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.

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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.

H3AsO4acidic form K1 H2AsO4-intermediate #1K2 HAsO42-intermediate #2K3 AsO43-basic form

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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.

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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.

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

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Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition practice problems.