Acid: Difference between revisions
No edit summary |
No edit summary |
||
| (22 intermediate revisions by 11 users not shown) | |||
| Line 1: | Line 1: | ||
pH value lower than 7. It is a substance that will react with [[ | An acid has a pH value lower than 7. It is a substance that will react with water to produce H<sub>3</sub>O<sup>+</sup> and with a base to neutralise to [[Water|water]] and a salt. On a universal indicator, [[Strong acids|strong acids]] show up as a red or dark orange colour, and weaker acids show up as an orange or yellow colour. | ||
Acid can cause serious damage to human health. The correct PPE ([[Personal Protective Equipment|Personal Protective Equipment]]) should be worn when working with acids. | |||
Acids can be and often are used as catalysts in chemical reactions such as the reaction between amide nucleophiles and imines. Using a Bronsted Lowry acid for this reaction produced an extremely high yield more than 99%<ref>Rowland GB, Zhang H, Rowland EB, Chennamadhavuni S, Wang Y, Antilla JC. Brønsted acid-catalyzed imine amidation. Journal of the American Chemical Society. 2005 Nov 16;127(45):15696-7.</ref>. | |||
Also see [[Alkali|alkali]]. | |||
=== Brønsted Lowry Acid === | |||
A molecule that donates a [[Proton|proton]], in the form of a hydrogen ion. | |||
=== Lewis Acid === | |||
A Molecule that can accept a pair of [[Electrons|electrons]]. | |||
Structure - ends with -COOH | |||
[[Hydrochloric acid|Hydrochloric acid]] | |||
[[Hydrochloric acid|HCl]] | |||
H<sup>+</sup> Cl<sup>-</sup> | |||
=== References === | |||
<references /> | |||
Latest revision as of 17:44, 4 December 2018
An acid has a pH value lower than 7. It is a substance that will react with water to produce H3O+ and with a base to neutralise to water and a salt. On a universal indicator, strong acids show up as a red or dark orange colour, and weaker acids show up as an orange or yellow colour.
Acid can cause serious damage to human health. The correct PPE (Personal Protective Equipment) should be worn when working with acids.
Acids can be and often are used as catalysts in chemical reactions such as the reaction between amide nucleophiles and imines. Using a Bronsted Lowry acid for this reaction produced an extremely high yield more than 99%[1].
Also see alkali.
Brønsted Lowry Acid
A molecule that donates a proton, in the form of a hydrogen ion.
Lewis Acid
A Molecule that can accept a pair of electrons.
Structure - ends with -COOH
H+ Cl-
References
- ↑ Rowland GB, Zhang H, Rowland EB, Chennamadhavuni S, Wang Y, Antilla JC. Brønsted acid-catalyzed imine amidation. Journal of the American Chemical Society. 2005 Nov 16;127(45):15696-7.