# Identify Acid using Stoic

Lori

## Homework Statement

8.040 grams of a strong, monoprotic acid was added to enough water to make 500 ml of solution and used o completely neutralize 2.080 g aluminum hydroixide. identify the acid.

m1v1 = m2v2
M = n/1 Liter

## The Attempt at a Solution

i know that 2.08 g of Aluminum hydroxide is 0.02667 mols using molar mass of Aluminum hydroxide.
I also might know that there is 491.96 grams of water since i took the % from 8.040 grams/500 ml. Not sure if this is correct. I'm kinda stuck from here on.

I somewhat got a chemical equation going on with HX + Al(OH)3 --> H2O + AlX

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mjc123
Homework Helper
What do you think would be the stoichiometry of the HX - Al(OH)3 reaction?

Lori
You mean the mole conversions? I think X would have 3 mols right because Al has a +3 charge

Borek
Mentor
m1v1 = m2v2
See my comment in your second titration thread. Forget you ever saw this formula.

Lori
See my comment in your second titration thread. Forget you ever saw this formula.
I'm aware that this formula won't work with this problem but I'm still stuck

Borek
Mentor
Balance the reaction correctly and use the masses given to calculate molar mass of HX.

Lori
Ok. I got 100 grams/lol of HX using 3 moles HX/1mol al (oh)2

So Since it says strong acid, I just have to match it to the molar mass of the list of strong acids I know right? It would be HCLO4 since it also as like 100g/mol

Borek
Mentor
Looks reasonable.