H2CO3(aq) + H2O <--> HCO3-(aq) + H3O+(aq)
Given that Ka = 2.9*10^-4 moldm^-3, calculate the pH of 0.010moldm^-3 carbonic acid
Ka = Am I correct in saying H2O(l) doesnt effect Ka ? And that [H3O+] = [H+] ? (why is this please?)
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- ?
P.S. sorry im not sure how to do subscripts on here
pH calculation help please :) Watch
- Thread Starter
- 02-12-2010 20:50
- 02-12-2010 21:14
For a weak acid such as this: HA ---> H+ + A-
and so [A-] = [H+] so Ka = [H+]2/[HA]
how to do subscripts and superscripts: http://www.thestudentroom.co.uk/anno...hp?f=130&a=581
- 02-12-2010 21:48
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).