0.004 M K_2SO_4 solution is isotonic with 0 | vedclass

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

Question

(D) For isotonic solutions, the osmotic pressure $(\pi)$ is equal: $\pi_{K_2SO_4} = \pi_{	ext{glucose}}$.Since $\pi = iCRT$, we have $i_{K_2SO_4} 	i

Vedclass · Accepted Answer

$75$

Vedclass · Answer

(D) For isotonic solutions, the osmotic pressure $(\pi)$ is equal: $\pi_{K_2SO_4} = \pi_{	ext{glucose}}$.Since $\pi = iCRT$, we have $i_{K_2SO_4} 	imes 0.004 	imes RT = 1 	imes 0.01 	imes RT$.Solving for the van't Hoff factor $(i)$: $i = \frac{0.01}{0.004} = 2.5$.For the dissociation of $K_2SO_4$ $(K_2SO_4 ightarrow 2K^+ + SO_4^{2-})$, the number of ions produced $(n)$ is $3$.The degree of dissociation $(\alpha)$ is given by the formula: $i = 1 + (n - 1)\alpha$.Substituting the values: $2.5 = 1 + (3 - 1)\alpha$.$1.5 = 2\alpha$, which gives $\alpha = 0.75$.The percentage dissociation is $\alpha 	imes 100 = 75\%$.

$0.004 \ M \ K_2SO_4$ solution is isotonic with $0.01 \ M$ glucose solution. The percentage dissociation of $K_2SO_4$ is $........$ (Nearest integer).

Similar Questions

For the dissociation of $Na_2SO_4$,how is the degree of dissociation $\alpha$ used to calculate the van't Hoff factor $(i)$?

$A$ $0.2 \ m$ solution of acid $HX$ is $20\%$ ionized in the solution. Given $K_f = 1.86 \ K \ kg \ mol^{-1}$,the freezing point of the solution is ........... $^oC$.

The depression in freezing point for $0.01 \ m$ aqueous solution of $K_{x}[Fe(CN)_6]$ is $0.0744 \ K$. The molal depression constant for solvent is $1.86 \ K \ kg \ mol^{-1}$. If the solute undergoes complete dissociation,what is the correct molecular formula for the solute?

$0.1 \ m$ solutions of sodium sulphate,urea,and sodium chloride are taken. The correct ratio of the elevation of boiling point of these solutions is

$MX_{2}$ dissociates into $M^{2+}$ and $X^{-}$ ions in an aqueous solution,with a degree of dissociation $(\alpha)$ of $0.5$. The ratio of the observed depression of freezing point of the aqueous solution to the value of the depression of freezing point in the absence of ionic dissociation is

Vedclass Test Series

Exam Paper Generator

Online Exam Module