Question:
1.520 g of hydroxide of a metal on ignition gave 0.995 g of oxide . The equivalent weight of the metal
Answer:
One equivalent of the metal reacts with one mole of OH-, 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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