Carbon dioxide dissolves in water to form carbonic acid, which is primarily dissolved CO2. Dissolved CO2 satisfies the equilibrium equation The acid dissociation constants listed in most standard reference texts for carbonic acid actually apply to dissolved CO2. For a CO2 partial pressure of 1.8×10–4 bar in the atmosphere, what is the pH of water in equilibrium with the atmosphere? (For carbonic acid Ka1 = 4.46× 10–7 and Ka2 = 4.69× 10–11).
given partial pressure = 1.8*10^-4 bar
atmospheric pressure = 0.9869 bar
so moles fraction of CO2 in air =1.8*10^-4/0.9826 =1.8239*10^-4
lets do the caclculation for one mole of air so no of moles CO2 =1.8239*10^-4
CO2 [g] <--------------> CO2[aq]
c-x x
given K =0.032= x/[c-x] where c initial concentration of CO2
so x= Kc/[1+K]= 0.032*1.8239*10^-4/[1+0.032]=5.65*10^-6 M
this concentraion will be the initial CO2 concentration in water
as Ka1 = [concentration of H+ ion]^2/x =4.46*10^-7
[concentration of H+ ion]^2 =4.46*10^-7*5.65*10^-6=2.52*10^-12
gives [H+]=1.588*10^-6 M
so pH = -log 1.588*10^-6 =5.799
Carbon dioxide dissolves in water to form carbonic acid, which is primarily dissolved CO2. Dissolved CO2...
Carbon dioxide dissolves in water to form carbonic acid, which is primarily dissolved CO2. Dissolved CO2 satisfies the equilibrium equation CO2(gas)<------>CO2(aq) K=0.032 M*atm-1 The acid dissociation constants listed in most standard reference texts for carbonic acid actually apply to dissolved CO2. For a CO2 partial pressure of 3.1×10-4 atm in the atmosphere, what is the pH of water in equilibrium with the atmosphere?
Carbon dioxide dissolves in water to form carbonic acid, which is primarily dissolved CO2. Dissolved CO2 satisfies the equilibrium equation. CO2 (g) <--> CO2 (aq) K= 0.032 M atm-1 The acid dissociation constants listed in most standard reference texts for carbonic acid actually apply to dissolved CO2. For a CO2 partial pressure of 8.8×10-4 atm in the atmosphere, what is the pH of water in equilibrium with the atmosphere?
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