A sample of a metal oxide has formula $\mathrm{M}_{0.83} \mathrm{O}_{1.00}$. The metal $\mathrm{M}$ can exist in two oxidation states $+2$ and $+3$.
In the sample of $\mathrm{M}_{0.83} \mathrm{O}_{1.00}$, the percentage of metal ions existing in $+2$ oxidation state is __________ $\%$. (nearest integer)
Answer (integer)
59
Solution
Let, metal $\mathrm{M}$ present x and (0.83 - x) in oxidation states $+2$ and $+3$ respectively.
<br/><br/>$$
\begin{aligned}
& 2 x+3(0.83-x)=2 \\\\
& x=0.49 \\\\
& \% M^{2+}=\frac{0.49}{0.83} \times 100 \\\\
& =59 \%
\end{aligned}
$$
About this question
Subject: Chemistry · Chapter: Some Basic Concepts of Chemistry · Topic: Mole Concept
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