Use stoichiometry to determine the mols of HCl needed.
Probably the easiest thing to do next is to determine the molarity of the commerical HCl.
M = mols/L.
density = 1.18 g/mL; therefore,
mass of 1000 mL = 1.18 g/mL x 1000 mL = 1180 grams.
How much of that is HCl.
1180 g x 0.37 = 436.6 grams HCl.
How many mols. 436.6/36.46 = 11.97 so HCl is 11.97 Molar.
mols needed to dissolve Al = M x L
You know mols needed. You know M. Solve for Liters
Post your work if you needed additional help.
Commerical hydrochloric acid is 37% by mass HCl and has a solution density of 1.18g/mL. What minimum volume of hydrocloric acid is needed to dissolve 16g Al. The balanced equation is
2Al + 6Hcl --> 2AlCl3 + 3H2
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