Strong acid

Acids and bases
Diagrammatic representation of the dissociation of acetic acid in aqueous solution to acetate and hydronium ions.
Acceptor number Acid Acid–base reaction Acid–base homeostasis Acid strength Acidity function Amphoterism Base Buffer solutions Dissociation constant Donor number Equilibrium chemistry Extraction Hammett acidity function pH Proton affinity Self-ionization of water Titration Lewis acid catalysis Frustrated Lewis pair Chiral Lewis acid
Acid types
Brønsted–Lowry Lewis Mineral Organic Oxide Strong Superacids Weak Solid
Base types
Brønsted–Lowry Lewis Organic Oxide Strong Superbases Non-nucleophilic Weak

In chemistry, a strong acid is an acid which ionizes (splits) completely in a solution of water. It always loses a proton (A H₊) when put in water. A weak acid does not always lose a proton, though; It can lose its proton, but not all the time. They also have a very low pH, usually between 1 and 3. Many strong acids have a negative pKa value, which means they are very strong.

The six common strong acids are: (Acronym:CBSPIN)

1. HydroChloric acid HCl
2. HydroBromic acid HBr
3. Sulfuric acid H₂SO₄
4. Perchloric acid HClO₄
5. HydroIodic acid HI
6. Nitric acid HNO₃

Almost strong acids include:

1. Chloric acid HClO₃

Strong Acid Media

• Image of a strong acid mostly dissociating. The small red circles represent H+ ions.

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  Image of a weak acid partly dissociating

• 2chlorobutanoic.png

  2-chlorobutanoic acid, used in acid

• 3chlorobutanoic.png

  3-chlorobutanoic acid, used in acid

• 4chlorobutanoic.png

  4-chlorobutanoic acid, used in acid

• Butanoic.png

  en:butyric acid aka butanoic acid

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  Perchloric-acid-2D-dimensions

• Chloric-acid-2D.png

  ChloricacidD

• Chlorous-acid-2D.png

  ChlorousacidD

• Hypochlorous-acid-2D-dimensions.svg

  Hypochlorous-acid-2D-dimensions