Question

$1.520\text{g}$ of a hydroxide of a metal on ignition gave $0.995\text{g}$ of an oxide of the same metal. The equivalent weight of the metal is _______.

• A. $0.995\text{g}$
• B. $19.0\text{g}$
• C. $1.90\text{g}$
• D. $9.00\text{g}$

Answer 1

The correct option is D $9.00\text{g}$

Mass of the hydroxide = $1.520\text{g}$; mass of the oxide = $0.995\text{g}$
$\frac{\text{weight of the metal hydroxide}}{\text{weight of the metal oxide}}=\frac{\text{equivalent weight of the metal hydroxide}}{\text{equivalent weight of the metal oxide}}$
$\Rightarrow \frac{1.520}{0.995}=\frac{M+17}{M+8}$
On solving, $M=9\text{g}$