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.

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 E Assertion is correct but Reason is not correct
The solubility product of AgBr is $5 \times 10^{- 13}$ .
The solubility prodct of AgCl is $5 \times 10^{- 10}$ .
Hence, the solubility product of AgBr is lower than the solubility product of AgCl.
Thus, when silver ions are added to a mixture of aqueous sodium chloride and sodium bromide solution, AgBr will precipitate first.

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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: Ksp of AgCl < Ksp of AgBr.

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.