# If 2.0 mL of 6.0M HCl is used to make a 500.0-mL aqueous solution, what is the molarity?

May 16, 2017

$\text{Molarity"="Moles of solute"/"Volume of solution} = 0.024 \cdot m o l \cdot {L}^{-} 1$

#### Explanation:

And thus..........$\frac{6.0 \cdot m o l \cdot {L}^{-} 1 \times 2.0 \times {10}^{-} 3 \cdot L}{0.500 \cdot L}$

$= 0.024 \cdot m o l \cdot {L}^{-} 1$.

What is $p H$ of this solution?

I forgot to remind you that the order of addition is important. While it is not crucial here, you ALWAYS add ACID to water, and never the reverse! Why? See here..........