Diprotic | Wikipedia audio article
Channel: Subhajit Sahu
Date: 13/12/2018

This is an audio version of the Wikipedia Article:
Diprotic


00:03:01 1 Definitions and concepts
00:03:53 1.1 Arrhenius acids
00:05:38 1.2 Brønsted–Lowry acids
00:08:34 1.3 Lewis acids
00:10:54 2 Dissociation and equilibrium
00:12:56 3 Nomenclature
00:13:12 4 Acid strength
00:14:04 5 Chemical characteristics
00:16:26 5.1 Monoprotic acids
00:16:35 5.2 Polyprotic acids
00:17:36 5.3 Neutralization
00:26:09 5.4 Weak acid–weak base equilibrium
00:26:16 6 Titration
00:27:28 6.1 Example: Diprotic acid
00:28:09 6.1.1 Equivalence points
00:28:51 6.1.2 Buffer regions and mid points
00:29:09 7 Applications of acids
00:30:05 7.1 In industry
00:30:45 7.2 In food
00:31:07 7.3 In human bodies
00:32:31 7.4 Acid catalysis
00:34:13 8 Biological occurrence
00:35:30 9 Common acids
00:36:02 9.1 Mineral acids (inorganic acids)
00:40:50 9.2 Sulfonic acids
00:40:59 9.3 Carboxylic acids
00:42:11 9.4 Halogenated carboxylic acids
00:43:10 9.5 Vinylogous carboxylic acids
00:44:06 9.6 Nucleic acids
00:44:36 10 References
00:45:01 11 External links



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SUMMARY
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An acid is a molecule or ion capable of donating a hydron (proton or hydrogen ion H+), or, alternatively, capable of forming a covalent bond with an electron pair (a Lewis acid).The first category of acids is the proton donors or Brønsted acids. In the special case of aqueous solutions, proton donors form the hydronium ion H3O+ and are known as Arrhenius acids. Brønsted and Lowry generalized the Arrhenius theory to include non-aqueous solvents. A Brønsted or Arrhenius acid usually contains a hydrogen atom bonded to a chemical structure that is still energetically favorable after loss of H+.
Aqueous Arrhenius acids have characteristic properties which provide a practical description of an acid. Acids form aqueous solutions with a sour taste, can turn blue litmus red, and react with bases and certain metals (like calcium) to form salts. The word acid is derived from the Latin acidus/acēre meaning sour. An aqueous solution of an acid has a pH less than 7 and is colloquially also referred to as 'acid' (as in 'dissolved in acid'), while the strict definition refers only to the solute. A lower pH means a higher acidity, and thus a higher concentration of positive hydrogen ions in the solution. Chemicals or substances having the property of an acid are said to be acidic.
Common aqueous acids include hydrochloric acid (a solution of hydrogen chloride which is found in gastric acid in the stomach and activates digestive enzymes), acetic acid (vinegar is a dilute aqueous solution of this liquid), sulfuric acid (used in car batteries), and citric acid (found in citrus fruits). As these examples show, acids (in the colloquial sense) can be solutions or pure substances, and can be derived from acids (in the strict sense) that are solids, liquids, or gases. Strong acids and some concentrated weak acids are corrosive, but there are exceptions such as carboranes and boric acid.
The second category of acids are Lewis acids, which form a covalent bond with an electron pair. An example is boron trifluoride (BF3), whose boron atom has a vacant orbital which can form a covalent bond by sharing a lone pair of electrons on an atom in a base, for example the nitrogen atom in ammonia (NH3). Lewis considered this as a generalization of the Brønsted definition, so that an acid is a chemical species that accepts electron pairs either directly or by releasing protons (H+) into the solution, which then accept electron pairs. However, hydrogen chloride, acetic acid, and most other Brønsted-Lowry acids cannot form a covalent bond with an electron pair and are therefore not Lewis acids. Conversely, many Lewis acids are not Arrhenius or Brønsted-Lowry acids. In modern terminology, an acid is implicitly a Brønsted acid and not a Lewis acid, since chemists almost always refer to a Lewis acid explicitly as a Lewis acid.