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# Determine the amount of CaCl2 dissolved in 2.5 litre of water such that its osmotic pressure is 0.75 atm at 27°C - CBSE (Science) Class 12 - Chemistry

ConceptColligative Properties and Determination of Molar Mass Osmosis and Osmotic Pressure

#### Question

Determine the amount of CaCl2 (= 2.47) dissolved in 2.5 litre of water such that its osmotic pressure is 0.75 atm at 27°C.

#### Solution

We know that,

pi = n/V RT

=>pi = i w/(MV)RT

=>w = (piMV)/iRT

pi = 0.75 atm

V = 2.5 L

i = 2.47

T = (27+273)K = 300K

Here,

R = 0.0821 L atm K-1mol-1

M = 1 × 40 + 2 × 35.5

= 111g mol-1

Therefore, w = (0.75 x 111 x 2.5)/(2.47xx0.0821xx300)

= 3.42 g

Hence, the required amount of CaCl2 is 3.42 g.

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Solution Determine the amount of CaCl2 dissolved in 2.5 litre of water such that its osmotic pressure is 0.75 atm at 27°C Concept: Colligative Properties and Determination of Molar Mass - Osmosis and Osmotic Pressure.
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