A solution of urea (Molar mass`=60gmol^(-1)`) has been prepared by dissolving `6g` of urea in `500g` of water. The depression in freezing point of the solution obtained will be
(`K_(f)` for water`=1.86K.kg.mol^(-1)`)

A solution of sucrose (molar mass =342 g mol^(-1) ) has been prepared by dissolving 68.5 g of sucrose in 1000 g of water. The depression in freezing point of the solution obtained will be ( K_(f) for water = 1.86K kg mol^(-1) )

A solution of sucrose (molar mass =342) is prepared by dissolving 68.4 g in 1000 g of water. Calculate The freezing point of solution.

45 g of ethylene glycol (C_(2) H_(6)O_(2)) is mixed with 600 g of water. The freezing point of the solution is (K_(f) for water is 1.86 K kg mol^(-1) )

If 0.1 m aqueous solution of calcium phosphate is 80% dissociated then the freezing point of the solution will be (K_f of water = 1.86K kg mol^(-1))

0.1 mole of sugar is dissolved in 250 g of water. The freezing point of the solution is [K_(f) "for" H_(2)O = 1.86^(@)C "molal"^(-1)]

6 g of a substance is dissolved in 100 g of water depresses the freezing point by 0.93^(@)C . The molecular mass of the substance will be: ( K_(f) for water = 1.86^(@)C /molal)

In a 0.5 molal solution KCl, KCl is 50% dissociated. The freezing point of solution will be ( K_(f) = 1.86 K kg mol^(-1) ):

What mass of ethlene ethyelne glycol ("molar mass"=62 g mol^(-1)) must be dissolved in 5.5kg of water to lower the freezing point of from 0^(@)C to-10^(@)C ? (K_(f)) for water=1.86 K kg mol^(-1) ).

What mass of NaCl ("molar mass" =58.5g mol^(-1)) 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 van't Hoff factor for NaCl is 1.87 .