# To react with a 5.00*g mass of calcium hydroxide, what volume of 0.100*mol*L^-1 HCl is required?

Oct 3, 2016

Approx. $1.4 \cdot L$ hydrochloric acid are required.

#### Explanation:

We need (i) a chemical reaction:

$C a {\left(O H\right)}_{2} \left(s\right) + 2 H C l \left(a q\right) \rightarrow C a C {l}_{2} \left(a q\right) + 2 {H}_{2} O \left(l\right)$*

And (ii), the molar quantity of calcium hydroxide:

$=$ $\frac{5.00 \cdot g}{74.09 \cdot g \cdot m o {l}^{-} 1}$ $=$ $0.0675 \cdot m o l$.

Given the rxn stoichiometry, clearly, we need $2 \times 0.0675 \cdot m o l = 0.135 \cdot m o l$ $H C l \left(a q\right)$.

And given our concentration of $H C l$, $\frac{0.135 \cdot m o l}{0.100 \cdot m o l \cdot {L}^{-} 1} \times {10}^{3} \cdot m L \cdot {L}^{-} 1$ $=$ ??mL