Question 4 for A=456.4;B=2.85; The pH of rain water can be approximated by considering the dissolution to equilibrium of CO2 in pure expect the pH to be? Instead of rain water in the atmosphere, what would the pH be if pure water is in equilibrium with CO2 at a partial pressure of Batm (which is similar to a soda can)? ( KH=0.0334mol (Latm)1;pKal,=6.35,pKal,=10.33). Relevant chemical equations: CO2(g)HH2CO3(aq) Hint: For simplifying the mass balance, you need to do two comparisons: [H+]vs. [OH]and [HCO3] vs. [CO32]. Alpha's of carbonate svstem 0=[H+]/[H+]2+Ka1[H+]+Ka1Ka2)1=Ka1[H+]/[H+]2+Ka1[H+]+Ka1Ka2)2=Ka1Ka2/[[H+]2+Ka1[H+]+Ka1Ka2)