Home
Class 12
CHEMISTRY
2.1 g of non-electrolyte solute (molar m...

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 solution if freezing point of pure benzene is 5.5^0 C.

Promotional Banner

Topper's Solved these Questions

  • MODEL TEST PAPER-10

    ACCURATE PUBLICATION|Exercise SECTION-C (LONG ANSWER QUESTIONS)|8 Videos

  • MODEL TEST PAPER-10

    ACCURATE PUBLICATION|Exercise SECTION-D (LONG ANSWER QUESTIONS) (TYPE II)|15 Videos

  • MODEL TEST PAPER-10

    ACCURATE PUBLICATION|Exercise SECTION-A (True/False )|5 Videos

  • MODEL TEST PAPER-1

    ACCURATE PUBLICATION|Exercise SECTION-D (LONG ANSWER QUESTIONS) (TYPE II)|11 Videos

  • MODEL TEST PAPER-2

    ACCURATE PUBLICATION|Exercise SECTION-D (LONG ANSWER QUESTIONS) (TYPE II)|14 Videos

Similar Questions

Explore conceptually related problems

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

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.

A 5% solution (by mass) of cane sugar in water has freezing point of 27IK Calculate the freezing point of 5% glucose in water if freezing point of pure water is 273.15 K.

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?

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.

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.

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 )