# pH-dependency of the acidic dissociation of carbonic acid

I know the product of $\ce{CO2 +H2O}$ yields $\ce{H2CO3}$. This is a reversible equation so $\ce{H2CO3}$ goes back to $\ce{H2O + CO2}$. However, my question is: Is there a certain pH which will dissociate $\ce{H2CO3}$ into $\ce{H+}$ and $\ce{CO3^2-}$ ions? If so, lets say you started with $2\ \mathrm{mol}$ of $\ce{H2O}$ and $1\ \mathrm{mol}$ of $\ce{CO2}$, how many moles of $\ce{H+}$ and $\ce{CO3^2-}$ ions will form?

• Hi and welcome to chemistry.stackexchange.com. Since you already took the tour, all that remains is to guide you towards the help center where you can find useful hints, e.g. on how to format your posts with MathJax — check out what I did while editing your post ;) – Jan Jan 20 '16 at 22:52
• Related: Does H2CO3 exist in solution? – Loong Jan 20 '16 at 22:53
• At what temperature and pressure? Solubility of CO2 depends on them strongly. – Mithoron Jan 20 '16 at 22:56
• at 25 degrees and 1 atm – user510 Jan 20 '16 at 23:02