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Ideal Gas Equation

Upon mixing e...

Question

Upon mixing equal volumes of aqueous solutions of 0.1 M HCl and 0.2 M $H_{2} S O_{4}$ , the concentration of $H^{+}$ in the resulting solution is:

0.30 mol/L

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0.25 mol/L

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0.15 mol/L

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0.10 mol/L

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Solution

The correct option is B 0.25 mol/L
Assume that 0.5 L each of aqueous solutions of 0.1 M $H C l$ and 0.2 M $H_{2} S O_{4}$ are mixed.
0.5 L of 0.1 M $H C l$ will give $0.5 L \times 0.1 m o l / L = 0.05 m o l$ of $H^{+}$ ions.
Each molecule of $H_{2} S O_{4}$ produce 2 $H^{+}$ ion.

0.5 L of 0.2 M $H_{2} S O_{4}$ will give $0.5 L \times 0.2 m o l / L \times 2 = 0.2 m o l$ of $H^{+}$ ions.
Total number of moles of $H^{+}$ ions $= 0.05 + 0.2 = 0.25$ moles.
Total volume $= 0.5 + 0.5 = 1.0 L$
$[H^{+}] = \frac{0.25 m o l}{1.0 L} = 0.25 m o l / L$

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Upon mixing equal volumes of aqueous solutions of 0.1 M HCl and 0.2 M H2SO4 , the concentration of H+ in the resulting solution is:

Upon mixing equal volumes of aqueous solutions of 0.1 M HCl and 0.2 M $H_{2} S O_{4}$ , the concentration of $H^{+}$ in the resulting solution is: