Assertion:
Solubility of $A g C l$ in water decreases if $N a C l$ is added to it.
Reason:
$N a C l$ is soluble freely in water but $A g C l$ is sparingly soluble.

Both Assertion and Reason are correct and Reason is the correct explanation of Assertion

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Both Assertion and Reason are correct but Reason is not the correct explanation of Assertion

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Assertion is correct but Reason is not correct

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Assertion is not correct but Reason is correct

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Both Assertion and Reason are not correct

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Solution

The correct option is C Both Assertion and Reason are correct but Reason is not the correct explanation of Assertion
$N a C l$ is a strong electrolyte. It completely dissociates to form ions. Hence, it is highly soluble in water.
$A g C l$ dissociates to little extent. Hence, it is sparingly soluble in water.
When $N a C l$ is added to a solution of $A g C l$ , due to common ion effect (chloride ion is the common ion), the dissociation of $A g C l$ is suppressed. Also as the concentration of chloride ion (from $N a C l$ ) increases, the ionic product of $A g C l$ exceeds its solubility product and precipitation occurs.

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Assertion:Solubility of AgCl in water decreases if NaCl is added to it.Reason:NaCl is soluble freely in water but AgCl is sparingly soluble.

Assertion:
Solubility of $A g C l$ in water decreases if $N a C l$ is added to it.
Reason:
$N a C l$ is soluble freely in water but $A g C l$ is sparingly soluble.