Question

How many milliliters of a 1.25 molar hydrochloric acid (HCl) solution would be needed to react completely with 60.0 grams of calcium metal? (2 points)
Ca (s) + 2HCl (aq)yields CaCl2 (aq) + H2 (g)

Answer 1

Answer:

2400 mL

Explanation:

$Ca + 2HCl \implies CaCl_2 + H_2$

According to this equation, the stoichiometric ratio between $Ca$ and $HCl$ for the complete reaction is 1:2.

We know that the number of moles of $Ca$ can be calculated using the mole formula. (number of moles = mass / molar mass)

Moles of Calcium = $\frac{60}{40}$ = 1.5 mol

So the moles of $HCl$ = $1.5 \times 2$ = 3.0 mol

Volume of HCl solution = Moles of HCl/ concentration of HCl

Volume of HCl solution = $\frac{3}{1.25}$ = 2400 mL