Question

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

• A. $1.520$
• B. $0.995$
• C. $19.00$
• D. $9.00$

Answer 1

The correct option is D $9.00$

Since the hydroxide and oxide are involved in the same reaction, the ratio of their molecular weight is equal to the ratio of their equivalent weight.

$\frac{weightofmetalhydroxide}{weightofmetallicoxide}=\frac{eqmassofmetal+eqmassofO{H}^{-}}{eqmassofmetal+eqmassof{O}^{2-}}$

Therefore, $\frac{1.520}{0.995}$ $=$ $\frac{x+17}{x+8}$.

On solving, we get $x$ $=$ $9.0$