consider a 1.00 M solution of a weak acid, HA. The pH of thesolution is found to be 3.85. A) calculate the [H3O+] in thesolution. This would be the equilibrium concentration of H3O+ inthe solution. B) write out an ICE table as before. Here, we don’tknow the numerical value of Ka but we know the [H3O+] atequilibrium which you should see from your ICE table easily relatesto the value of “x†in your table and knowing “x†from [H3O+], onecan easily determine the other equilibrium concentrations of allspecies and solve for value of Ka.
C) [H3O+] = __________________
