Statement I : When salt dissolves in water, $Δ S$ for the process is positive.
Statement II : Aqueous ions have a greater entropy than ions in a solid.

Statement 1 and Statement 2 are correct and Statement 2 is the correct explanation of Statement 1 .

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Both the Statement 1 and Statement 2 are correct and Statement 2 is not the correct explanation of Statement 1.

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Statement 1 is correct but Statement 2 is not correct.

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Statement 1 is not correct but Statement 2 is correct.

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Both the Statement 1 and Statement 2 are not correct.

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Solution

The correct option is A Statement 1 and Statement 2 are correct and Statement 2 is the correct explanation of Statement 1 .
The entropies of gases are much larger than those of liquids, which are larger than those of solids. When salt dissolves in water, $Δ S$ for the process is positive because salt transfer from solid phase to liquid phase,which have higher entropy.
Aqueous ions have a greater entropy than ions in a solid,this statement is also true and also correct explanation of statement 1.

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Statement I : When salt dissolves in water, ΔS for the process is positive.Statement II : Aqueous ions have a greater entropy than ions in a solid.

Statement I : When salt dissolves in water, $Δ S$ for the process is positive.
Statement II : Aqueous ions have a greater entropy than ions in a solid.