Given that Ka = 2.9*10^-4 moldm^-3, calculate the pH of 0.010moldm^-3 carbonic acid
Ka = [H2CO3][HCO3−][H3O+] Am I correct in saying H2O(l) doesnt effect Ka ? And that [H3O+] = [H+] ? (why is this please?)
Ka=2.0×10−4moldm−3=0.010[HCO3−][H+]
Im not sure how to work out [HCO3-]...theres no volume given so I cant use c=m/v...or can you assuem the reaction uses exactly 1mol of H2CO3(aq) and therefore use v = m/c..or would that only give the volume of H2CO3- ?
Please help!
Thank you
P.S. sorry im not sure how to do subscripts on here
yeah beacuse H+ and A- have the same concentrations, then you can treat them as the same value. So you just square the concentration of H+ (well thats the generally accepted method of doing it but it still works mathematically if you do it the other way, obviously).