1.0 g of a nonelectrolyte solute dissolved in 50g of benzene lowered the freezing point of benzene by 0.40 K. The freezing point depression constant of benzene is 5.12 K kg mol. Find the molar mass of the solute.

2g of a non-electrolyte solute dissolved in 100g of benzene lowered the freezing point of benzene by 0.40 K. find the molar mass of the solute.

What mass of NaCl (molar mass= 58.5g mol^-1) must be dissolved in 65g of water to lower the freezing point by 7.5^@C ? The freezing point depression constant, K_f for water is 1.86 K kg mol^-1 . Assume vant Hoff factor for NaCl is 1.87.

Two elements A and B form compounds having formula AB_2 and AB_4 . 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.

A 0.561 m solution of an unknown electrolyte depresses the freezing point of water by 2.93^@C . What is Vant Hoff factor for this electrolyte? The freezing point depression constant (K_f) for water is 1.86^@C Kg mol^-1 .

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

Why is freezing point depression of 0.1 M sodium chloride solution nearly twice that of 0.1 M Glucose solution?

A 5% solution (by mass) of canesugar in water has freezing point of 271K. Calculate the freezing point of a 5% glucose in water if freezing point of pure water is 273.15K.

A 0.1539 molal aqueous solution of canesugar (molar mass = 342g mol^-1) has a freezing point 271K. While the freezing point of pure water is 273.15k. What will be the freezing point of an aqueous solution, containing 5g of glucose (Mol mass = 180g mol^-1) per 100g of solution?

100 mg of a protein is dissolved in just enough water to make 10.0 mL of solution. If this solution has an osmotic pressure of 13.3mm Hg at 25^@C , what is the molar mass of the protein? (R = 0.0821L atm mol^-1 K^-1 and 760mm Hg = 1atm)

Calculate the freezing point of an aqueous solution containing 10.50g of MgBr_2 = 184g, K_f for water = 1.86 K kg mol^-1 .