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


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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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