TS EAMCET · Chemistry · Some Basic Concepts of Chemistry
The formula of a metal oxide is \(\mathrm{M}_{0.96} \mathrm{O}_1\). The fractions of metal that exists as \(\mathrm{M}^{3+}\) and \(\mathrm{M}^{2+}\) ions in that oxide are respectively
- A \(0.083,0.916\)
- B \(0.916,0.083\)
- C \(0.88,0.12\)
- D \(0.12,0.88\)
Answer & Solution
Correct Answer
(A) \(0.083,0.916\)
Step-by-step Solution
Detailed explanation
Let \(\mathrm{x}=\) number of \(\mathrm{M}^{3+}\) ions \(\mathrm{y}=\) number of \(\mathrm{M}^{2+}\) ions Impure sample has \(\mathrm{M}^{3+}\) ions. replacing \(\mathrm{M}^{2+}\) ions. \[ \Rightarrow \mathrm{y}=0.96-\mathrm{x} \] Total charge of metal atoms \(=\) total charge…
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