2015年10月25日 · This shows that pure water is neither acidic or basic, it is neutral. The product of [H3O+] = [OH-] is the ionic product of water. [H3O+][OH-]=10^-7 × 10^-7 = 10^-14 . shows that in aqueous (water) solutions, whether acidic, basic or neutral, the product of the ion concentrations equals 10^-14. Acidic solutions contain more H3O+ ions than OH ...

In fact is not strictly self but a matter of "couple-ionization": you know the water atoms have different electronegativity, the more electronegative oxygen attracts the less electronegative hydrogen of another water molecule forming an hydrogen bonding.

2014年4月9日 · 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

2012年12月1日 · 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).

2016年1月24日 · The pH is close to 7. So the hydronium ion concentration of water can't be neglected. [H3O+fro water + H3O+ from acid][OH-]=10^-14. Please note that H2O dissociates partially to form H3O+ and OH- and that this process reaches equilibrium with finally the ionic product: [H+][OH-]=10^-14. If an acid is added to water.

2016年7月15日 · So far, we have only looked at water and its autoprotonation, no solvents and other molecules, which have their own acidies and basicities. 2) As for the reaction you mentioned in ammonia as a solvent, well, first of all, $\ce{H3O+}$ needs to come from somewhere (let's imagine we drop some aqueous solution of hydrochloric acid in there).

2016年6月7日 · These latter can be thought of as polymeric ions. (Because of charge repulsion, doubly negative species are a negligible component of liquid water.) The solvated (or aqueous) proton is generally just called the hydrogen ion, but other names are certainly possible. $\ce{H+}$ is the most common species in the Universe, but it doesn't exist in water.

2024年12月14日 · Are you saying when the acid and water become equivalent, all the water is turned to h3o so there is only trace while in dilute, only some of all the water is turned to h2o meaning in dilute strong acid solution, there is much more h2o molecules. Rather equimolar. And yes, you like repeat the obvious, paraphrasing what I have said.

2017年11月6日 · When water forms, oxygen shares two non-bonded electrons with hydrogen atoms, forming a covalent bond with them. $\ce{H3O+}$ forms via donor-acceptor bonding, when oxygen supplies its lone pair, which it has two, to form a bond with $\ce{H+}$ ion. To form $\ce{H3O-}$, you'll need an interaction between water molecule and $\ce{H-}$ ion.

2014年5月30日 · $\begingroup$ Nothing is "wrong" with $\ce{H3O+}$, but one needs to keep in mind that is a shorthand notation often used to describe reality, but it is not real itself, As the Wkipedia link says, "The reality is far more complicated, as a proton is bound to several molecules of water, such that other descriptions such as H5O2+, H7O3+ and H9O4 ...