Home
Class 12
CHEMISTRY
Define (i) Mole fraction (ii) Molali...

Define
(i) Mole fraction
(ii) Molality
(iii) Raoult's law
(b) Assuming complete dissociation, calculate the expected freezing point of a solution prepared by dissolving 6.00 g of Glauber's salt, `Na_(2)SO_(4).10 H_(2)O` in 0.100 kg of water. (`K_(f)` for water =`1.86 K kg "mol"^(-1)`, Atomic massess : Na=23, S=32, O=16 , H=1)

Promotional Banner

Similar Questions

Explore conceptually related problems

Assming complete dissociation, Calculate the expected the expected freezing point of a solution prepared by dissolving 6.0 g of Glauber's salt. Na_(2)SO_(4). 10H_(2)O in 0.1 kg of water. (Given value of K_(f)=1.86 K kg mol^(-1)) .

Assuming complete dissociation, calculate the expected freezing point of a solution prepared by dissolving 6g of Na_2SO_4 .10H_2O~ in 0.1 kg of water ( k_f for water= 1.86)

What will be the freezing point ("in"^(@)C) of solution obtained by dissolving 0.1 g potassium ferricyanide (mol wt = 329) in 100 g water. If K_(f) for water is 1.86 K kg mol^(-1)

A solution of sucrose (mol.mass=342) was prepared by dissolving 34.2g of it in 1000g water. Find its freezing point. (K_f for water = 1.86k kg mol^(-1) )

Calculate the freezing point of a solution when 3 g of CaCI_(2) (M=111 g mol^(-1)) was dissolved in 100g of water assuming that CaCI_(2) undergoes complete ionisation (K_(f) "for water"=1.86 K kg mol^(-1)) .

Calculate the temperature at which a solution containing 54g of glucose, (C_(6)H_(12)O_(6)) in 250g of water will freeze. ( K_(f) for water = 1.86 K mol^(-1) kg)

Calculate the temperature at which a solution containing 54g of glucose, (C_(6)H_(12)O_(6)) in 250g of water will freeze. ( K_(f) for water = 1.86 K mol^(-1) kg)

Calculate the temperature at which a solution containing 54 g of glucose (C_(6)H_(12)O_(6)) in 250 g of water will freeze. ( K_(f) for water = 1.86 K mol^-1 kg).