The boiling point of water in a  0.1 molal silver nitrate solution (solution A) is $\mathrm{x}°\mathrm{C}$.  To this solution  A ,  an equal volume of  0.1  molal aqueous barium chloride solution is added to make a  new solution B. The difference in the boiling points of water in the two solutions A  and B  is $\mathrm{y}\times {10}^{-2}°\mathrm{C}$ (Assume densities of the solutions A and B  are the same as that of water and  the soluble salts dissociate completely) 
Use:  Molal elevation constat ( Ebullioscopic constant)  
${\mathrm{K}}_{\mathrm{b}}=0.5\mathrm{K}\mathrm{kg}{\mathrm{mol}}^{-1},\mathrm{Boiling}\mathrm{point}\mathrm{of}\mathrm{pure}\mathrm{water}\mathrm{as}{100}^0\mathrm{C})$