Assertion: Addition of silver ions to a mixtu | vedclass

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(A) The precipitation of a salt occurs when the ionic product exceeds its solubility product constant $(K_{sp})$. Since $K_{sp}$ of $AgBr$ $(5.0 	ime

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If both Assertion and Reason are correct and the Reason is a correct explanation of the Assertion.

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(A) The precipitation of a salt occurs when the ionic product exceeds its solubility product constant $(K_{sp})$. Since $K_{sp}$ of $AgBr$ $(5.0 	imes 10^{-13})$ is significantly lower than the $K_{sp}$ of $AgCl$ $(1.8 	imes 10^{-10})$,the ionic product of $AgBr$ reaches its $K_{sp}$ value first upon the addition of $Ag^+$ ions. Therefore,$AgBr$ precipitates first. Both the Assertion and the Reason are correct,and the Reason correctly explains the Assertion.

Assertion: Addition of silver ions to a mixture of aqueous sodium chloride and sodium bromide solution will first precipitate $AgBr$ rather than $AgCl$.
Reason: $K_{sp}$ of $AgCl > K_{sp}$ of $AgBr$.

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Assertion: Addition of silver ions to a mixture of aqueous sodium chloride and sodium bromide solution will first precipitate $AgBr$ rather than $AgCl$.Reason: $K_{sp}$ of $AgCl > K_{sp}$ of $AgBr$.