A 1.00 molal aqueous Solution of trichloroacetic acid `(C Cl_(3)COOH)` is heated to its boiling point. The solution has the boiling point of 100.18°C. Determine the van't Hoff factor for trichloroacetic acid.
`K_b`= 0.512 K kg/mol

A 0.2 molal aqueous solution of a weak acid (HX) is 20 percent ionised. The freezing point of this solution is: ( K_f = 1.86 K/m for water)

A solution of urea in water has a boiling point of 100.128^@ C. calculate its freezing point (K_b=0.512 and K_f = 1.86K kg mol_(-1) )

An aqueous solution freezes at -0.186^@C (K_f= 1.86^@: K_b=0.512^@) . What is the elevation in boiling point:

The boiling point of an aqueous solution of a nonvolatile solute is 100.15^@C. What is the freezing point of an aqueous solution obtained by diluting the above solution with an equal volume of water? The value of K_b and K_f for water are 0.512^@C and 1.86^@C K molality^-1: