# Problem: Arsenic acid (H3AsO4) is a triprotic acid with K a1 = 5.5 X 10 -3, Ka2 = 1.7 X 10 -7, and Ka3 = 5.1 X 10-12. Calculate [H+], [OH-], [H3AsO4], [H2AsO4-], [HAsO42-], and [AsO43-] in a 0.20-M arsenic acid solution.

85% (87 ratings)
###### FREE Expert Solution

Arsenic acid (H3AsO4) is a weak oxyacid with only one oxygen greater than hydrogen. H3AsO4 is a triprotic acid, meaning it can donate three protons (H+)

It has three K values and it will have three equilibrium reactions.

85% (87 ratings)
###### Problem Details

Arsenic acid (H3AsO4) is a triprotic acid with K a1 = 5.5 X 10 -3, Ka2 = 1.7 X 10 -7, and Ka3 = 5.1 X 10-12. Calculate [H+], [OH-], [H3AsO4], [H2AsO4-], [HAsO42-], and [AsO43-] in a 0.20-M arsenic acid solution.

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Polyprotic Acid concept. You can view video lessons to learn Polyprotic Acid Or if you need more Polyprotic Acid practice, you can also practice Polyprotic Acid practice problems .

How long does this problem take to solve?

Our expert Chemistry tutor, Alyssa took 14 minutes to solve this problem. You can follow their steps in the video explanation above.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Hove's class at RUTGERS.

What textbook is this problem found in?

Our data indicates that this problem or a close variation was asked in . You can also practice practice problems .