(B) The formula for osmotic pressure is $\pi = iMRT = \frac{i \times W_2 \times R \times T}{M_2 \times V}$.Given values are: $i = 2.47$,$W_2 = 1.7 \ g

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

(B) The formula for osmotic pressure is $\pi = iMRT = \frac{i \times W_2 \times R \times T}{M_2 \times V}$.Given values are: $i = 2.47$,$W_2 = 1.7 \ g$,$R = 0.082 \ dm^3 \ atm \ mol^{-1} \ K^{-1}$,$T = 300 \ K$,$M_2 = 111 \ g \ mol^{-1}$,and $V = 1.25 \ dm^3$.Substituting these values into the formula:$\pi = \frac{2.47 \times 1.7 \times 0.082 \times 300}{111 \times 1.25} \ atm$.$\pi = \frac{103.3638}{138.75} \ atm$.$\pi = 0.744 \ atm$.

Class 12 Chemistry Solutions Osmosis and Osmotic pressure of the solution

Medium

What is the osmotic pressure of a solution of $1.7 \ g$ of $CaCl_2$ in $1.25 \ dm^3$ of water at $300 \ K$,if the van't Hoff factor and molar mass of $CaCl_2$ are $2.47$ and $111 \ g \ mol^{-1}$ respectively (in $atm$)? $[R=0.082 \ dm^3 \ atm \ mol^{-1} \ K^{-1}]$

MHT CET 2023 All MHT CET

A
$0.625$
B
$0.744$
C
$0.827$
D
$0.936$

Explore More

Browse All

Question Bank

All Subjects

Class 12 Questions

Class 12

Chemistry Questions

Chapter

Solutions

Subtopic

Osmosis and Osmotic pressure of the solution

Previous Year

MHT CET 2023 Paper All MHT CET years →

Which of the following $0.1 \ M$ solutions has the maximum osmotic pressure at $25^o \ C$?

Easy

View Solution

$A$ $5\% \text{ (w/v)}$ solution of cane sugar (molar mass = $342 \text{ g/mol}$) is isotonic with a $1\% \text{ (w/v)}$ solution of an unknown solute. What is the molar mass of the unknown solute in $\text{g/mol}$?

Medium

View Solution

For a very dilute solution of an electrolyte,which of the following relations is correct? (Assume other parameters are constant)

Medium

View Solution

What will be the osmotic pressure of $0.2 \ M$ $K_4[Fe(CN)_6]$ at $27^{\circ} C$ (in $atm$)?

Medium

View Solution

Calculate the molar mass of a solute when $4 \ g$ of it is dissolved in $1 \ dm^3$ of solvent,having an osmotic pressure of $2 \ atm$ at $300 \ K$. $[R = 0.082 \ dm^3 \ atm \ K^{-1} \ mol^{-1}]$

EasyMHT CET 2024

View Solution

Vedclass Products

For Students

Vedclass Test Series

Mock tests in real JEE/NEET style with performance analysis. 5-day free trial.

Start Free Trial

For Teachers

Exam Paper Generator

Generate Set A/B/C/D exam papers from 7.5L+ questions in 2 minutes. 3 chapters free.

Try Free

For Institutes

Online Exam Module

Live online exams with unlimited students, 360° analytics & white-label branding.

See Demo

What is the osmotic pressure of a solution of $1.7 \ g$ of $CaCl_2$ in $1.25 \ dm^3$ of water at $300 \ K$,if the van't Hoff factor and molar mass of $CaCl_2$ are $2.47$ and $111 \ g \ mol^{-1}$ respectively (in $atm$)? $[R=0.082 \ dm^3 \ atm \ mol^{-1} \ K^{-1}]$

Similar Questions

Which of the following $0.1 \ M$ solutions has the maximum osmotic pressure at $25^o \ C$?

$A$ $5\% \text{ (w/v)}$ solution of cane sugar (molar mass = $342 \text{ g/mol}$) is isotonic with a $1\% \text{ (w/v)}$ solution of an unknown solute. What is the molar mass of the unknown solute in $\text{g/mol}$?

For a very dilute solution of an electrolyte,which of the following relations is correct? (Assume other parameters are constant)

What will be the osmotic pressure of $0.2 \ M$ $K_4[Fe(CN)_6]$ at $27^{\circ} C$ (in $atm$)?

Calculate the molar mass of a solute when $4 \ g$ of it is dissolved in $1 \ dm^3$ of solvent,having an osmotic pressure of $2 \ atm$ at $300 \ K$. $[R = 0.082 \ dm^3 \ atm \ K^{-1} \ mol^{-1}]$

Vedclass Test Series

Exam Paper Generator

Online Exam Module