# Hydration number: Carbonic acid in water

Carbonic acid ($\ce{H2CO3}$) is known to be soluble in water, and that this particular compound is unstable, so much so that according to the 2014 article from Berkeley Lab: New Insights on Carbonic Acid in Water, it only exists for a fraction of a second (300 nanoseconds according the article).

Newly reported experiments and observations from the Berkeley Lab found that:

“Our results support an average hydration number of 3.17 with the acid’s two protons each donating a strong hydrogen bond to solvating waters, the carbonyl oxygen accepting a strong hydrogen bond from solvating water, and the hydroxyl oxygen molecules accepting weak hydrogen bonds from the water”

What is not clear is how is the hydration number calculated and how does this relate to the short existence of carbonic acid in water?

• Please note, the first two links point to the linked questions indicated for this question. – user15489 Jun 26 '15 at 8:45

Then, by analyzing the spectra, it is possible to calculate the approximate hydration number, as "the increasing H-bond strength is proportional to the hydration number (measured for distances up to $2.5\mathrm{\overset{\circ}A}$): $\ce{Na2CO3}$ (5.55), $\ce{HCO3}$ (4.26), $\ce{H2CO3}$ (3.17)".
• I will add that the radial distribution function ($g(r)$), which is used in this and similar studies to infer how many of (some species) are distributed around (some central point) up to (some distance), is tied directly to the hydration number. That quantity (as detailed in the reference given by Andy and in Kumar et al., referenced therein) is being interpreted to correspond to stronger hydrogen bonding if it's high, and weaker hydrogen bonding if it's low. – Todd Minehardt Jul 2 '15 at 18:09