If the concentration of Cr_2O_7^{2-} in a sat | vedclass

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(A) The dissociation of $Ag_2Cr_2O_7$ is given by: $Ag_2Cr_2O_7(s) \rightleftharpoons 2Ag^+(aq) + Cr_2O_7^{2-}(aq)$.Let the solubility of $Ag_2Cr_2O_7

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$1.10 	imes 10^{-12}$

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(A) The dissociation of $Ag_2Cr_2O_7$ is given by: $Ag_2Cr_2O_7(s) ightleftharpoons 2Ag^+(aq) + Cr_2O_7^{2-}(aq)$.Let the solubility of $Ag_2Cr_2O_7$ be $s \ M$.Then,$[Cr_2O_7^{2-}] = s = 6.5 	imes 10^{-5} \ M$.And $[Ag^+] = 2s = 2 	imes (6.5 	imes 10^{-5}) = 1.3 	imes 10^{-4} \ M$.The solubility product expression is $K_{sp} = [Ag^+]^2 [Cr_2O_7^{2-}]$.Substituting the values: $K_{sp} = (1.3 	imes 10^{-4})^2 	imes (6.5 	imes 10^{-5})$.$K_{sp} = (1.69 	imes 10^{-8}) 	imes (6.5 	imes 10^{-5}) = 1.0985 	imes 10^{-12} \approx 1.10 	imes 10^{-12}$.

If the concentration of $Cr_2O_7^{2-}$ in a saturated solution of $Ag_2Cr_2O_7$ is $6.5 \times 10^{-5} \ M$ at a constant temperature,calculate the value of $K_{sp}$ for $Ag_2Cr_2O_7$.

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