Dissolving NaCl in water does not form HCl because sodium and chloride ions remain fully dissociated
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Reference literature confirms that sodium chloride is a strong electrolyte that dissociates fully into independent sodium and chloride ions in aqueous solution rather than reacting to form hydrochloric acid.
Strong and Weak Electrolytes
Electrolytes can be further classified as strong or weak electrolytes. Strong electrolytes are compounds like NaCl, which are nearly 100% dissociated in solution. This means that nearly every sodium chloride formula unit exists as sodium ions surrounded by water molecules and chloride ions surrounded by water molecules. We can represent this by the following equation:
\[\ce{NaCl(s) -> Na^{+}(aq) + Cl^{–}(aq)} \nonumber \]
The Proton in Chemistry
Acids and bases form a special and very important class of electrolytes. Some acids, such as hydrochloric acid, HCl, almost completely dissociate in aqueous solution. They are strong electrolytes. These acids are similar to sodium chloride in that they exist as ions when in solution. Other acids such as acetic acid, CH3COOH, dissociate only slightly when dissolved in water. These are classified as weak electrolytes. For example, at a certain concentration and temperature, only four of every one hundred acetic acid molecules will ionize in solution.
In the Arrhenius theory, sodium hydroxide is a base, and hydrochloric acid is an acid, which has the Arrhenius neutralization reaction
- NaOH + HCl → NaCl + H2O
that produces a salt (sodium chloride) and water. In the Brønsted-Lowry theory, sodium hydroxide is no longer considered a base, but rather an equivalent of the actual base, the hydroxide ion OH−. When sodium hydroxide dissolves, it splits into OH− and Na+. The sodium is considered a spectator ion that does not participate in the actual reaction. The acid-base reaction is
- HCl + OH− → Cl− + H2O
Here, the chloride ion is the conjugate base of HCl, while water is the conjugate acid of OH−. The dissolved ions making sodium chloride is not part of the acid-base reaction. References
- ↑ "Brønsted–Lowry theory | chemistry". Encyclopedia Britannica. Retrieved 2025-06-06. - ↑ IUPAC, Compendium of Chemical Terminology, 5th ed. (the "Gold Book") (2025). Online version: (2006–) "Acid". doi:10.1351/goldbook.A00071
- ↑ Brönsted, J. N. (1923). "Einige Bemerkungen über den Begriff der Säuren und Basen" [Some observations about the concept of acids and bases]. Recueil des Travaux Chimiques des Pays-Bas. 42 (8): 718–728.
acid (HCl) with sodium hydroxide (NaOH) solutions produces a solution of sodium chloride (NaCl) and some additional water molecules. HCl ( aq ) + NaOH (
In chemistry, an acid–base reaction is a chemical reaction that occurs between an acid and a base. It can be used to determine pH via titration. Several theoretical frameworks provide alternative conceptions of the reaction mechanisms and their application in solving related problems; these are called the acid–base theories, for example, Brønsted–Lowry acid–base theory.
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The modifier (aq) in this equation was implied by Arrhenius, rather than included explicitly. It indicates that the substances are dissolved in water. Though all three substances, HCl, NaOH and NaCl are capable of existing as pure compounds, in aqueous solutions they are fully dissociated into the aquated ions H+, Cl−, Na+ and OH−.
The…
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