In equimolar solutions of glucose,NaCl,and Ba | vedclass

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

Question

(C) Osmotic pressure $(\pi)$ is a colligative property,which depends on the number of particles in the solution. The formula is $\pi = iCRT$,where $i$

Vedclass · Accepted Answer

$BaCl_2 > NaCl >$ Glucose

Vedclass · Answer

(C) Osmotic pressure $(\pi)$ is a colligative property,which depends on the number of particles in the solution. The formula is $\pi = iCRT$,where $i$ is the van't Hoff factor.For glucose,it is a non-electrolyte,so $i = 1$.For $NaCl$,it dissociates as $NaCl \rightarrow Na^+ + Cl^-$,so $i = 2$.For $BaCl_2$,it dissociates as $BaCl_2 \rightarrow Ba^{2+} + 2Cl^-$,so $i = 3$.Since the solutions are equimolar ($C$ is constant),the osmotic pressure depends directly on $i$. Therefore,the order is $BaCl_2 (i=3) > NaCl (i=2) >$ Glucose $(i=1)$.

In equimolar solutions of glucose,$NaCl$,and $BaCl_2$,the order of osmotic pressure is as follows:

Similar Questions

We have three aqueous solutions of $NaCl$ labelled as $A$,$B$ and $C$ with concentrations $0.1 \ M$,$0.01 \ M$ and $0.001 \ M$,respectively. The value of van 't Hoff factor $(i)$ for these solutions will be in the order:

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

Which solution has the maximum boiling point?

For $0.01 \ M$ solutions of urea,$NaCl$,and $Na_2SO_4$,the ratio of their depression in freezing point is .......

The observed molar mass of an electrolyte is always less than its calculated value because the value of the van't Hoff factor '$i$' is...

Vedclass Test Series

Exam Paper Generator

Online Exam Module