The osmotic pressure of a 0.5 M aqueous solu | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(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: $\pi = 1.02 	imes 0.5 	imes RT = 0.51 \ RT$.

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

Similar Questions

The solution from the following with the highest depression in freezing point (lowest freezing point) is:

Identify the false statement from the following.

$1 \, \text{mole}$ of each of $A$ and $B$ form an ideal solution of vapour pressure $100 \, \text{mm Hg}$. Addition of $2 \, \text{moles}$ of $B$ to it decreases the vapour pressure by $20 \, \text{mm Hg}$. The vapour pressure of $A$ and $B$ in pure state are,respectively:

At $100\, ^oC$ the vapour pressure of a solution of $6.5\, g$ of a solute in $100\, g$ water is $732\, mm.$ If $K_b = 0.52,$ the boiling point of this solution will be .........$^oC$

An aqueous solution of urea:

Vedclass Test Series

Exam Paper Generator

Online Exam Module