnS(s) <---------> Mn+2 (aq) + S-2(aq)

s s

and Ksp = s2

= (1.7x10-7)2

= 2.89 x10-14

OPTION C

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