Apr 9, 2014 · The pKa of H3O^+ is 0.0. The pKa of water is 14.0. As a simple proof, the pKa of the Na+ ion in water is 13.9

Oct 25, 2015 · The H3O+ ion is considered to be the same as the H+ ion as it is the H+ ion joined to a water molecule. The proton cannot exist in aqueous solution, due to its positive charge it is attracted to the electrons on water molecules and the symbol H3O+ is …

Dec 1, 2012 · Once this was recognized, chemists started to write the bare proton as being bound to a water molecule, thus $\ce{H3O^+}$. However, studies also showed that water molecules are typically linked together in clusters containing a fair number of water molecules held together by hydrogen bonds (Google for this if you are not familiar with it).

Science; Chemistry; Chemistry questions and answers; Calculate either [H3O+] or [OH−] for each of the solutions at 25 °C.

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Mar 22, 2018 · I expected $\ce{H3O+}$ to be a nucleophile due to the presence of electrons in the $\ce{2p}$ orbitals of $\ce{O}$. But the answer key of the test states that its none of them. I can rationalise it this way: If $\ce{O}$ donates its 2 electrons then there would be 2 positive charges on $\ce{O}$ leading to instability.

That seems to matter here because in first case H3O+ will not even be acidic in water as the equilibrium H2O + H+ ---» H3O+ has a very high equilibrium constant. 2) Similarly even if the solvent is NH3, the equilibrium constant of NH3 + H3O+ ---» NH4+ + H2O would be very low due to the same reason, and hence it would actually be a very weak acid.

Nov 30, 2021 · $\begingroup$ Because nobody is sure that aqueous hydrogen cation is always made of $\ce{H3O^+}$. Some scientists think that Hydrogen cations may also be making more complex ions in water, like $\ce{H5O2^+}$ or even$\ce{H_{2n+1}O_n^+}$ with n>2. $\endgroup$

Jun 7, 2016 · Due to the abundance of water in solution, molecules of $\ce{H2O}$ will readily pick up the hydrogen ions, meaning that most of the $\ce{H+}$ in an aqueous solution is actually of the form $\ce{H3O+}$. While this is the case, using $\ce{H+}$ over $\ce{H3O+}$ is more correct in general contexts.

Which after looking at Wikipedia, looks like a simplified definition, but it got me thinking - how can water have a pH of around seven if it dissociates into $\ce{H3O+}$ instead of $\ce{H+}$? Why does it do this instead of the expected dissociation?