The osmotic pressures of $0.1 M N a_{2} S O_{4}$ more than 0.1 M NaCl solutions but osmotic pressure of 0.1 N $N a_{2} S O_{4}$ is less than 0.1 N NaCl,
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Solution

The osmotic pressure of a solution is its colligative property and depends upon the number of particles present in the solution. The dissociation of 1 molecule of $N a_{2} S O_{4}$ gives 3 ions whereas dissociation of 1 molecule of $N a C l$ gives 2 ions. However the molar concentration of $0.1 M N a_{2} S O_{4}$ and 0.1 M NaCl solutions is same. The total number of particles present in $0.1 M N a_{2} S O_{4}$ solution is more than the total number of particles present in 0.1 M NaCl solution Hence, the osmotic pressure of $0.1 M N a_{2} S O_{4}$ more than the osmotic pressure of 0.1 M NaCl solutions.
However, 0.1 N $N a_{2} S O_{4}$ solution corresponds to 0.05 M $N a_{2} S O_{4}$ whereas 0.1 N NaCl solution corresponds to 0.1 M NaCl solution. Hence, the osmotic pressure of 0.1 N $N a_{2} S O_{4}$ is less than the osmotic pressure of 0.1 N NaCl.

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