A mixture contains NaCl and unknown chloride, MCl. When 1 g of this mixture is dissolved in water an

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A mixture contains NaCl and unknown chloride, MCl. When 1 g of this mixture is dissolved in water and excess of AgNO3 solution is added to it, 2.567 g of white precipitate is obtained. In another experiment, 1 g of the same original mixture is heated to 300oC. Some vapours come out which are absorbed in acidified AgNO3 solution by which 1.341 g of white precipitate is formed. The molecular mass of unknown chloride is

Accepted Answer

NaCl → AgCl and MCl → AgClx mole x mole y mole y mole∴ (x + y) × 143.5 = 2.567 (1)From the second expression:MCl → AgCly mole y mole∴ y × 143.5 = 1.341 (2)Hence, x =$\frac{1.226}{143.5}$ , y =$\frac{1.341}{143.5}$Now, x × 58.5 + y × M = 1 ⇒ M = 53.5

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