Question

A soda pop has a pH = 3.80 at 25oC. Calculate the pressure of CO2 inside a closed-bottle of this soda pop at 25oC. Assume only water and CO2 are present and all dissolved CO2 is present as H2CO3. Ka,1(H2CO3) = 4.3 x 10-7 and ΔGfo(H2CO3,aq) = - 623.08 kJ/m

Please include all math steps.

The answer is Pco2=1.7atm

Answer 1

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3.80 10 PH T= 25°c pH [ht] - 3.80 = 10 = 1.58 x 1044 Kag (H2CO3) = 4.3 x 10-7 (25+273.15) K 298.15k H₂CO3 is a combination & H₂O and coz H2CO3 = H+ + HCOZ [H+] = [H.coz:] ka [ht] [HCO3 ] [ CH2603 J = [H20] [202] [H₂CO3] 4.3 x 10+ (1.58x10 Yx (1-58x104) (H₂CO3) 4.3 X 10-7 (1:58 x 10-42 [H₂o] [coz [H2O3 = 1 4.3 X 10.7 (1.588 10-42 [co] [Co2 J = (1-58 x 10-4]? 4.3 X 10.7 [Coza= 0.580 55 M. According to theory low - Khe X partial puesswe of ges [co] = ky x P co2 Pool = [co] Гka 3.33947 x 10.2 molar KH for Co2 = atm Pro2 = 0.58055 m 3.33947. X 10 2 M atm = 1.73 atm 1.7 atm Pressure of co2 is 1. f atm ca - Pcoz Thanks

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