Find out molarity of $H^{+}$ ions in $2$ M, $500$ ml of $H_{2} S O_{4}$ solution.

4 M

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2 M

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1 M

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8 M

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Solution

The correct option is B 4 M
$H_{2} S O_{4} ⇌ 2 H^{+} + S O_{4}^{-}$

$1$ $:$ $2$

$500 m L$ of $2 M$ solution contains $1 M H_{2} S O_{4}$ molecules. We see from dissociation reaction that $H_{2} S O_{4} : H^{+}$ ratio is $1 : 2$

Therefore, $2 m o l e s H^{+}$ ions are present in $500 m L$ solution.

$500 m L s o l u t i o n \to 2 m o l e s H^{+} i o n s$

$1000 m L s o l u t i o n \to 4 m o l e s H^{+} i o n s$

$∴$ Molarity of $H^{+}$ ions is $4 M$

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