Redox and Equivalent ConceptMedium
Question
A volume of 12.5 ml of 0.05 M selenium dioxide, SeO2, reacted with exactly 25.0 ml of 0.1 M – CrSO4. In this reaction, Cr2+ is converted to Cr3+. To what oxidation state the selenium is converted by the reaction?
Options
A.0
B.+1
C.+2
D.+4
Solution
$n_{eq}SeO_{2} = n_{eq}Cr^{2 +}$
$\text{Or }\frac{12.5 \times 0.05}{1000} \times (4 - x) = \frac{25 \times 0.1}{1000} \times 1 \Rightarrow x = 0$
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