The solubility product of AgCl is 1.8 times 1 | vedclass

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(B) Precipitation occurs when the ionic product $(IP)$ exceeds the solubility product $(K_{sp})$.When equal volumes are mixed,the concentration of eac

Vedclass · Accepted Answer

$10^{-3} \ M \ Ag^{+}$ and $10^{-3} \ M \ Cl^{-}$ ions

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(B) Precipitation occurs when the ionic product $(IP)$ exceeds the solubility product $(K_{sp})$.When equal volumes are mixed,the concentration of each ion is halved.For option $B$,the new concentrations are $[Ag^{+}] = \frac{10^{-3}}{2} \ M$ and $[Cl^{-}] = \frac{10^{-3}}{2} \ M$.$IP = [Ag^{+}][Cl^{-}] = (0.5 	imes 10^{-3}) 	imes (0.5 	imes 10^{-3}) = 0.25 	imes 10^{-6} = 2.5 	imes 10^{-7}$.Since $2.5 	imes 10^{-7} > 1.8 	imes 10^{-10}$,the condition $IP > K_{sp}$ is satisfied,and precipitation will occur.

The solubility product of $AgCl$ is $1.8 \times 10^{-10}$. Precipitation of $AgCl$ will occur by mixing which of the following solutions when mixed in equal volume?

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