Given: 0.010 M HCO3 Ka1 = 4.5 × 10–7 Ka2 = 4.7 × 10–11
ICE Chart for Ka1:
Calculate [CO32-] in a 0.010-M solution of CO2 in water (usually written as H2CO3). If all the CO32- in this solution comes from the reaction
HCO3-(aq) ⇌ H+(aq) + CO32-(aq)
what percentage of the H+ ions in the solution is a result of the dissociation of HCO3-? When acid is added to a solution of sodium hydrogen carbonate (NaHCO3), vigorous bubbling occurs. How is this reaction related to the existence of carbonic acid (H2CO3) molecules in aqueous solution?
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