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A 12.0 M acid solution that contains 75.0 % acid by mass has a density of 1.57 g/mL. What is the identity of the acid?

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HCl (M = 36.5)

HBr (M=80.9)

CH₃CO₂H (M = 60.0

H₃PO₄(M = 98.0)

answer is D.

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Detailed Solution

$12 \times M = \frac{75}{100} \times 1.57 \times 1000$

$\Rightarrow M = 98.125$

$H_{3} {PO}_{4}$

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