Home
Class 12
CHEMISTRY
If Kf "value of " H2 O is 1.86 ^@C /mola...

If `K_f "value of " H_2 O` is `1.86 ^@C` /molal. The value of `DeltaT_f` for 0.1 m solution of non-volatile solute is

A

18.6

B

0.186

C

1.86

D

0.0186

Text Solution

AI Generated Solution

The correct Answer is:
To find the value of ΔTf for a 0.1 m solution of a non-volatile solute in water, we can use the formula for freezing point depression: ### Step-by-Step Solution: 1. **Identify the given values:** - Kf (freezing point depression constant for water) = 1.86 °C/m (molal) - Molality (m) of the solution = 0.1 m 2. **Write the formula for freezing point depression:** \[ \Delta T_f = K_f \times m \] where ΔTf is the freezing point depression, Kf is the freezing point depression constant, and m is the molality of the solution. 3. **Substitute the known values into the formula:** \[ \Delta T_f = 1.86 \, °C/m \times 0.1 \, m \] 4. **Perform the multiplication:** \[ \Delta T_f = 1.86 \times 0.1 = 0.186 \, °C \] 5. **State the final answer:** The value of ΔTf for a 0.1 m solution of a non-volatile solute is **0.186 °C**.
Promotional Banner

Topper's Solved these Questions

  • LIQUID SOLUTIONS

    VMC MODULES ENGLISH|Exercise IN-CHAPTER EXERCISE -H|10 Videos

  • LIQUID SOLUTIONS

    VMC MODULES ENGLISH|Exercise IN-CHAPTER EXERCISE -I|10 Videos

  • LIQUID SOLUTIONS

    VMC MODULES ENGLISH|Exercise IN-CHAPTER EXERCISE -F|10 Videos

  • LIQUID SOLUTION

    VMC MODULES ENGLISH|Exercise IMPECCABLE|100 Videos

  • MOCK TEST 1

    VMC MODULES ENGLISH|Exercise PART II : CHEMISTRY (SECTION-2)|10 Videos

Similar Questions

Explore conceptually related problems

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 value of K_(f) for water is 1.86^(@) , calculated from glucose solution, The value of K_(f) for water calculated for NaCl solution will be,

A solution containing 8.6 g urea in one litre was found to be isotonic with 0.5% (mass/vol) solution of an organic, non volatile solute. The molecular mass of organic non volatile solute is:

Given that DeltaT_(f) is the depression in freezing point of the solvent in a solution of a non-volatile solute of molarity m ,the quantity underset(m rarr0)(Lt) (DeltaT_(f)//m) is equal to ……………. .

The freezing point of 0.20 M solution of week acid HA is 272.5 K . The molality of the solution is 0.263 "mol" kg^(-1) . Find the pH of the solution on adding 0.25 M sodium acetate solution. K_(f) of water = 1.86 K m^(-1)

0.1mole aqueous solution of NaBr freezes at - 0.335^@C at atmospheric pressure , k_f for water is 1.86^@C . The percentage of dissociation of the salt in solution is

An aqueous solution freezes on 0.36^@C K_f and K_b for water are 1.8 and 0.52 k kg mol^-1 respectively then value of boiling point of solution as 1 atm pressure is

The relative lowering of vapour pressure of an aqueous solution containing a non-volatile solute, is 0.0125. The molality of the solution is

The relative lowering of vapour pressure of an aqueous solution containing a non-volatile solute, is 0.0125. The molality of the solution is

The relative lowering of vapour pressure of an aqueous solution of a non-volatile solute of molecular weight 60 (which neither dissociates nor associates in the solution) is 0.018. If K_(f) of water is 1.86^(@)Cm^(-1) the depression in freezing point will be :