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1.520 g of hydroxide of a metal on ignition gave 0.995 g of oxide

1.520 g of hydroxide of a metal on ignition gave 0.995 g of oxide. The equivalent weight of metal is

Options

(a) 1.52
(b) 0.995
(c) 190
(d) 9

Correct Answer:

9

Explanation:

One equivalent of the metal reacts with one mole of hydroxide, i.e., 17g

Similarly, one equivalent of the metal reacts with 1/2 mole oxygen atoms, i.e., 8g of oxygen atoms.

Let E be the equivalent mass of the metal. And let x be the number of equivalents of metal hydroxide ignited.

Therefore,

x(E+17) = 1.520g and

x(E+8) = 0.995
Eliminating x, we get E=9.06g.

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