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Byju's Answer

Standard XII

Chemistry

Balancing Redox Equations

1 g of H2O2...

Question

$1$ g of $H_{2} O_{2}$ solution containing $x %$ of $H_{2} O_{2}$ by mass requires $x$ mL of $K M n O_{4}$ for complete oxidation in acid medium. Calculate the normality of $K M n O_{4}$ solution. (write the value to the nearest integer)

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Solution

The redox changes are as follows:
$M n^{7 +} + 5 e ⟶ M n^{2 +}$
$(O^{-})_{2} ⟶ O_{2} + 2 e$

Meq. of $K M n O_{4} =$ Meq. of $H_{2} O_{2}$

Normality $\times x = \frac{Mass of H_{2} O_{2}}{Equivalent mass} \times 1000$ $= \frac{x}{100 \times \frac{34}{2}} \times 1000$
Normality of $K M n O_{4} = 0.588 N$

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Q. A

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1 g of H2O2 solution containing x% of H2O2 by mass requires x mL of KMnO4 for complete oxidation in acid medium. Calculate the normality of KMnO4 solution. (write the value to the nearest integer)

The redox changes are as follows:Mn7++5e⟶Mn2+(O−)2⟶O2+2eMeq. of KMnO4= Meq. of H2O2Normality × x=Mass of H2O2Equivalent mass×1000 =x100×342×1000Normality of KMnO4=0.588N

$1$ g of $H_{2} O_{2}$ solution containing $x %$ of $H_{2} O_{2}$ by mass requires $x$ mL of $K M n O_{4}$ for complete oxidation in acid medium. Calculate the normality of $K M n O_{4}$ solution. (write the value to the nearest integer)