Calculate the mass of ascorbic acid (Vitamin C, `C_6H_8O_6)` to be dissolved in 75 g of acetic acid to lower its melting by `1.5^@C. K_f =3.9K kg mol^-1`.

Ethylene glycol is used as antifreezing agent to prevent the freezing of water in car radiator in cold climate. Calculate the amount of ethylene glycol to be added to 5 kg of water to prevent it from freezing at -6^@C . Given K_f for water = 1.85 kg mol^-1 .

Calculate the mass percentage of benzene (C_6H_6) and carbon tetrachloride (C Cl_4) if 22g of benzene is dissolved in 122g of carbon tetrachloride.

When 20 g of naphthoic acid (C_11H_8O_2) is dissolved in 50 g of benzene , a freezing point depression of 2K is observed. The vant Hoff factor (i) is [ K_f="1.72 K kg mol"^(-1) ]

Calculate the elevation of boiling point of water when 0.6 gm urea is dissolved in 250 ml water given [ K_b 0.52 k.kg mol^(-1) ]

The freezing point of benzene decreases by 0.45^(@)C when o.2g of acetic acid is added to 20 g of benzene . If acetic acid associates to form a dimer in benzene, percentage association of acetic acid in benzene will be - ( K_(f) for benzene = 5.12. kg. mol^(-1) )

Calculate the pH of 0.1 (N) acetic acid solution. Given: K_(a) (acetic acid) =1.8xx10^(-5)

Calculate the normality of solution containing 3.15 g of hydrated oxalic acid (H_2C_2O_4. 2H_2O) in 250 ml of solution ( Mol. Mass = 126).

Calculate the total pressure in a mixture of 8g of oxygen and 4 g of hydrogen confined in a vessel of Idm^3 at 27^@C [R= 0 08 bar. dm_3. k^-1 mol^-1]

The depression in the freezing point of a benzene solution containing 0.784g of Acetic acid dissolved in 100ml of benzene is 0.35k. Calculate the van't Hoff factor and the degree of association of the solute at this concentration (k_(f)" for benzene = 5.10 k.kg.mol"^(-1)," molar mass of acetic acid is 60.01").

A solution of 2.44xx10^-3 kg of a nonelectrolyte solute dissolved in 0.075 kg of water boiled at 100.413^@C . Calculate the molecular mass of the solute. K_b for water = 0.52 K kg mol^-1