You visited us 1 times! Enjoying our articles? Unlock Full Access!

Osmotic Pressure

QUESTION 2.40...

Question

QUESTION 2.40

Determine the amount of $C a C l_{2}$ (i = 2.47) dissolved in 2.5 L of water such that its osmotic pressure is 0.75 atm at $27^{\circ} C$ .

Open in App

Solution

According to van't Hoff equation
Osmotic pressure $(π) = i C R T = \frac{i n_{B} R T}{V}$
$i = 2.47; V = 2.5 L; R = 0.0821 L a t m K^{- 1} m o l^{- 1}$
$T = 27 + 273 = 300 K; π = 0.75 a t m$
$n_{B} = \frac{π V}{i R T} = \frac{(0.75 a t m) \times (2.5 L)}{(2.47) \times (0.0821 L a t m K^{- 1} m o l^{- 1}) \times (300 K)} = 0.0308 m o l$
Amount of $C a C l_{2}$ dissolved $= n_{B} \times M_{B}$
$= (0.0.08 m o l) \times (111 g m o l^{- 1})$
$= 3.42 g$

Suggest Corrections

Similar questions

C a C l_{2} (i = 2.4)

2.5 l

0.75 atm

27^{\circ} C

R = \frac{1}{12} latm/molK

C a C l_{2} (i = 2.47)

2.5

0.75

27^{\circ} C

C a {C l}_{2}

i = 2.47

2

0.5 a t m

27^{o} C

C a C l_{2}

i = 2.47

2.5 L

300 K

0.75

C a C l_{2}

111 g . m o l^{- 1}

R = 0.082 L . a t m . K^{- 1} m o l^{- 1}

C a C l_{2}

27^{0} C

C a C l_{2}

Join BYJU'S Learning Program