A solution of citric acid `C_6H_6O_7` in 50 g of acetic and has boiling point elevation of 1.76 K. if `K_b` for acetic acid is 3.07 K kg `mol^(-1)`, What is the molality of solution?

A solution containing 0.62g of an unknown solute in 50g CCI_4 gavea boiling point elevation of 0.65K. If the molal elevation constant of CCI_4 is 5.02Kkgmol^(-1) Calculate molecular weight of solute:

A 0.1m solution of K_2SO_4 in water has freezing point of -4.3^@C . What is the value of van't Hoff factor if Kf for water is 1.86 K kgmol^(-1) .

2 g of benzoic add (C_6H_5COOH) dissolved in 25 g of benzene shows a depression in freezing point equal to 1.62 K. Molal depression constant for benzene is 4.98 K kg mol^(-1) . What is the percentage assodation of the acid if it forms dimer in solution.

At certain Hill-station pure water boils at 99.725^(@)C . If K_(b) for water is 0.513^(@)C kg mol^(-1) , the boiling point of 0.69m solution of urea will be:

The boiling point of 0.1 molal K_4 [Fe(CN)_6 ] solution will be (given K_b for water = 0.52 k kg mol^(-1))

What is the molality of solution of a certain solute in a solvent .If there is a freezing point depression of 0.184 ""^(@) C and if the freezing point constant is 18.4 K kg mol^(-1) ?

1.00 g of a non-electrolyte solute dissolved in 50 g of benzene lowered the freezing point of benzene of 0.40K. The freezing point depression constant of benzene is 5.12K kgmol^(-1) . Find the molar mass of the solute .

Assuming complete dissociation, calculate the molality of an aqueous solution of KBr whose freezing point is -2.95^@C . K, for water is 1.86 K kg mol^(-1) .