Answer to Question #15657 in Other Chemistry for rahma

Question #15657
The below chemicals are added into a closed (no gas phase), perfectly
mixed vessel containing 1 litre of pure water, temperature remains constant at 25ºC.

Propionic Acid (CH3CH2COOH) = 0.03 mol
Sodium acetate (CH3COONa) = 0.02 mol
Sodium bicarbonate (NaHCO3) = 0.04 mol
Calcium carbonate (CaCO3) = 0.01 mol
Ammoniun Chloride (NH4Cl) = 0.02 mol
Ammonia (NH3) = 0.01 mol
Salt (NaCl) = 0.05 mol
NaOH = 0.02 mol
HCl = 0.0075 mol

1) 0.01 mol of hydrogen chloride (HCl) are added into the solution, calculate the new resulting
equilibrium pH.

2) After the addition of the HCl above the vessel is opened and left in contact with the
atmospheric air for a very long time. Assuming no liquid volume changes, calculate the new
equilibrium pH of the solution.
Concentration of CO2 in the atmosphere is 388 ppm (volumetric)
Equilibrium data for the temperature selected:
pKw = 13.669
pKProH = 4.733
pKAcH = 4.777
pKCO2 = 6.319
pKNH4+ = 8.979
KH,CO2 = 37.909 bar/M
Concentration of CO2 in the atmosphere is 388 ppm (volumetric)
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