The Solubility Product Of A Saturated Solution Of Ag2cro4 In Water At 298 K If The Emf Of The Cell Ag Is 0.164 V At 298 K.

Sol:

$E_{cell} = \frac{0.059}{1} log \frac{[Ag^{+}]RHS}{[Ag^{+}]LHS}\\\Rightarrow [Ag^{+}] LHS = 1.66 * 10^{-4 M}$

So, $[CrO_{4}^{2-}] = \frac{1.66 * 10^{-4}}{2}\\K_{sp}(Ag_{2}CrO_{4}) = [Ag^{+}]^{2} [CrO^{2-}_{4}]\\\Rightarrow (1.66 * 10^{-4})^{2} (\frac{1.66 * 10^{-4}}{2})\\\Rightarrow 2.287 * 10^{-12} mol^{3} L^{-3}$

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