The concentration of `CoCl_(3)xNH_(3)` in aqueous solution is `0.2m`. `K_(f)` of water is `1.86Kkgmol^(-1)`, its `DeltaT_(f)` is `0.744K`. If it undergoes complete ionization in aqueous solution its correct formula is:

Mole fraction of a non-electrolyte in aqueous solution is 0.07 . If K_(f) is 1.86^(@) "mol"^(-1)kg , depression if f.p.,DeltaT_(f), is:

0.5 molal aqueous solution of a weak acid (HX) is 20% ionised. If K_(f) for water is 1.86K kg mol^(-1) , the lowering in freezing point of the solution is

An aqueous solution freezes on 0.36^@C K_f and K_b for water are 1.8 and 0.52 k kg mol^-1 respectively then value of boiling point of solution as 1 atm pressure is

A 0.1 molal aqueous solution of a weak acid is 30% ionized. If K_(f) for water is 1.86^(@)C//m , the freezing point of the solution will be.

Complete the following statements by selecting the correct alternative from the choices given : An aqueous solution of urea freezes at - 0.186^(@)C, K_(f) for water = 1.86 K kg. mol^(-1),K_(b) for water = 0.512 "K kg mol"^(-1) . The boiling point of urea solution will be :

The lowering in freezing point of 0.75 molal aqueous solution NaCI (80% dissociated) is [Given, K_f, for water 1.86 K kg mol^(-1)]

A complex is represented as CoCl_(3)Xnh_(3) . Its 0.1 molal solution in water DeltaT_(f)=0.588 K. K_(f) for H_(2)O is 1.86K" molality"^(-1) . Assuming 100% ionisation of complex and co - ordination number of Co is six calculate formula of complex.

Elevation in boiling point of an aqueous solution of urea is 0.52 ( k_(b) "for water"=0.52K"molality"^(-1)) . The mole fraction of urea in this solution is :

A complex is represented as CoCl_(3) . XNH_(3) . Its 0.1 molal solution in aqueous solution shows Delta T_(f) = 0.558^(circ). (K_(f) for H_(2)O is 1.86 K "molality"^(-1)) Assuming 100% ionisation of complex and co-ordination number of Co as six, calculate formula of complex.

The hydrolysis constant of 0.1M aqueous solution of sodium acetate if K_(a) of CH_(3)COOH = 1.8 xx 10^(-5) is