What would be the concentration

Reference no: EM13534529

A) What is the aqueous phase CO2 concentration (mg/L) of a watersample that is not in equilibrium with the atmosphere and has a pH= 7.1, an alkalinity of 300 mg/L and a temperature of 25 degrees C?

This I was able to figure out, [CO2(aq)] = 8.74 x 10^ -4 M

Use pH to find [H+].

Alk = [HCO3 (-)] at this pH so I converted 300 mg/L into M.

Using the equilibrium expression and the Ka of it given in class(Ka = 4.47 x 10^ -7 M), I found [H2CO3 *] = 8.74 x 10^ -4 M.

In natural waters, [H2CO3 *] = [CO2(aq)] so therefore [CO2(aq)] =8.74 x 10^ -4 M.

note: [H2CO3 *] just means CO2 (aq) and H2CO3 combined becausethey're difficult to distinguish quantitatively.

B) What would be the concentration (in atm) of CO2 in the gas phase of this system?

Reference no: EM13534529

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