Acids and Bases

Hydrochloric Acid ($HCl$)

A strong acid that completely dissociates in aqueous solution into hydrogen ions ($H^+$) and chloride ions ($Cl^-$).

Hydrobromic Acid ($HBr$)

A strong acid that dissociates fully in water to yield hydrogen ions ($H^+$) and bromide ions ($Br^-$).

Hydroiodic Acid ($HI$)

A strong acid known for its complete ionization in solution, releasing hydrogen ions ($H^+$) and iodide ions ($I^-$).

Nitric Acid ($HNO_3$)

A strong, highly corrosive mineral acid that dissociates completely into hydrogen ions ($H^+$) and nitrate ions ($NO_3^-$).

Sulfuric Acid ($H<em>2SO</em>4$)

A strong diprotic acid; its first dissociation step is complete, releasing hydrogen ions ($H^+$) and hydrogen sulfate ions ($HSO_4^-$).

Chloric Acid ($HClO_3$)

A strong oxoacid that undergoes full dissociation in water to produce hydrogen ions ($H^+$) and chlorate ions ($ClO_3^-$).

Perchloric Acid ($HClO_4$)

One of the strongest mineral acids, it completely ionizes in solution into hydrogen ions ($H^+$) and perchlorate ions ($ClO_4^-$).

Lithium Hydroxide ($LiOH$)

A strong base that dissociates completely in aqueous solution into lithium ions ($Li^+$) and hydroxide ions ($OH^-$).

Sodium Hydroxide ($NaOH$)

A strong base, often called lye, which dissociates fully in water to release sodium ions ($Na^+$) and hydroxide ions ($OH^-$).

Potassium Hydroxide ($KOH$)

A strong base that provides a high concentration of hydroxide ions ($OH^-$) through complete dissociation in water.

Rubidium Hydroxide ($RbOH$)

A strong base that ionizes completely in solution into rubidium ions ($Rb^+$) and hydroxide ions ($OH^-$).

Cesium Hydroxide ($CsOH$)

A very strong base that undergoes 100% dissociation in water to yield cesium ions ($Cs^+$) and hydroxide ions ($OH^-$).

Calcium Hydroxide ($Ca(OH)_2$)

A strong base that dissociates completely in water, although it has lower solubility compared to alkali metal hydroxides.

Strontium Hydroxide ($Sr(OH)_2$)

A strong base that fully dissociates into strontium ions ($Sr^{2+}$) and hydroxide ions ($OH^-$) in solution.

Barium Hydroxide ($Ba(OH)_2$)

A strong base that dissociates completely in aqueous solution, providing two moles of hydroxide ions ($OH^-$) per mole of base.

Hydrofluoric Acid ($HF$)

A weak acid that only partially dissociates in water; the strong bond between hydrogen and fluorine prevents full ionization.

Nitrous Acid ($HNO_2$)

A weak acid that exists in an equilibrium state in solution, with only a small fraction of molecules dissociating into ions.

Sulfurous Acid ($H<em>2SO</em>3$)

A weak, unstable acid that does not dissociate completely in water, formed by dissolving sulfur dioxide in water.

Carbonic Acid ($H<em>2CO</em>3$)

A weak acid formed when carbon dioxide dissolves in water, characterized by its partial dissociation and role in blood buffering.

Phosphoric Acid ($H<em>3PO</em>4$)

A weak, triprotic acid that dissociates in three stages, with each stage having a progressively smaller dissociation constant.

Acetic Acid ($CH_3COOH$)

The main component of vinegar; it is a weak organic acid that only partially ionizes into acetate ($CH_3COO^-$) and hydrogen ions.

Ammonia ($NH_3$)

A common weak base that reacts partially with water to form ammonium ions ($NH_4^+$) and hydroxide ions ($OH^-$).

Methylamine ($CH<em>3NH</em>2$)

An organic weak base (amine) that partially accepts a proton from water to produce methylammonium ions ($CH<em>3NH</em>3^+$).