Carbonic acid is a diprotic acid, it can donate two protons (H+) and it will have two equilibrium reactions.
Ka1 = 4.3x10-7
• 1st equilibrium reaction: H2CO3(aq) + H2O(l) → HCO3-(aq) + H3O+(aq
Ka2 = 5.6x10-11
• 2nd equilibrium reaction: HCO3-(aq) + H2O(l) → CO32-(aq) + H3O+(aq)
• H3O+(aq) is also produced from the 2nd equilibrium reaction
Which of the following concentrations would be practically equal in a calculation of the equilibrium concentrations in a 0.134-M solution of H2CO3, a diprotic acid: [H3 O+], [OH−], [H2CO3], [HCO3 −], [CO3 2−]? No calculations are needed to answer this question.
Frequently Asked Questions
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 Diprotic Acid concept. You can view video lessons to learn Diprotic Acid. Or if you need more Diprotic Acid practice, you can also practice Diprotic Acid practice problems.
What professor is this problem relevant for?
Based on our data, we think this problem is relevant for Professor Teets' class at UH.
What textbook is this problem found in?
Our data indicates that this problem or a close variation was asked in Chemistry - OpenStax 2015th Edition. You can also practice Chemistry - OpenStax 2015th Edition practice problems.