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  4. What amount of CaCl2 (i = 2.47) is dissolved in 2 litres of water so that its osmotic pressure is 0.5 atm at 27 °C?

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Q. What amount of $CaCl_2 \,(i = 2.47)$ is dissolved in $2$ litres of water so that its osmotic pressure is $0.5\, atm$ at $27\,{}^°C$?

Solutions

Solution:

$\pi = iCRT = i \frac{n}{V} RT$
$n = \frac{\pi \times V}{i\times R\times T}$
$= \frac{0.5 \times 2}{2.47 \times 0.0821 \times 300} = 0.0164\,mol$
Amount of $CaCl_{2} = n \times M= 0.0164 \times 111 = 1.820 \,g$