# Problem: 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.

###### FREE Expert Solution

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

95% (182 ratings) ###### Problem Details

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.

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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.

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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.