The following solutions have equal concentrations. Which one will show minimum osmotic pressure?

B a C l_{2}

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A g N O_{3}

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N a_{2} S O_{4}

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(N H_{4})_{3} P O_{4}

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Solution

The correct option is B $A g N O_{3}$
We know that, $P_{i} = C R T \times i$
Since every solution has the same concentration and we assume that all the temperatures are the same (lets say its room temperature but it doesn't matter at all) and R is a constant, the minimum osmotic pressure will be the one which dissolves to the least number of ions.
$a) B a C l_{2} - - - > B a^{2 +} + 2 C l^{-} (3 i o n s)$
$b) A g N O_{3} - - - > A g^{+} + N O 3^{-} (2 i o n s)$
$c) N a 2 S O 4 - - - > 2 N a^{+} + S O_{4}^{2 -} (3 i o n s)$
$d) (N H_{4})_{3} P O_{4} - - - > 3 N H_{4}^{+} + P O^{3 -} (4 i o n s)$
As $A g N O_{3}$ has the least number of ions (2), so its solution has the minimum osmotic pressure.

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