In a 0.2 molal aqueous solution of a weak acid HX the degree of dissociation is 0.25. The freezing point of the solution will be nearest to: (`K_(f)=1.86 K kg "mol"^(-1)`)
A
`-0.26^(@)C`
B
`0.465^(@)C`
C
`-0.48^(@)C`
D
`-0.465^(@)C`
Text Solution
Verified by Experts
The correct Answer is:
d
Topper's Solved these Questions
DILUTE SOLUTION
NARENDRA AWASTHI|Exercise Level 2|1 Videos
DILUTE SOLUTION
NARENDRA AWASTHI|Exercise Level 3 - Match The Column|1 Videos
A 0.5 molal aqueous solution of a weak acid (HX) is 20 percent ionized. The lowering in freezing point of this solution is ( K_f = 1.86 K/m for water)
Equal volumes of 1.0M AgNO_(3) and 1.0M KCl are mixed . The depression of freezing point of the resulting solution will be (K_(f)(H_(2)O)=1.86 K kg "mol"^(-1), 1M=1m)
The P^(H) of a weak mono basic acid is 5. The degree of ionisation of acid in 0.1 M solution is
1.0 molal aqueous solution of an electrolyte X_(3)Y_(2) is 25% ionized. The Boiling point of the solution is (K_(b) of H_(2)O=0.52K kg mol^(-1))
12.25 g of CH_(3)CH_(2)CHCICOOH is added to 250 g of water to make a solution . If the dissociation constant of above acid is 1.44xx10^(-3) the depression in freezing point of water in ""^(@)C "is" (K_(f) for water is 1.86 K kg "mol"^(-1))
A solution of sucrose (molar mass 342 "gmol"^(-1) ) has been produced by dissolving 68.5g sucrose in 1000g water. The freezing point of the solution obtained will be ( K_f for H_2O = 1.86 kg "mol"^(-1) )
The elevation in boling point of an aqueous solutions of NaCl is 0.01 .^(@) C . If its van't Hoff factor is 1.92 ,the molality of NaCl solution is ( K_(b) for water = 0 . 52 k kg mol^(-1) )
31 g of ethylene glycol (C_2H_6O_2) is dissolved in 600g of water. The freezing point depression of the solution is (K_f for water is 1.86 K Kg mol^-1)
NARENDRA AWASTHI-DILUTE SOLUTION-Level 3 - Match The Column
