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NEET CHEMISTRYMedium

The concentration of the Ag+Ag^+ ions in a saturated solution of Ag2C2O4Ag_2C_2O_4 is 2.2×10−4 M2.2 \times 10^{-4}\text{ M}. The solubility product of Ag2C2O4Ag_2C_2O_4 is:

A

2.42×10−82.42 \times 10^{-8}

B

2.66×10−122.66 \times 10^{-12}

C

4.5×10−114.5 \times 10^{-11}

D

5.3×10−125.3 \times 10^{-12}

Step-by-Step Solution

The dissociation of silver oxalate (Ag2C2O4Ag_2C_2O_4) in aqueous solution is given by the equation: Ag2C2O4(s)⇌2Ag+(aq)+C2O42−(aq)Ag_2C_2O_4(s) \rightleftharpoons 2Ag^+(aq) + C_2O_4^{2-}(aq) From the stoichiometry of the reaction, if SS is the molar solubility of Ag2C2O4Ag_2C_2O_4, then: [Ag+]=2S[Ag^+] = 2S and [C2O42−]=S[C_2O_4^{2-}] = S Given that the concentration of Ag+Ag^+ ions is 2.2×10−4 M2.2 \times 10^{-4}\text{ M}: 2S=2.2×10−4 M2S = 2.2 \times 10^{-4}\text{ M} S=1.1×10−4 MS = 1.1 \times 10^{-4}\text{ M} Therefore, the concentration of oxalate ions is [C2O42−]=1.1×10−4 M[C_2O_4^{2-}] = 1.1 \times 10^{-4}\text{ M}. The solubility product constant (KspK_{sp}) is expressed as: Ksp=[Ag+]2[C2O42−]K_{sp} = [Ag^+]^2[C_2O_4^{2-}] Substitute the given values into the KspK_{sp} expression: Ksp=(2.2×10−4)2×(1.1×10−4)K_{sp} = (2.2 \times 10^{-4})^2 \times (1.1 \times 10^{-4}) Ksp=(4.84×10−8)×(1.1×10−4)K_{sp} = (4.84 \times 10^{-8}) \times (1.1 \times 10^{-4}) Ksp=5.324×10−12≈5.3×10−12K_{sp} = 5.324 \times 10^{-12} \approx 5.3 \times 10^{-12}

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