The osmotic pressure of a dilute solution of | vedclass

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

Question

(B) 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

$6 	imes 10^{-2}$

Vedclass · Answer

(B) 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 $XY$,which dissociates as $XY ightarrow X^+ + Y^-$,the van't Hoff factor $i = 2$.For $BaCl_2$,which dissociates as $BaCl_2 ightarrow Ba^{2+} + 2Cl^-$,the van't Hoff factor $i = 3$.Given that $\pi_{XY} = 4 	imes \pi_{BaCl_2}$,we have:$2 	imes C_{XY} 	imes RT = 4 	imes (3 	imes 0.01 	imes RT)$$2 	imes C_{XY} = 0.12$$C_{XY} = 0.06\, M = 6 	imes 10^{-2}\, mol\, L^{-1}$.

The osmotic pressure of a dilute solution of an ionic compound $XY$ in water is four times that of a solution of $0.01\, M\, BaCl_2$ in water. Assuming complete dissociation of the given ionic compounds in water,the concentration of $XY$ (in $mol\, L^{-1}$) in solution is

Similar Questions

Which of the following salts has the same value of Van't Hoff factor $i$ as that of $K_4[Fe(CN)_6]$?

The molal elevation constant of water is $0.51 \ K \, kg \, mol^{-1}$. The boiling point of $0.1 \ m$ aqueous $NaCl$ solution is nearly .......... $^oC$.

The freezing point of equimolal aqueous solution will be highest for

$0.2 \ molal$ aqueous solution of an electrolyte $A_3B$ is $90\%$ ionised. The boiling point of the solution at $1 \ atm$ is ........ $K.$ ($K_b$ for $H_2O = 0.52 \ K \ Kg \ mol^{-1}$ and $B.pt.$ of $H_2O = 373 \ K$)

What is the percentage of dissociation of a $0.011 \ m$ aqueous solution of $K_3[Fe(CN)_6]$ having a freezing point of $-0.063 \ ^oC$? (Given: $K_f = 1.86 \ K \ kg \ mol^{-1}$ for water)

Vedclass Test Series

Exam Paper Generator

Online Exam Module