Home
Class 12
CHEMISTRY
Calculate the freezing point depression ...

Calculate the freezing point depression expected for `0.0711` m aqueous solution of `Na_(2)SO_(4)` . If this solution actually freezes at `-0.320 ^(@)C` , what would be the value of Van't Hoff factor ?
(`K_(f)` for water is `1.86 ^(@)C mol^(-1)`) .

Text Solution

AI Generated Solution

To solve the problem, we will follow these steps: ### Step 1: Understand the formula for freezing point depression The freezing point depression (\( \Delta T_f \)) can be calculated using the formula: \[ \Delta T_f = K_f \times m \times i \] where: ...
Promotional Banner

Topper's Solved these Questions

  • XII BOARDS

    XII BOARD PREVIOUS YEAR PAPER ENGLISH|Exercise [SET-I]|71 Videos

  • XII BOARDS

    XII BOARD PREVIOUS YEAR PAPER ENGLISH|Exercise [SET-II]|10 Videos

  • XII BOARDS

    XII BOARD PREVIOUS YEAR PAPER ENGLISH|Exercise Delhi Board : Set - II|7 Videos

  • SAMPLE PAPER 2019

    XII BOARD PREVIOUS YEAR PAPER ENGLISH|Exercise SECTION: D|1 Videos

Similar Questions

Explore conceptually related problems

An aqueous solution containing an ionic salt having molality equal to 0.19 freezes at -0.704^(@)C . The Van't Hoff factor of the ionic salt is ( K_(f) for water= 1.86 K m^(-1) )

The ratio of freezing point depression values of 0.01 M solutions of urea, common salt, and Na_(2)SO_(4) are

0.01 m aqueous solution of K_(3)[Fe(CN)_(6)] freezes at -0.062^(@)C . What is the apparent percentage of dissociation ? ( K_(f) for water = 1.86" K kg mol"^(-1) )

A 0.5% aqueous solution of KCl was found to freeze at -0.24^(@)C . Calculate the Van,t Hoff factor and degree of dissociation of the solute at this concentration. ( 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)

Van't Hoff factor of 0.1 m aqueous solution of Al_2(SO_4)_3 which undergoes 80% dissociation is

What is the expected value of van't Hoff factor for K_(3)[Fe(CN)_(6)] in dilute solution?

The freezing point depression constant for water is 1.86^(@)Cm^(-1) . If 5.00g NaSO_(4) is dissolved in 45.0 g H_(2)O the freezing point is changed by -3.82^(@)C . Calculate the van't Hoff factor for Na_(2)SO_(4) .

The freezing point of a 5g CH_(3)COOH (aq) per 100g water is 01.576^(@)C . The van't Hoff factor (K_(f) of water -1.86K mol^(-1)kg) :

K_(2)HgI_(4) is 55% ionized in aqueous solution. The value of Van't Hoff factor is