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InterviewSolution
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The values of Ksp of two sparingly soluble salts Ni(OH)2 and AgCN are 2.0 x 10-15 and 6.0 x 10-17 respectively. Which salt is more soluble? Explain. |
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Answer» AgCN ⇌ Ag+ + CN− Ksp = [Ag+][CN−] = 6 × 10−17 Ni(OH)2 ⇌ Ni2+ + 2OH- Ksp = [Ni2+][OH−] 2 = 2 × 10−15 Let [Ag+] = S,then [CN−] = S1 Let [Ni2+] = S2,then [OH−] = 2S2 ∴ From eq. (i) S1 × S1 = 6 × 10−17 S12 = 6 × 10−17 S1 = 7.8 × 10−9 ∴ From eq. (ii) (S1) × (2S2)2 = 2 × 10−15 4S23 = 2 × 10−15 S23 = \(\frac{2\times10^{-15}}{4}\) = 0.5 × 10−15 or S2 = 0.58 × 10−4 Since solubility of Ni(OH)2 is more than AgCN, so, Ni(OH)2 is more soluble than AgCN. |
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