The boiling point of water in a \( 0.1 \) molal silver nitrate solution (solution \( A \)) is \( x^\circ \mathrm{C} \). 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 \( y \times 10^{-2} \, ^\circ \mathrm{C} \). (Assume: Densities of the solutions \( A \) and \( B \) are the same as that of water and the soluble salts dissociate completely. Use: Molal elevation constant (Ebullioscopic Constant), \( K_b = 0.5 \, \text{K kg mol}^{-1} \); Boiling point of pure water as \( 100^\circ \mathrm{C} \).)
The value of \( x \) is ______.
