Assertion :Addition of silver ions to a mixture of aqueous sodium chloride and sodium bromide solution will first precipitate $A g B r$ rather than $A g C l$ Reason: $K_{s p}$ of $A g C l < K_{s p}$ of $A g B r$

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

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

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Assertion is correct but Reason is incorrect

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Both Assertion and Reason are incorrect

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Solution

The correct option is C Assertion is correct but Reason is incorrect
The species having minimum value of $K_{s p}$ will get precipitated first of all because ionic product will exceed the solubility product of such species.

As $K_{s p}$ of $A g C l > K_{s p}$ of $A g B r$

So addition of silver ions to a mixture of aqueous sodium chloride and sodium bromide solution will first precipitate AgBr rather than AgCl.

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Similar questions

Q. Assertion :The addition of silver ions to a mixture of aqueous sodium chloride and sodium bromide solution, will first precipitate

A g B r

rather than

A g C l

. Reason: The value of

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A g C l < K_{s p}

A g B r

Q. Assertion: Addition of silver ions to a mixture of aqueous sodium chloride and sodium bromide solution will first precipitate AgBr rather than AgCl.
Reason: Ksp of AgCl < Ksp of AgBr.

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(d) Assertion is wrong statement but reason is correct statement.
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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: Kspof AgCl<Ksp of AgBr

Assertion :Addition of silver ions to a mixture of aqueous sodium chloride and sodium bromide solution will first precipitate $A g B r$ rather than $A g C l$ Reason: $K_{s p}$ of $A g C l < K_{s p}$ of $A g B r$