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Equilibrium · NEET Preparation Chemistry

The solubility product (K{sp}) of Ag2CrO4 is 3.2 times 10^{-11} at a certain temperature. What is the maximum concentration of Ag^+ ions in a saturat…

Practice question from Equilibrium (NEET Preparation Chemistry), with the correct answer and a step-by-step solution.

medium · MCQ · Q-BDD554

The solubility product (KspK_{sp}) of Ag2CrO4Ag2CrO_4 is 3.2×10−113.2 \times 10^{-11} at a certain temperature. What is the maximum concentration of Ag+Ag^+ ions in a saturated solution of Ag2CrO4Ag_2CrO_4?

  1. A.2.0 \times 10^{-4} M
  2. B.4.0 \times 10^{-4} MCorrect answer
  3. C.2.0 \times 10^{-3} M
  4. D.8.0 \times 10^{-4} M

Solution

Let solubility of Ag2CrO4Ag_2CrO_4 be ss. Dissociation: Ag2CrO4⇌2Ag++CrO42−Ag_2CrO_4 \rightleftharpoons 2Ag^+ + CrO_4^{2-}. Thus, [Ag+]=2s[Ag^+] = 2s and [CrO42−]=s[CrO_4^{2-}] = s. Ksp=(2s)2(s)=4s3K_{sp} = (2s)^2(s) = 4s^3. Given Ksp=3.2×10−11K_{sp} = 3.2 \times 10^{-11}, so 4s3=3.2×10−11  ⟹  s3=8×10−12  ⟹  s=2×10−44s^3 = 3.2 \times 10^{-11} \implies s^3 = 8 \times 10^{-12} \implies s = 2 \times 10^{-4} M. Therefore, [Ag+]=2s=4×10−4[Ag^+] = 2s = 4 \times 10^{-4} M.

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