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 …

Apr 9, 2014 · There is the problem of having 55.56 molar hydronium re its counterion being included. Consider water azeotropes of strong acids not by wt-% but by mole ratio. Is there anything …

Why does water dissociate to $\ce {H3O+ + OH-}$ instead of $\ce {H+ + OH-}$? This question came to surface when I was learning about acids and bases, and learned this definition:

Jul 15, 2016 · I know as a fact that HCl is a stronger acid than H3O+, but I want to know the reason behind it. The definition of an acid is a substance which dissociates to give H3O+ ions. In that case …

Jan 24, 2016 · 1 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 …

0 H3O+ is just the combination of a a $\ce {H+}$ ion, which we know to be released from the dissociation of an acid in an aqueous solution, with a water molecule.

5 This question already has answers here: What is the pKa of the hydronium, or oxonium, ion (H3O+)? (3 answers)

Dec 1, 2012 · I am doing my chemistry homework and I am supposed to write the products when strong acids react with water, but I am unsure of the physical state for hydronium ions. Should it be liquid (l) …

Jun 7, 2016 · 3 When dealing with an aqueous solution, you are correct that the $\ce {H+}$ ion is equivalent to $\ce {H3O+}$ for all intents and purposes. Due to the abundance of water in solution, …

May 30, 2014 · Yes, $\ce {H3O^+}$ is a closer representation of reality and so if "that" is important to you, then you would use $\ce {H3O^+}$. However, I could imagine someone else arguing that …