1 g of non - electrolyte solute (molar m...

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

0.3 K

0.5K

0.2 K

0.4 K

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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.

1.00g of a non-electrolyte solute dissolved in 50g of benzene lowered the freezing point of benzene by 0.40K. The freezing point depression constant of benzene is 5.12K mol^-1 . Find the molar mass of the solute.

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)

2g of benzoic acid ( C_6H_5COOH ) is dissolved in 25g of benzene show depression in freezing point equal to 1.62K. Molar depression constant for benzene, K_f =4.9K kg mol^-1 . What is percentage association of acid if it forms a dimer in solution?

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 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%.

10g of non-volatile solute when dissolved in 100g of benzene raises its boiling point by 1^@ C. What is the molecular mass of the solute. ( k_b for benzene=2.53 K kg mol^-1 )

If 30 g a solute of molecular mass 154 is dissolved in 250 g of benzene. What will be the elevation in boiling point of the resuling solution ? (Given : K_B(C_(6)H_(6)) =2.6 K kg mol^(-1) )

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