Molar depression constant for a solvent is 4.0 K kg 
. The depression in the freezing point of the solvent for 0.03 mol 
solution of K2SO4 is (Assume complete dissociation of the electrolytes)
(a)
0.36 k
(b)
0.18 k
(c)
0.12 k
(d)
0.24 k
Molar depression constant for a solvent is 4.0 K kg . The depression in the freezing point of the solvent for 0.03 mol solution of K2SO4 is (Assume complete dissociation of the electrolytes)
(a)
0.36 k
(b)
0.18 k
(c)
0.12 k
(d)
0.24 k
Question ID - 52646 | SaraNextGen Top Answer
Molar depression constant for a solvent is 4.0 K kg . The depression in the freezing point of the solvent for 0.03 mol solution of K2SO4 is (Assume complete dissociation of the electrolytes)
(a)
0.36 k
(b)
0.18 k
(c)
0.12 k
(d)
0.24 k
|
Molar depression constant for a solvent is 4.0 K kg |
|||
|
(a) |
0.36 k |
(b) |
0.18 k |
|
(c) |
0.12 k |
(d) |
0.24 k |
1 Answer
127 votes
Answer Key / Explanation : (a) -
K2SO4
2K+ + SO42−
I(can’t Hoff Factor)=3
∴
=iKf m
=3×4×0.03
=0.36 k
127 votes
Answer Link
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