JEE MAIN - Chemistry (2019 - 9th April Evening Slot - No. 2)
Molal depression constant for a solvent is
4.0 kg mol–1. The depression in the freezing
point of the solvent for 0.03 mol kg–1 solution
of K2SO4 is :
(Assume complete dissociation of the electrolyte)
(Assume complete dissociation of the electrolyte)
0.18 K
0.24 K
0.36 K
0.12 K
Explanation
K2SO4 $$ \to $$ 2K+ + SO42-
Van’t Hoff Factor (i) = 3
$$ \therefore $$ $$\Delta $$Tf = ikfm
= 3 $$ \times $$ 4 $$ \times $$ 0.03 = 0.36 K
Van’t Hoff Factor (i) = 3
$$ \therefore $$ $$\Delta $$Tf = ikfm
= 3 $$ \times $$ 4 $$ \times $$ 0.03 = 0.36 K
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