Proving that an oxide is acidic?

Question

I realize that the compound As2O3 is an acidic oxide, but I am not quite sure what sort of balanced equation to use to prove its acidity. I am planning on using As2O3 + H2O, but I can't remember how to figure out exactly what this yields. I assumed that it was H3AsO4, but I couldn't balance the equation with this, so it seems as though it might yield H3AsO3. I should know how to formulate my balanced equation properly, but apparently I have forgotten what steps to take.

Am I using the right reactants? If so, what should my product be?

Thanks for your help. =)

Answer 1

Arsenic (III) oxide and water are the correct reactants. They will form Arsenious acid (H3AsO3):

As2O3 + 3 H2O --> 2 H3AsO3

The proof of acidity is:

H3AsO3 --> H+ + (H2AsO3)-

This shows the possibility of donating a proton.

Answer 2

An arsenious acid solution is prepared with one gram As2O3 , 5 ml dilute hydrochloric acid HCl and enough water to make up to 100 ml. It has been used in skin and blood disorders. It is poisonous, and should be used with care.
Arsenic acid(a.k.a orthoarsenic acid),has the formula AsH3O4 with a molecular weight of 141.94
It is prepared from As2O3 and HNO3. See Simon, Thaler Z. Anorg. Allgem. Chem. 161, 143, 1927: and same journal 246, 19, (1941).
Hope that helps.
Dan.

Answer 3

Yes, you are using the right reactants. Acidic anhydrides produce acids in water. Unfortunately, that's all I know. :P

Answer 4

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