Asked by Anonymous
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
2Al + 6Hcl --> 2AlCl3 + 3H2
Answers
Answered by
DrBob222
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.
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.
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