What will be the freezing point of 0.2 molal aqueous solution of `MgBr_(2)` ? If salt dissociates 40% in solution and `K_(f)` for water is 1.86 KKg `mol^(-1)`

The lowering in freezing point of 0.75 molal aqueous solution NaCI (80% dissociated) is [Given, K_f , for water 1.86 K kg mol^(-1)]

A weak electrolyte XY is 5% dissociated in water. What is the freezing point of a 0.01 molal aqueous solution of XY ? The cryoscopic constant of water is 1.86 K/m.

A weak electrolyte XY is 5% dissociated in water. What is the freezing point of a 0.01 molal aqueous solution of XY ? The cryoscopic constant of water is 1.86 K/m.

The lowering in freezing point of 0.75 molal aqueous solution NaCI (80% dissociated) is [Given, K_f, for water 1.86 K kg mol^(-1)]

The freezing point of an aqueous solutions is 272 .93 K . Calculate the molality of the solution if molal depression constant for water is 1.86 Kg mol^(-1)

Calculate the freezing point of 1 molal NaCl solution assuming NaCl to be 100% dissociated in water. ( K_(f) for water = 1.86^(@)"mol"^(-) ).

Calculate the freezing point of an aqueous solution containing 10.50 g of MgBr_(2) in 200 g of water (molar mass of MgBr_(2) = 184 g. K_(f) for water = 1.86 K kg mol^(-1) )

The freezing point of 1 molal NaCl solution assuming NaCl to be 100% dissociated in water is (Molal depression constant of water=1.86Kkg/mol)

Calculate the freezing point of an aqueous solution containing 10.50 g of MgBr_(2) in 200 g of water (Molar mass of MgBr_(2) = 184g ). ( K_(f) for water = 1.86" K kg mol"^(-1) )

The expression in freezing point of a 0.1 molal solution of a substance is 0.372^@ C. what can you say about the solute? (K_f for water is 1.86 K kg mol^(-1))