Difference between revisions of "Acid"
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| − | An '''acid''' is a [[molecule]] that creates H<sup>+</sup> and H<sub>3</sub>O<sup>+</sup> ions in water (according to the Arrhenius definition), that donates H<sup>+</sup> [[ions]] ([[proton]]s) in a chemical reaction (according to the [[Bronsted-Lowry theory|Bronsted-Lowry]] definition), or that accepts an electron pair in a reaction(according to the Lewis definition) | + | An '''acid''' is a [[molecule]] that creates H<sup>+</sup> and H<sub>3</sub>O<sup>+</sup> ions in water (according to the Arrhenius definition), that donates H<sup>+</sup> [[ions]] ([[proton]]s) in a chemical reaction (according to the [[Bronsted-Lowry theory|Bronsted-Lowry]] definition), or that accepts an electron pair in a reaction(according to the Lewis definition). |
| − | ==See | + | ==Properties== |
| + | Acids taste sour and turn blue [[litmus paper]] red; they have pH values of less than 7. Acids are covalent compounds, but when dissolved in [[water]], they will conduct electricity. When an Arrhenius acid is put into water, it will lose its H<sup>+</sup>, a process called aqueous dissociation. [[Strong acid]]s are those that completely give up their protons in solution, whereas [[weak acid]]s reach an equilibrium concentration of H<sup>+</sup> in solution. Many [[organic molecule]]s that play important roles in biological processes are also acids, such as [[amino acid]]s and [[carboxylic acid]]s. | ||
| + | |||
| + | ==Safety== | ||
| + | '''Never''' taste, or even touch, an acid stronger than 5% acetic acid, commonly known as vinegar; acids can be highly corrosive. | ||
| + | |||
| + | ==See also== | ||
*[[Base]] | *[[Base]] | ||
| + | *[[Common Acids]] | ||
*[[pH]] | *[[pH]] | ||
| + | [[Category:Acid–base chemistry]] | ||
[[Category:Chemistry]] | [[Category:Chemistry]] | ||
Latest revision as of 12:33, April 9, 2017
An acid is a molecule that creates H+ and H3O+ ions in water (according to the Arrhenius definition), that donates H+ ions (protons) in a chemical reaction (according to the Bronsted-Lowry definition), or that accepts an electron pair in a reaction(according to the Lewis definition).
Properties
Acids taste sour and turn blue litmus paper red; they have pH values of less than 7. Acids are covalent compounds, but when dissolved in water, they will conduct electricity. When an Arrhenius acid is put into water, it will lose its H+, a process called aqueous dissociation. Strong acids are those that completely give up their protons in solution, whereas weak acids reach an equilibrium concentration of H+ in solution. Many organic molecules that play important roles in biological processes are also acids, such as amino acids and carboxylic acids.
Safety
Never taste, or even touch, an acid stronger than 5% acetic acid, commonly known as vinegar; acids can be highly corrosive.
