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

Π_{1} = Π_{2}

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Π_{2} > Π_{1}

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

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Π_{1} > Π_{2}

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Solution

The correct option is D $Π_{1} > Π_{2}$
We have,
$Π = i C R T$

$K N O_{3}$ is an ionic salt and completely dissociated and have $i = 2$

$C H_{3} C O O H$ is weak acid and partially dissociated in solution,

so, $Π_{1} = 2 C R T$ and $Π_{1} = C R T$

$∴ Π_{1} > Π_{2}$

Hence, option(D) is correct.

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The relationship between the values of osmotic pressure of 0.1 M solutions of KNO3 (Π1) and CH3COOH(Π2) is:

The correct option is D Π1>Π2We have,Π=iCRTKNO3 is an ionic salt and completely dissociated and have i=2CH3COOH is weak acid and partially dissociated in solution,so, Π1=2CRT and Π1=CRT ∴Π1>Π2Hence, option(D) is correct.

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