Home
Class 12
CHEMISTRY
The freezing point of 1 molal NaCl solut...

The freezing point of `1` molal `NaCl` solution assuming `NaCl` to be `100%` dissociated in water is:

A

(a) `-1.86^(@)C`

B

(b) `-3.72^(@)C`

C

(c ) `+1.86^(@)C`

D

(d) `+3.72^(@)C`

Text Solution

Verified by Experts

The correct Answer is:
B
`Delta T_(f) = 1.86 xx 1 xx 2 = 3.72`,
`:. T_(f) = 0-3.72 = -3.72^(@)C`
`NaCl` dissociates to give experimental molality `= 1xx2=2`
Promotional Banner

Topper's Solved these Questions

  • DILUTE SOLUTION AND COLLIGATIVE PROPERTIES

    P BAHADUR|Exercise Exercise 3B Objectice Problems|1 Videos

  • DILUTE SOLUTION AND COLLIGATIVE PROPERTIES

    P BAHADUR|Exercise Exercise 9 Advanced Numerical|12 Videos

  • CHEMICAL KINETICS

    P BAHADUR|Exercise Exercise 9|13 Videos

  • ELECTROCHEMISTRY

    P BAHADUR|Exercise Exercise (9) ADVANCED NUMERICAL PROBLEMS|36 Videos

Similar Questions

Explore conceptually related problems

The freezing point of one molal NaCl solution assuming NaCl to be 100% dissociated in water is (molal depression constant= 1.86)

The lowering in freezing point of 0.75 molal aqueous solution NaCI (80% dissociated) is [Given, K_f , for water 1.86 K kg mol^(-1)]

What will be the freezing point of 0.2 molal aqueous solution of MgBr_(2) ? If salt dissociates 40% in solution and K_(f) for water is 1.86 KKg mol^(-1)

A weak electrolyte XY is 5% dissociated in water. What is the freezing point of a 0.01 molal aqueous solution of XY ? The cryoscopic constant of water is 1.86 K/m.

The molal depression constant for water is 1.86^(@)C . The freezing point of a 0.05-molal solution of a non-electrolyte in water is

The freezing point of a 0.05 molal solution of a non-electrolyte in water is: ( K_(f) = 1.86 "molality"^(-1) )

A solution of NaCl in water is…..

The freezing point depression of 0.1 molal NaCl solution is 0.372 K. What conclusion can you draw about the molecular state of NaCl in water. K_f of water = 1.86 k/m.