Caculate the mass of a compound `(molar mass=256g mol^-1)` to be dissolved in 75g of benzene to lower its freezing point by 0.48K `(K_f=5.12 K kg mol^-1)`

What mass of NaCl (molar mass= 58.5 g mol^-1 ) must be dissolved in 65.0 g of water to lower the freezing point by 7.50 ^@C ? The freezing point depression constant, K_f , for water is 1.86 K kg mol^-1 . Assume Van's Hoff factor for NaCl is 1.87.

Calculate the amount of CaCl_(2) (molar mass = 111g "mol"^(-1) ) which must be added to 500 g of water of lower its freezing point by 2K, assuming CaCl_(2) is completely dissociated. (Kf for water = 1.86 k kg "mol"^(-1) ).

Calculate the mass of a non-volatile solute ( molar mass 40g mol^-1 ) which should be dissolved in 114g octane to reduce its vapour pressure to 80%.

The mass of a non-volatile solute of molar mass 40gmol^-1 that should be dissolved in 114 g of octane to lower its vapour pressure by 20% is

1 g of non - electrolyte solute (molar mass 250 g/mol) was dissolved in 5.12g of benzene. If the freezing point of depression constant, k_f of benzene is 5.12 K kg/mol, the freezing point of benzene will be lowered by

2.1 g of non-electrolyte solute (molar mass 250 g/mol) was dissolved in 5.12 g of benzene. If the freezing point of depression constant, k_f of benzene is 5.12 K kg/mol, Calculate the freezing point of benzene.

Two elements A and B form compounds having formula AB2 and AB4. When dissolved in 20 g of benzene (C_6H_6), 1 g of AB_2 lowers the freezing point by 2.3 K whereas 1.0 g of AB_4 lowers it by 1.3 K. The molar depression constant for benzene is 5.1 K kg mol^(-1) . Calculate atomic masses of A and B.

2.82g of glucose (Molar mass: 180g mol^-1 ) are dissolved in 30g of water . Calculate mole fraction of glucose and water.

Calculate mass of 2.7moles of C_(12)H_(22)O_(11) (molar mass = 342 g/ mol)

Addition of 0.643g of a compound to 43.95g of benzene lowers the freezing point from 5.51^@ C to 5.03^@ C. If K_f for benzene is 5.12K kg mol^-1 , calculate the molar mass of the compound.