# Chemistry: dissolving aluminum metal in hydrochloric acid

## Homework Statement

Aluminum metal dissolves in hydrochloric acid. What volume, in mL, of 1.58 M HCl is needed to completely dissolve 3.200 g of aluminum?(Hint: write the single-replacement reaction first)

## Homework Equations

VM=VM

## The Attempt at a Solution

I got the single-replacement reaction:
2Al(s) + 6HCl(aq) = 2AlCl(aq) + 3H(g)
But from there, I'm not really sure what to do. I think stoichiometry's involved, but I'm not sure how to use it.

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BvU
Homework Helper
2019 Award
If you have
2Al(s) + 6HCl(aq) = 2AlCl(aq) + 3H(g)
you have the stoechiometry ! My guess is that it's time to convert mol(ecul)es to mass Borek
Mentor
My guess is that it's time to convert mol(ecul)es to mass
I would rather convert mass to moles BvU
Homework Helper
2019 Award
Sure, and perhaps you can explain to the audience why this is a better idea (generally or in this sspecific case) ?

symbolipoint
Homework Helper
Gold Member
Stepwise path to find the volume of HCl,

Find moles of Aluminum (need formula weight of Aluminum)
Find moles of HCl (use ratio according to reaction)
Find volume of HCl solution of 1.58 M (concentration computation)

Am I correct in remembering that you may need to add a near-catalytic amount of copper chloride to accelerate breakdown of surface passivation ?

symbolipoint
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