Acids
Definition
Acids are substances that can donate a proton (H+) to another substance and typically have a pH less than 7. They are often characterized by their sour taste and ability to turn blue litmus paper red.
5 Must Know Facts For Your Next Test
- Acids are defined by the Arrhenius, Brønsted-Lowry, and Lewis theories, each providing a different perspective on their behavior.
- The strength of an acid is determined by its ability to ionize in water; strong acids completely dissociate while weak acids partially dissociate.
- Common examples of acids include hydrochloric acid (HCl), sulfuric acid (H2SO4), and acetic acid (CH3COOH).
- In chemical nomenclature, acids containing oxygen are named based on the polyatomic ion they contain; for instance, HNO3 is nitric acid because it contains the nitrate ion.
- The pH scale is logarithmic, so each whole number change represents a tenfold change in hydrogen ion concentration.
Review Questions
- What defines an acid according to the Brønsted-Lowry theory?
- How does the strength of an acid relate to its degree of ionization in water?
- What is the correct name for H2SO4 using chemical nomenclature?
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Related terms
Base: A substance that can accept a proton (H+) or donate an electron pair in reactions. Bases typically have a pH greater than 7.
pH Scale: A scale used to specify how acidic or basic a water-based solution is. It ranges from 0 to 14, with 7 being neutral.
Ionization: The process by which an atom or molecule gains or loses electrons to form ions. In the context of acids, it refers to the dissociation into H+ ions in water.
