Equilibrium Question 756

Question: When equal volumes of the following solutions are mixed, precipitation of AgCl ( $ K _{sp} $ = $ 1.8\times {10^{-10}} $ ) will occur only with

Options:

A) $ {10^{-4}}M(A{g^{+}}),and,{10^{-4}}M(C{l^{-}}) $

B) $ {10^{-5}}M(A{g^{+}}),and,{10^{-5}}M(C{l^{-}}) $

C) $ {10^{-16}}M(A{g^{+}}),and,{10^{-6}}M(C{l^{-}}) $

D) $ {10^{-10}}M(A{g^{+}}),and,{10^{-10}}M(C{l^{-}}) $

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Answer:

Correct Answer: A

Solution:

$ AgCl\rightarrow [A{g^{+}}]+[C{l^{-}}] $

$ =( \frac{{10^{-4}}\times V}{2V} )( \frac{{10^{-4}}\times V}{2V} )=2.5\times {10^{-9}} $

This value is greater than $ K _{sp}=1.8\times {10^{-10}} $

(2) IP= $ ( \frac{{10^{-5}}\times V}{2V} )( \frac{{10^{-5}}\times V}{2V} )=2.5\times {10^{-11}}<K _{sp} $

(3) IP= $ ( \frac{{10^{-16}}\times V}{2V} )( \frac{{10^{-6}}\times V}{2V} )=2.5\times {10^{-23}}<K _{sp} $

(4) IP= $ ( \frac{{10^{-10}}\times V}{2V} )( \frac{{10^{-10}}\times V}{2V} )=2.5\times {10^{-21}}<K _{sp} $



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