Alkalinity has been defined as the acid-neutralizing capacity of a water, and we commonly use the...

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Alkalinity has been defined as the acid-neutralizing capacity of a water, and we commonly use the following definition for the alkalinity of natural waters: Alk (eq/L) = [OH] + [HCO3] + 2[CO3]-[H]; where [X] = molar concentration of species X (a) How does one convert concentrations from moles/L to eq/L? (b) Why do the carbonic acid species play a role in natural alkalinity? And why do the acetic acid. species not play a role in natural alkalinity? (c) Given a natural water with pH = 9.3, Alk= 75 mg/L as CaCO3, and pK₁ = 6.35 and pk₂= 10.33 for carbonic acid, report the molar concentrations of each of the carbonic acid species: [H₂CO3], [HCO3] and [CO3²]. Alkalinity has been defined as the acid-neutralizing capacity of a water, and we commonly use the following definition for the alkalinity of natural waters: Alk (eq/L) = [OH] + [HCO3] + 2[CO3]-[H]; where [X] = molar concentration of species X (a) How does one convert concentrations from moles/L to eq/L? (b) Why do the carbonic acid species play a role in natural alkalinity? And why do the acetic acid. species not play a role in natural alkalinity? (c) Given a natural water with pH = 9.3, Alk= 75 mg/L as CaCO3, and pK₁ = 6.35 and pk₂= 10.33 for carbonic acid, report the molar concentrations of each of the carbonic acid species: [H₂CO3], [HCO3] and [CO3²].

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