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Question

Calculate the equivalent mass of $${H}_{2}{SO}_{4}$$ from the given reactions.
$$(a)\ {H}_{2}{SO}_{4}+NaOH\rightarrow NaH{SO}_{4}+{H}_{2}O$$
$$(b)\ {H}_{2}{SO}_{4}+2NaOH\rightarrow {Na}_{2}{SO}_{4}+2{H}_{2}O$$


A
49 and 98
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B
98 and 49
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C
Both 49
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D
Both 98
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Solution

The correct option is A $$98$$ and $$49$$
$$(a) {H}_{2}{SO}_{4}+NaOH\rightarrow NaH{SO}_{4}+{H}_{2}O$$

Number of equivalent moles in the reaction = $$1$$ as only 1 $$H^+$$ is involved.

$$Equivalent\ weight= \dfrac {Molecular \ weight}{Number\ of\ equivalent \ moles}$$

$$\Rightarrow Equivalent \ weight= \dfrac {98}{1} = 98$$

$$(b) {H}_{2}{SO}_{4}+2NaOH\rightarrow {Na}_{2}{SO}_{4}+2{H}_{2}O$$

Number of equivalent moles in the reaction = $$2$$ as both $$H^+$$ are reacting with base.

$$\Rightarrow Equivalent \ weight= \dfrac {98}{2} = 49$$

Chemistry

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