Strong base
From Biocrawler, the free encyclopedia.
| Acids and Bases: |
|---|
| Acid-base reaction theories |
| pH |
| Self-ionization of water |
| Buffer solutions |
| Systematic naming |
| Redox reactions |
| Electrochemistry |
| Strong acids |
| Weak acids |
| Strong bases |
| Weak bases |
A strong base is a basic chemical compound that is able to deprotonate very weak acids in an acid-base reaction. The strength of a base is indicated by its pKb value, compounds with a pKb of less than about 1 are called strong bases. Common examples of strong bases are the hydroxides of alkali metals and alkaline earth metals like NaOH and Ca(OH)2. In water strong bases form hydroxyl ions (OH-), either by complete dissociation through solvation (metal hydroxides) or by chemical reaction with water (e.g. NaH and LDA).
The general reaction of a base with water is:
A-(aq) + H2O(l) ↔ HA(aq) + OH-(aq)
Very strong bases are even able to deprotonate very weakly acidic C-H groups in the absence of water.
| Contents |
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Common examples
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Medium strong bases
- Sodium hydrogen carbonate (NaHCO3)
- Sodium carbonate (Na2CO3)
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Strong bases
- Sodium hydroxide (NaOH)
- Potassium hydroxide (KOH)
- Barium hydroxide (Ba(OH)2)
- Calcium hydroxide (Ca(OH)2)
- Lithium hydroxide (LiOH)
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Very strong bases
- Sodium hydride (NaH)
- Sodium amide (NaNH2)
- Lithium diisopropylamide (LDA)
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See also
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External links
- (to be provided)
