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:

The boiling point of 0.15 molal aqueous solution of an unknown solute is 373.23 K at 1 atm. The molal elevation constant of water is ______ K kg mol ^(-1)

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?

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 .

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) ?

The ionization constant of base is 5.4 xx 10^(-4) . Calculate its degree of ionization in its 0.02 M solution.

The dissociation constant of NH_4OH is 1.8 xx 10^(-5) . Calculate its degree of dissociation in 0.01 M solution.

0.15 molal solution of a substance boils at 373.23 K. Calculate molal elevation constant of water, (Given boiling point of water=373.15K)

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))