The boiling point of water in a \( 0.1 \) molal silver nitrate solution (solution A) is \( x^\circ \, \text{C} \). 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 \( y \times 10^{-2} \, ^\circ \text{C} \).
(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 \( 100^\circ \text{C} \).)
The value of \( |y| \) is ______.
