A solution of ,urea In water boils at` 100.18 ^@C`.‘Calculate the freezing point of the same solution. Molar constants `K_f` and `K_b` are 1.86 and `0.512 km^-1` respectively.

A solution of ,urea In water boils at 100.18 ^@C .‘Calculate the freezing point of the same solution. Molar constants K_t and K_b are 1.86 and 0.512 km^-1 respectively. How-will you differentiate between molar elevation constant and molar depression constant ?

Molal depression constant for water is 1.86^@C . What is freezing point of a 0.05 molal solution of a non electrolyte in water?

0.2 molal aqueous solution of acid HX is 20% ionised. K_f="1.86 K molal"^(-1) . The freezing point of the solution is very close to:

A 5% solution (by mass) of cane sugar (C_12 H_22 O_11) in water has a freezing point of 271 K. Calculate the freezing point of 5%. (by mass) solution of glucose (C_6 H_12 O_6) In water. Freezingpoint of pure water is 273.15 K.

A 0.10 M aqueous solution of a monoprotic acid ("d=1.01 g/cm"^3) is 5% ionized. What is the freezing point of the solution? The mol.wt. of the acid is 300 and K_f (H_(2)O)="1.86"^@C//m:

5 %' solution (by mass) of cane sugar in water has freezing point of '271 K .' Calculate the freezing point of '5 %' glucơse in water if freezing point of pure water is 273.15

What mass of NaCl ("molar mass =58.5 g mol"^(-1)) dissolved in 50g of water will lower the freezing point by 5^@C? The freezing point depression constant, K_p for water is 1.86" K kg mol"^(-1) , van't Hoff factor for NaCl is 1.87.

Calculate the pH of a 0.2M solution of hydrocyanic acid (HCN). Ionisation constant (K_a) of HCN at 298K is 7.2xx10^(-10)

An aqueous solution of glucose containing 12 g in 100g of water was found to boil at 100.34^@C. Calculate K_b for water in K mol ""^(-1) kg.