Answer:
In a neutralization reaction, hydronium and hydroxide ions react to form water.
Step-by-step explanation:
Acids/Bases and how they interact:
A Bronsted-Lowry base is a substance that tends to bond with and "steal" a hydrogen ion, while an acid is a molecule containing a hydrogen ion that prefers to dissociate. Acids "give up" their hydrogen ions to water molecules in water, resulting in the formation of a hydronium ion. The pH of a given solution is determined by the amount of hydronium ions present.
A quick neutralization reaction takes place when a base is added to an acid because bases want to "take" the hydrogen. We have the ideal combination of bases that want to "take" the hydrogen ion and acids that want to "give up" the hydrogen ion, which allows them to neutralize one another. A conjugate base is created when hydrogen separates from an acid; having had its hydrogen torn from the complex, it may now receive a hydrogen (i.e., acts as a base). Once the base has a hydrogen, it behaves as a conjugate acid; it may then "lose" that hydrogen and behave as an acid.
Depending on which form the molecule favors, the acid's potency varies. The fact that hydrochloric acid (HCl) fully dissociates in aqueous solutions makes it a powerful acid:
HCl + H₂O -> Cl- + H₃O+
That is to say that the reaction equation strongly favours the right side.
Acetic acid, on the other hand, is a weak acid because only a small part of it dissociates:
CH₃COOH + H₂O <--> CH₃COO- + H₃O+
In contrast to the bulk of the chemical, which is shown on the left in the uncharged state, only a minor portion of acetic acid dissociates.
This brief explanation of acids and bases anthropomorphizes chemical substances as aware creatures with specific preferences for certain actions. These so-called "preferences" are, in reality, rough summaries of the relative stabilities of the compounds (acid vs. its conjugate base), mostly as a result of electrical processes.