# What is the molarity of hydrochloric acid in a solution that contains a 3.65*g mass of HCl(g) in 500*mL aqueous solution?

May 9, 2017

$\text{Molarity"-="Moles of solute"/"Volume of solution}$

#### Explanation:

And here, $\text{molarity} = \frac{\frac{3.65 \cdot g}{36.5 \cdot g \cdot m o {l}^{-} 1}}{500 \cdot m L \times {10}^{-} 3 \cdot L \cdot m {L}^{-} 1} = 0.200 \cdot m o l \cdot {L}^{-} 1$.

Is the calculation consistent dimensionally?

And thus if it is $0.200 \cdot m o l \cdot {L}^{-} 1$ with respect to hydrogen chloride, it is $0.200 \cdot m o l \cdot {L}^{-} 1$ with respect to ${H}_{3} {O}^{+}$, AND $C {l}^{-}$.

What is the $p H$ of this solution?