If $S_{0}, S_{1}, S_{2}$ and $S_{3}$ are the solubilities in water of $A g C l$ , $0.01 M C a C l_{2}, 0.01 M N a C l$ and $0.5 M A g N O_{3}$ solutions, respectively, then which of the following is true?

S_{0} > S_{2} > S_{1} > S_{3}

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S_{0} = S_{2} = S_{1} > S_{3}

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S_{3} > S_{1} > S_{2} > S_{0}

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none of these

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Solution

The correct option is B $S_{0} > S_{2} > S_{1} > S_{3}$
The solubility of $A g C l$ or its ion formation will depend inversely on the concentration
$S_{0} = H_{2} O$
$S_{1} = 0.01 M C a C l_{2}$
$S_{2} = 0.01 M N a C l$
$S_{3} = 0.05 M A g N O_{3}$
$H_{2} O$ is dilute solution and least concentrated hence have maximum solubility of $A g C l$ in it. Out of $N a C l$ and $C a C l_{2}$ , the solubility of $N a C l$ is high due to loess number of ions produced from $N a C l$
as compare to $C a C l_{2}$ . More the ion produced lesser is the solubility of coming salt.
So, the Correct order is $S_{0} > S_{2} > S_{1} > S_{3}$
We know that concentration of common ion $α \frac{1}{s o l u b i l i t y}$ . The order of solubility of $A g C l : S_{1} > S_{3} > S_{2} > S_{4}$

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If S0,S1,S2 and S3 are the solubilities in water of AgCl, 0.01MCaCl2,0.01MNaCl and 0.5MAgNO3 solutions, respectively, then which of the following is true?

If $S_{0}, S_{1}, S_{2}$ and $S_{3}$ are the solubilities in water of $A g C l$ , $0.01 M C a C l_{2}, 0.01 M N a C l$ and $0.5 M A g N O_{3}$ solutions, respectively, then which of the following is true?