34.2 gm Sucrose (Molecular wt 342) is dissolved in 1000 gm of water. Find the freezing-point of the solution `kf = 1.86 K Kg mol^-1`

KBr is 80% dissociated in aqueous solution. The freezing point of a 0.5 molal solution is K_f =1.86 K kg mol^-1

A solution contains 5.6 gm of glucose in 1000 gm of water. Calculate the boiling point of the solution. ( k_b for water = 0.52 K kg mol^-1 )

How much quantity of ethylene glycol is added in 200 gm water to reduce the freezing point by 0.93K? Kf=1.86K. Kg mol^(-1)

The elevation of boiling poin is 0.70K when 12.5gm of a non electrolyte gets dissolved in 175 gm of water. Cacluate mole mass of the substance K_b =52K Kg mol^(-1)

Dry air was passed successively through a solution of 5 gm of solute dissolved in 80.0 gm of water and through pure water. The loss in weight of the solution was 2.5 gm and that of the pure solvent was 0.04 gm. What is the molecular weight of the solute?

A 0.2 molal aqueous solution of weak acid HX is 20% ionized. The freezing point of solution is ( K_f =1.86 )

58.5 gm of NaCl and 180 gm of glucose were separately dissolved in 1000 ml of water. Identify the correct statement regarding the elevation of boiling point (b.p.) of the resulting solutions.

2.00 g of non=electrolyte solute dissolved in 100 g of benzene lowered the freezing point of benzene by 0.50K. The freezing point depression constant of benzene is 5.12 K kg mol^(-1) . Find out the relative molar mass of the solute.

When 45 g of an unknown compound was dissolved in 500 g of water, the solution has freezing point of -0.93^(@)C (i) What is the molecular weight of compound ? (K_(f)=1.86) (ii) If empirical formula is CH_(2)O , what is the molecular formula of compound ?

What is the freezing point of solution containing 3g of a non-volatile solute in 20g of water. Freezing point of pure water is 273K, K_(f) of water = 1.86 Kkg/mol. Molar mass of solute is 300 g/mol. T^(@)-T=K_(f)m