Acid: Difference between revisions
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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 | 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 | 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 | 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]]. | Also see [[Alkali|alkali]]. | ||
=== | === Brønsted Lowry Acid === | ||
A molecule that donates a [[Proton|proton]]. | A molecule that donates a [[Proton|proton]]. | ||
=== Lewis Acid === | |||
A Molecule that can accept a pair of [[Electrons|electrons]]. | |||
Structure - ends with -COOH | |||
Structure - ends with -COOH | |||
[[Hydrochloric acid|Hydrochloric acid]] | [[Hydrochloric acid|Hydrochloric acid]] | ||
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H<sup>+</sup> Cl<sup>-</sup> | H<sup>+</sup> Cl<sup>-</sup> | ||
=== References === | === References === | ||
<references /> | <references /> | ||
Revision as of 10:48, 23 October 2017
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.
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.