(D) The osmotic pressure $(\pi)$ of a solution is given by the van't Hoff equation: $\pi = iCRT$,where $i$ is the van't Hoff factor,$C$ is the molar c

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Directly proportional to its absolute temperature

(D) The osmotic pressure $(\pi)$ of a solution is given by the van't Hoff equation: $\pi = iCRT$,where $i$ is the van't Hoff factor,$C$ is the molar concentration,$R$ is the gas constant,and $T$ is the absolute temperature in Kelvin. Since $i$,$C$,and $R$ are constants for a given solution,the osmotic pressure $\pi$ is directly proportional to the absolute temperature $T$ (i.e.,$\pi \propto T$).

Class 12 Chemistry Solutions Osmosis and Osmotic pressure of the solution

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The osmotic pressure of a decinormal solution of $BaCl_2$ in water is

A
Inversely proportional to its celsius temperature
B
Inversely proportional to its absolute temperature
C
Directly proportional to its celsius temperature
D
Directly proportional to its absolute temperature

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Osmosis and Osmotic pressure of the solution

Arrange the following solutions according to decreasing order of osmotic pressure under similar conditions of temperature,assuming complete dissociation:
$A. 0.2 \ m \ KCl$
$B. 0.3 \ m \ MgSO_4$
$C. 0.1 \ m \ BaCl_2$
$D. 0.5 \ m \ Al_2(SO_4)_3$

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$A$ $0.6\%$ solution of urea (molecular weight $= 60$) would be isotonic with

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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 $atm$)? $[R=0.082 \ dm^3 \ atm \ mol^{-1} \ K^{-1}]$

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Find the osmotic pressure of a $0.01 \text{ M}$ solution at $25 \text{ }^\circ\text{C}$ $(R = 0.0821 \text{ L atm mol}^{-1} \text{K}^{-1})$. (in $\text{ atm}$)

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Which of the following colligative properties is most suitable for determining the molar mass of polymers?

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The osmotic pressure of a decinormal solution of $BaCl_2$ in water is

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Arrange the following solutions according to decreasing order of osmotic pressure under similar conditions of temperature,assuming complete dissociation:$A. 0.2 \ m \ KCl$$B. 0.3 \ m \ MgSO_4$$C. 0.1 \ m \ BaCl_2$$D. 0.5 \ m \ Al_2(SO_4)_3$

$A$ $0.6\%$ solution of urea (molecular weight $= 60$) would be isotonic with

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 $atm$)? $[R=0.082 \ dm^3 \ atm \ mol^{-1} \ K^{-1}]$

Find the osmotic pressure of a $0.01 \text{ M}$ solution at $25 \text{ }^\circ\text{C}$ $(R = 0.0821 \text{ L atm mol}^{-1} \text{K}^{-1})$. (in $\text{ atm}$)

Which of the following colligative properties is most suitable for determining the molar mass of polymers?

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Arrange the following solutions according to decreasing order of osmotic pressure under similar conditions of temperature,assuming complete dissociation:
$A. 0.2 \ m \ KCl$
$B. 0.3 \ m \ MgSO_4$
$C. 0.1 \ m \ BaCl_2$
$D. 0.5 \ m \ Al_2(SO_4)_3$