(C) The formula for osmotic pressure $(\pi)$ is given by: $\pi = i \times C \times R \times T$ Where: $i = 1.125$ (van't Hoff factor) $C = 0.1 \ M$ (m

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(C) The formula for osmotic pressure $(\pi)$ is given by: $\pi = i \times C \times R \times T$ Where: $i = 1.125$ (van't Hoff factor) $C = 0.1 \ M$ (molar concentration) $R = 0.0821 \ atm \ dm^3 \ K^{-1} \ mol^{-1}$ (gas constant) $T = 300 \ K$ (temperature) Substituting the values: $\pi = 1.125 \times 0.1 \times 0.0821 \times 300$ $\pi = 1.125 \times 0.1 \times 24.63$ $\pi = 1.125 \times 2.463$ $\pi = 2.770875 \ atm$ Rounding to two decimal places,we get $\pi \approx 2.77 \ atm$.

Class 12 Chemistry Solutions Osmosis and Osmotic pressure of the solution

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Calculate the osmotic pressure of a $0.1 \ M$ aqueous solution of an electrolyte at $300 \ K$ if the van't Hoff factor is $1.125$. $[R = 0.0821 \ atm \ dm^3 \ K^{-1} \ mol^{-1}]$ (in $atm$)

MHT CET 2025 All MHT CET

A
$2.15$
B
$2.41$
C
$2.77$
D
$3.25$

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Osmosis and Osmotic pressure of the solution

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Calculate the osmotic pressure of a $0.1 \ M$ aqueous solution of an electrolyte at $300 \ K$ if the van't Hoff factor is $1.125$. $[R = 0.0821 \ atm \ dm^3 \ K^{-1} \ mol^{-1}]$ (in $atm$)

Similar Questions

When the temperature of a certain solution is increased from $37\, ^\circ C$ to $327\, ^\circ C$,how many times will the osmotic pressure change?

$A$ $5\% \ (w/v)$ solution of anhydrous $CaCl_2$ at $0^o C$ exerts an osmotic pressure of $15 \ atm$. The degree of dissociation $(\alpha)$ of $CaCl_2$ is ....... $\%$.

Which one of the following solutions of compounds shows the highest osmotic pressure? ($AB, AB_2$ and $A_2 B_3$ are ionic compounds)

$A$ graph of osmotic pressure $(\pi)$ vs molarity $(M)$ of an aqueous solution of $NaCl$ at room temperature is given below. The slope of the line represents :-

$A$ solution containing $4 \ g$ of polymer in $4.0 \ L$ solution at $27^{\circ} C$ shows an osmotic pressure of $3.0 \times 10^{-4} \ atm$. The molar mass of the polymer in $g \ mol^{-1}$ is

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