Which of the following $0.1 M$ aqueous solutions will exert the highest osmotic pressure?

A l_{2} (S O_{4})_{3}

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N a_{2} S O_{4}

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M g C l_{2}

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K C l

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Solution

The correct option is A $A l_{2} (S O_{4})_{3}$
1 molecule each of $A l_{2} (S O_{4})_{3}$ , $N a_{2} S O_{4}$ , $M g C l_{2}$ and $K C l$ will dissociate to provide 5, 3, 3 and 2 ions respectively. Thus, $A l_{2} (S O_{4})_{3}$ provides maximum number of ions in aqueous solution.

Hence, $A l_{2} (S O_{4})_{3}$ will exert the highest osmotic pressure for the same concentration.

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