A 0.10 M solution of a mono protic acid (`d=1.01g//cm^(3)`) is 5% dissociated what is the freezing point of the solution the molar mass of the acid is 300 and `K_(f)(H_(2)O)=1.86C//m`

A 0.10 M solution of a monoprotic acid ( d=1.01g//cm^(3) ) is 5% dissociated what is the freezing point of the solution the molar mass of the acid is 300 and K_(f)(H_(2)O)=1.86C//m

A 0.10 M aqueous solution of a monoprotic acid ("d=1.01 g/cm"^3) is 5% ionized. What is the freezing point of the solution? The mol.wt. of the acid is 300 and K_f (H_(2)O)="1.86"^@C//m:

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) )

If 0.1 m aqueous solution of calcium phosphate is 80% dissociated then the freezing point of the solution will be (K_f of water = 1.86K kg mol^(-1))

If 0.1 m aqueous solution of calcium phosphate is 80% dissociated then the freezing point of the solution will be ( K_f of water = 1.86K kg mol^(-1))

If 0.2 molal aqueous solution of a weak acid (HA) is 40% ionised then the freezing point of the solution will be ( K_f for water = 1.86^@ C