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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