Home
Class 12
CHEMISTRY
Calculate the freezing point of a soluti...

Calculate the freezing point of a solution containing `0.5 ` g KCl (Molar mass = `74.5 ` g/mol) dissolved in 100 g water, assuming KCl to be 92% ionized.
`K_(f)` of water = 1.86 K kg/mol.

Text Solution

Verified by Experts

`KCl to K^(+) + Cl^(-)`
n = 2
` i = 1 - alpha + nalpha`
` i = 1 + alpha`
`Delta T_(f) = iK_(f) m`
` = (1+ 0.92) x 1.86 x(0.5x 1000)/(74.5 x 100)`
` DeltaT_(f) = 0. 24`
` Delta T _(f) = 0.24`
` DeltaT_(f)=T_(f)^(0) - T_(f)`
` T'_(f) =- 0.24^(@) C`
Doubtnut Promotions Banner Mobile Dark
|

Topper's Solved these Questions

  • SAMPLE PAPER 2019

    XII BOARD PREVIOUS YEAR PAPER ENGLISH|Exercise SECTION: D|1 Videos
  • SAMPLE PAPER 2019

    XII BOARD PREVIOUS YEAR PAPER ENGLISH|Exercise SECTION -B|8 Videos
  • EXAM REVISION SERIES

    XII BOARD PREVIOUS YEAR PAPER ENGLISH|Exercise All Questions|28 Videos
  • XII BOARDS

    XII BOARD PREVIOUS YEAR PAPER ENGLISH|Exercise SET - II|12 Videos

Similar Questions

Explore conceptually related problems

Calculate the freezing point of a solution containing 8.1 g of HBr in 100g of water, assuming the acid to be 90% ionized. [Given : Molar mass Br = 80 g/mol, K_(f) water = 1.86 K kg/mol].

Calculate the freezing point of solution when 1.9 g of MgCl_(2) (M = 95 g Mol^(-1) ) was dissolved in 50g of water, assuming MgCl_(2) undergoes complete ionization. ( K_(f) for water = 1.86 K kg mol^(-1) ).

Calculate the freezing point of a solution containing 60 g glucose (Molar mass = 180 g mol^(-1) ) in 250 g of water . ( K_(f) of water = 1.86 K kg mol^(-1) )

The freezing point of a solution containing 0.1g of K_3[Fe(CN)_6] (Mol. Wt. 329) in 100 g of water ( K_f =1.86K kg mol^(−1) ) is:

Calculate the freezing point of an aqueous solution containing 10.50 g of MgBr_(2) in 200 g of water (Molar mass of MgBr_(2) = 184g ). ( K_(f) for water = 1.86" K kg mol"^(-1) )

Calculate the boiling point of solution when 4g of Mg SO_(4) (M=120g "mol"^(-1)) was dissolved in 100g of water, assuming MgSO_(4) undergoes complete ionization (K_(b) " for water " = 0.52 K " kg mol"^(-1))

Calculate the freezing point of an aqueous solution containing 10.5g of Magnesium bromide in 200 g of water, assuming complete dissociation of Magnesium bromide. (Molar mass of magnesium bromide =184 g mol ^(-1) , for water =1.86K kg mol^(-) ).

Calculate the freezing point of 1 molal NaCl solution assuming NaCl to be 100% dissociated in water. ( K_(f) for water = 1.86^(@)"mol"^(-) ).

The freezing point of a solution that contains 10 g urea in 100 g water is ( K_1 for H_2O = 1.86°C m ^(-1) )

A molecule A_(x) dissovle in water and is non volatile. A solution of certain molality showed a depression of 0.93K in freezing point. The same solution boiled at 100.26^(@)C . When 7.87g of A_(x) was dissovled in 100g of water, the solution boiled at 100.44^(@)C . Given K_(f) for water =1.86K kg "mol"^(-1) . Atomic mas of A=31u . Assume no association or dissociatioin of solute. Calculate the value of x ........