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Question

342g of 20% (by mass) of Ba(OH)2 solution (specific gravity = 0.57) reacts with 1200 mL of 2 M HNO3. If the resulting density is the same as pure water, then the molarity of the hydronium ions in the resulting solution is:

A
0.25 M
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B
0.5 M
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C
0.888 M
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D
None of these
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Solution

The correct option is C 0.888 M
The number of moles of Ba(OH)2=20×342100×171=0.4
Moles of OH ions=0.4×2=0.8
The number of moles of HNO3=1.2×2=2.4
Hence, the final solution is acidic due to the presence of excess H+
H+=(2.40.8)×10001200+3420.57=0.888M

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