The following aqueous solutions are common laboratory acids. What are their names? (a) HCl(aq); (b) \(\mathrm{H}_{2} \mathrm{SO}_{4}(\mathrm{aq}) ;\) (c) \(\mathrm{HNO}_{3}\) (aq); (d) \(\mathrm{CH}_{3} \mathrm{COOH}\) (aq); (e) \(\mathrm{H}_{2} \mathrm{SO}_{3}\) (aq); (f) \(\mathrm{H}_{3} \mathrm{PO}_{4}\) (aq).

Understanding the chemical formulas of acids is crucial in the field of chemistry, as it allows one to quickly identify the composition and properties of these substances. Acids are defined by their hydrogen ion (proton) donors when dissolved in water. The formulas represent the ratio of hydrogen ions to other elements or compounds in the acid molecule.

For example, hydrochloric acid (HCl) consists of hydrogen (H) and chlorine (Cl), indicating one hydrogen ion for each chlorine atom. Similarly, sulfuric acid (H_{2}SO_{4}), has two hydrogen ions for every sulfate group (SO_{4}). Organic acids, like acetic acid (CH_{3}COOH), include a carboxyl group (COOH) where the acidity primarily comes from the hydrogen atom of this functional group. It's essential for students to memorize these formulas and understand the systematic way in which they are named, as this helps in predicting the behavior of the acids in chemical reactions.

Inorganic acids are a fundamental category within chemistry, playing crucial roles in various industrial and biological processes. They are typically derived from minerals and do not contain carbon-hydrogen (C-H) bonds. Some of the most common inorganic acids found in a laboratory setting include hydrochloric acid (HCl), sulfuric acid (H_{2}SO_{4}), nitric acid (HNO_{3}), sulfurous acid (H_{2}SO_{3}), and phosphoric acid (H_{3}PO_{4}).

Each of these acids features different properties and uses. For instance, hydrochloric acid is commonly used in cleaning products, while sulfuric acid is essential in battery production and the manufacturing of fertilizers. Nitric acid, on the other hand, is often utilized in the production of explosives and for etching metals. Knowing their distinct properties helps in understanding their potential risks and proper handling procedures in the laboratory.

Organic acids stand apart from inorganic acids mainly because they contain carbon and typically arise from living organisms or synthetic organic compounds. The characteristic feature of an organic acid is the presence of one or more carboxyl groups (–COOH). A carboxyl group consists of a carbon (C) atom double-bonded to an oxygen (O) atom and also bonded to a hydroxyl group (–OH).

Acetic acid (CH_{3}COOH), the acid found in vinegar, is one of the simplest organic acids and a classic example often encountered in both laboratory settings and everyday life. Its structure includes a methyl group (CH_{3}) linked to a carboxyl group. Other examples of organic acids include citric acid, lactic acid, and tartaric acid. Organic acids are commonly used in food preservation and as additives, given their ability to donate hydrogen ions and provide a sour taste.