The osmotic pressure of a 0.5 M aqueous solu | vedclass

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(A) The osmotic pressure $\pi$ is given by the formula $\pi = iCRT$,where $i$ is the van't Hoff factor,$C$ is the molar concentration,$R$ is the gas c

Vedclass · Accepted Answer

$0.51$

Vedclass · Answer

(A) The osmotic pressure $\pi$ is given by the formula $\pi = iCRT$,where $i$ is the van't Hoff factor,$C$ is the molar concentration,$R$ is the gas constant,and $T$ is the temperature.For $CH_3COOH ightleftharpoons CH_3COO^- + H^+$,the degree of dissociation $\alpha$ is related to $[H^+]$.Given $pH = 2$,so $[H^+] = 10^{-pH} = 10^{-2} = 0.01 \ M$.Since $[H^+] = C \alpha$,we have $0.01 = 0.5 	imes \alpha$,which gives $\alpha = 0.01 / 0.5 = 0.02$.The van't Hoff factor $i = 1 + \alpha = 1 + 0.02 = 1.02$.Substituting the values into the osmotic pressure formula: $\pi = 1.02 	imes 0.5 	imes RT = 0.51 \ RT$.

List-$I$	List-$II$
$A$. Solution of chloroform and acetone	$I$. Minimum boiling azeotrope
$B$. Solution of ethanol and water	$II$. Dimerizes
$C$. Solution of benzene and toluene	$III$. Maximum boiling azeotrope
$D$. Solution of acetic acid in benzene	$IV$. $\Delta V_{mix}=0$

The osmotic pressure of a $0.5 \ M$ aqueous solution of $CH_3COOH$ having a $pH$ of $2$ at temperature $T$ is . . . . . . . (in $RT$)

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