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NEET CHEMISTRYMedium

The concentration of Ag+Ag^+ ions in a saturated solution of Ag2C2O4Ag_2C_2O_4 is 2.2×10−4 mol L−12.2 \times 10^{-4} \text{ mol L}^{-1}. The solubility product of Ag2C2O4Ag_2C_2O_4 is:

A

2.66×10−122.66 \times 10^{-12}

B

4.5×10−114.5 \times 10^{-11}

C

5.3×10−125.3 \times 10^{-12}

D

2.42×10−82.42 \times 10^{-8}

Step-by-Step Solution

The dissociation of silver oxalate is given by: Ag2C2O4(s)⇌2Ag+(aq)+C2O42−(aq)Ag_2C_2O_4(s) \rightleftharpoons 2Ag^+(aq) + C_2O_4^{2-}(aq) Given the concentration of Ag+Ag^+ ions, [Ag+]=2.2×10−4 M[Ag^+] = 2.2 \times 10^{-4} \text{ M}. From the stoichiometry of the dissociation reaction, the concentration of oxalate ions [C2O42−][C_2O_4^{2-}] is half the concentration of Ag+Ag^+ ions: [C2O42−]=[Ag+]2=2.2×10−42=1.1×10−4 M[C_2O_4^{2-}] = \frac{[Ag^+]}{2} = \frac{2.2 \times 10^{-4}}{2} = 1.1 \times 10^{-4} \text{ M}. The solubility product expression is: Ksp=[Ag+]2[C2O42−]K_{sp} = [Ag^+]^2[C_2O_4^{2-}] Substitute the values into the expression: Ksp=(2.2×10−4)2×(1.1×10−4)=(4.84×10−8)×(1.1×10−4)=5.324×10−12≈5.3×10−12K_{sp} = (2.2 \times 10^{-4})^2 \times (1.1 \times 10^{-4}) = (4.84 \times 10^{-8}) \times (1.1 \times 10^{-4}) = 5.324 \times 10^{-12} \approx 5.3 \times 10^{-12}.

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