Question

The pH of earth's water is controlled by the combination of several equilibria found in water, as well as between water and the atmosphere. This problem considers a model for oceanic water. H2CO3 + CO3 yields 2HCO3 1) Calculate the equilibrium constant for this equilibrium using Ka1 and Ka2 of carbonic acid. 3) Starting from a pure solution of HCO3, how are the concentrations of H2CO3 and CO3 related to each other? 4) Ocean water has an average pH of approx. 8.1. How are the concentrations of H2CO3 and CO3 related to each other in ocean water? 4) Do you think modeling ocean water as a pure dilute bicarbonate ion solution a good model

Answer 1

1) the equilibrium will be between

H₂CO₃ + CO₃^-2 --> 2HCO₃^-

Equilibrium constant = K = [HCO₃^-]^2 / [H₂CO₃][CO₃-2]

The Ka1 and Ka2 for H2CO3 will be

H2CO3 --> H+   + HCO3-

Ka1 = [H+] [ HCO₃^-] / [H₂CO₃]

HCO3- --> H+ + CO₃-2

Ka2 = [CO₃-2][H+] / [HCO₃^-]

so K =    Ka1 / Ka2

2) Question missing

3) HCO3- + H+ --> H2CO3 (1/Ka1)

1/Ka1 = [H2CO3] / [HCO3-] [H+]

Ka1 = [HCO3-] [H+] / [[H2CO3]

pKa1 = pHCO3- + pH - pH2CO3

pHCO3- = pKa1 - pH + pH2CO3......(1)

HCO3- ---> H+ + CO₃^-2     (Ka2)

Ka2 = [H+]'[CO3-2] / [HCO3-]

pKa2 = pH' + pCO3-2 - pHCO3-

pHCO3- = pH' + pCO3-2 -pKa2 ... ...(2)

So we can equate (1) and (2)

pKa1 - pH + pH₂CO₃ = pH' + pCO₃^-2 -pKa2

So (CO3^-2) = {(2Ka)/[H+]} X [HCO₃^-]

4) Average pH = 8.1

H2CO3 --> H+ + HCO3-

HCO3- --> H+ + CO3-2

[H+] = -antilog 8.1 = 7.94 X 10^-9

So if we know the concentratio of any species we can calcualte concentration of CO3-2 accrodingly

4) yes the modelling water is a good model