The boiling point of water in a 0.1 molal silver nitrate solution (solution A ) is x ^ 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 10⁻² ^ C . (Assume: Densities of the solutions A and B are the same as that of water and the soluble salts dissociate completely. U

Step-by-step solution

After adding BaCl 2 solution in AgNO 3 solution AgCl will be precipitate. Since volume of both solutions are equal let's take V = 1   L of each. so initial moles of AgNO 3 = 0 .1   mole initial moles of BaCl 2 = 0 .1   mole 2   AgNO 3 + BaCl 2 → 2 AgCl ↓ + Ba NO 3 2 2 AgNO 3 + BaCl 2 → 2 AgCl ↓ + Ba NO 3 2 Intial   moles 0 .1 0 .1 Change 0 .1 − 0 .05 + 0 .1 + 0 .05 Final   moles 0 0 .05 0 .05 Final   concentration 0 .05 2 0 .05 2 New ΔT b = 1