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Chemistry Question on Equilibrium

Concentration of the Ag+Ag^+ ions in a saturated solution of Ag2C2O4Ag_2C_2O_4 is 2.2×10−4 mol L−12.2 \times 10^{-4}\, mol\, L^{-1} 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}

Answer

5.3×10−125.3 \times 10^{-12}

Explanation

Solution

Ag2C2O4(s)⇌2Ag+2s(aq)+C2O42−s(aq)Ag _{2} C _{2} O _{4}( s ) \rightleftharpoons \underset{2s}{2 Ag ^{+}}( aq )+ C _{2} \underset{s}{O _{4}^{2-}}( aq )
KSP=[Ag+]2[C2O42−]K _{ SP }=\left[ Ag ^{+}\right]^{2}\left[ C _{2} O _{4}^{2-}\right]
[Ag+]=2.2×10−4M\left[ Ag ^{+}\right]=2.2 \times 10^{-4} M
∴[C2O42−]=2.2×10−42M=1.1×10−4M\therefore \left[ C _{2} O _{4}^{2-}\right]=\frac{2.2 \times 10^{-4}}{2} M =1.1 \times 10^{-4} M
∴KSP=(2.2×10−4)2(1.1×10−4)\therefore K _{ SP }=\left(2.2 \times 10^{-4}\right)^{2}\left(1.1 \times 10^{-4}\right)
=5.324×10−12=5.324 \times 10^{-12}