25mLof decimolar solution of a stable divalent transition metal cation is oxidised by 50mL of 0.02M acidified permanganate solution. What is the final oxidation state of the metal?

25mLof decimolar solution of a stable divalent transition metal cation

1.	25mLof decimolar solution of a stable divalent transition metal cation is oxidised by 50mL of 0.02M acidified permanganate solution. What is the final oxidation state of the metal?
Answer» <html><body><p></p>Solution :<a href="https://interviewquestions.tuteehub.com/tag/5-319454" style="font-weight:bold;" target="_blank" title="Click to know more about 5">5</a> moles of `M^(<a href="https://interviewquestions.tuteehub.com/tag/2-283658" style="font-weight:bold;" target="_blank" title="Click to know more about 2">2</a>+)` ion =x moles of permanganate , where x is the increase in oxidation number of the metal ion, `M^(2+)` <br/> Using the <a href="https://interviewquestions.tuteehub.com/tag/molarity-1100268" style="font-weight:bold;" target="_blank" title="Click to know more about MOLARITY">MOLARITY</a> <a href="https://interviewquestions.tuteehub.com/tag/equation-974081" style="font-weight:bold;" target="_blank" title="Click to know more about EQUATION">EQUATION</a> for the <a href="https://interviewquestions.tuteehub.com/tag/titration-710389" style="font-weight:bold;" target="_blank" title="Click to know more about TITRATION">TITRATION</a> <br/> `(V_(1)M_(1))/(5)=(V_(2)M_(2))/(x)` <br/> The final oxidation state of metal `=+2-(-2)=+4`</body></html>