`20`g of a binary electrolyte(mol.wt.=`100`)are dissolved in `500`g of water.The freezing point of the solution is `-0.74^(@)CK_(f)=1.86K "molality"^(-1)`.the degree of ionization of the electrolyte is

20 g of a binary electrolyte (mol. Wt. = 100) are dissolved in 500 g of water. The freezing point of the solution is -0.74^@C , K = 1.86 k molality^-1. The degree of ionization of the electrolyte is:

20 g of a biaryelectrolyte (Molecular mass =100) are dissolved in 500 g of water. The freezing point of the solution is -0.74^(@)C and K_(f)=1.86 K kg mol^(-1) . The degree of ionisation of eletrolyte as :

3g urea is dissolved in 100ml water. Find the freezing point of solution ( K_f = 1.86k kg mol_(-1) )

2g of a non-electrolyte solute dissolved in 100g of benzene lowered the freezing point of benzene by 0.40 K. find the molar mass of the solute.

If 10.0 g of a non-electrolyte dissolved in 100 g of water lowers the freezing point of water by 1.86^(@)C , the molar mass of the non-electrolyte is ( K_(f)=1.86 Km^(-1) )

The freezing point of a 0.05 molal solution of a non-electrolyte in water is: ( K_(f) = 1.86 "molality"^(-1) )

The freezing point of a 0.05 molal solution of a non-electrolyte in water is: ( K_(f) = 1.86 "molality"^(-1) )