The relationship between the values of osmotic pressure of 0.1 M solutions of $K N O_{3} (P_{1})$ and $C H_{3} C O O H (P_{2})$ is:

P_{1} > P_{2}

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P_{2} > P_{1}

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P_{1} = P_{2}

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\frac{P_{1}}{P_{1} + P_{2}} = \frac{P_{2}}{P_{1} + 2 P_{2}}

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Solution

The correct option is B $P_{1} > P_{2}$
Since $K N O_{3}$ is a strong electrolyte, so it undergoes 100% dissociation but $C H_{3} C O O H$ is a weak electrolyte. Therefore, $P_{1} > P_{2}$ .

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The relationship between the values of osmotic pressure of 0.1 M solutions of KNO3(P1) and CH3COOH(P2) is:

The correct option is B P1>P2Since KNO3 is a strong electrolyte, so it undergoes 100% dissociation but CH3COOH is a weak electrolyte. Therefore, P1>P2.

The relationship between the values of osmotic pressure of 0.1 M solutions of $K N O_{3} (P_{1})$ and $C H_{3} C O O H (P_{2})$ is:

The correct option is B $P_{1} > P_{2}$
Since $K N O_{3}$ is a strong electrolyte, so it undergoes 100% dissociation but $C H_{3} C O O H$ is a weak electrolyte. Therefore, $P_{1} > P_{2}$ .