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A piece of Al weighing 27 g is reacted with 200 ml of $H_{2} {SO}_{4}$ (specific gravity = 1.8 and 54.5% by weight). After the metal is completely dissolved, 73 gm $HCl$ is added and solution is further diluted to 500 ml solution then find the concentration of $H^{+}$ ion in mol/litre.

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answer is 6.

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Detailed Solution

$2 Al + 3 H_{2} {SO}_{4} \to {Al}_{2} {({SO}_{4})}_{3} + 3 H_{2} O$

$1 mole [200 \times \frac{1.8}{98} \times \frac{64.5}{100}]$

$= 2 moles 2 - \frac{3}{2} = 0.5 moles$

$[H^{+}] = \frac{0.5 \times 2 + \frac{73}{36.5}}{0.5} = 6$ .

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