wiz-icon
MyQuestionIcon
MyQuestionIcon
1
You visited us 1 times! Enjoying our articles? Unlock Full Access!
Question

QUESTION 2.41

Determine the osmotic pressure of a solution prepared by dissolving 25 mg of K2SO4 in 2L of water at 25C, assuming that it is completely dissociated.

Open in App
Solution

Amount of K2SO4 dissolved = 25 mg = 0.025g
Volume of solution = 2L
T=25C=25+273K=298K
Molar mass of
K2SO4=(2×39)+(32)+(4×16)=174 g mol1
Since, K2SO4 dissociates completely as
K2SO4aq2K++SO24
Total ions produced after dissociation (per mole) = 3
So, i = 3, π=iCRT=i×nVRT=i×W×R×TM×V
=3×(0.025g)×(0.0821 L atm K1 mol1)×(298K)(174 g mol1)×(2L)
=5.27×103 atm


flag
Suggest Corrections
thumbs-up
55
Join BYJU'S Learning Program
similar_icon
Related Videos
thumbnail
lock
Osmotic Pressure
CHEMISTRY
Watch in App
Join BYJU'S Learning Program
CrossIcon