A classification of acids and bases in chemistry depends on the ionization force of these substances in aqueous medium. A) Yes:
| Strong acids and bases | Weak acids and bases | |
|---|---|---|
| Definition | Substances that completely ionize in solution. | Substances that partially ionize in solution. |
| Ionization | Complete | Partial |
| Elements in aqueous solution | Cations and anions in the same concentration. | Cations, anions and molecules in different proportions. |
| Ionization constant | Elevated | Little |
| Examples |
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A acid or a base are strong when in an aqueous medium they dissociate completely, that is, the ionization process is total and the solution will contain the same concentration of anions and cations.
A strong acid, such as hydrochloric acid HCl, ionizes in the following ways:
A strong base, such as sodium hydroxide NaOH, ionizes in the following ways:
| Strong acids | Formula |
|---|---|
| Hydrochloric acid | HCl |
| Sulfuric acid | HtwoSW4 |
| Nitric acid | HNO3 |
| Hydrobromic acid | HBr |
| Perchloric acid | HClO4 |
| Chromic acid | HtwoCrO4 |
| Tetrafluroboric acid | HBF4 |
| Strong base | Formula |
|---|---|
| Sodium hydroxide | NaOH |
| Lithium hydroxide | LiOH |
| Potassium hydroxide | KOH |
| Rubidium hydroxide | RbOH |
| Cesium hydroxide | CsOH |
| Calcium hydroxide | Ca (OH)two |
| Barium hydroxide | Ba (OH)two |
| Strontium hydroxide | Sr (OH)two |
| Aluminum hydroxide | Al (OH)3 |
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A acid or a base is weak when in aqueous solution it partially ionizes, that is, in the solution there are ions and non-ionized molecules.
A weak acid, such as acetic acid CH3COOH, is ionized in the following way:
The equilibrium of this reaction is expressed by the two arrows in opposite directions.
When a weak acid dissociates or ionizes, an equilibrium is established between the species present in the solution; this can be expressed by a ionization constant sour:
The ionization constant is nothing more than the ratio between the multiplication of the concentration of the products over the multiplication of the concentration of the reactants.
A weak base, such as NH ammonia3, ionizes in the following way:
When a weak base dissociates or ionizes, an equilibrium is established between the species present in the solution; this can be expressed by a base ionization constant:
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| Weak acid | Formula | Ionization constant |
|---|---|---|
| Formic acid | HtwoCOtwo | 1.77 x 10-4 |
| Acetic acid | H3CCOH | 1.75 x 10-5 |
| Hydrocyanic acid | HOCN | 3.30 x 10-4 |
| Hydrogen cyanide | HCN | 6.20 x 10-10 |
| Hypochlorous acid | HOCl | 3.50 x 10-8 |
| Nitrous acid | HNOtwo | 4.00 x 10-4 |
| Lactic acid | HC3H5OR3 | 1.40 x 10-4 |
| Carbonic acid | HtwoCO3 | 4.30 x 10-7 5.60 x 10-eleven |
| Boric acid | H3BO3 | 5.80 x 10-10 1.80 x 10-13 3.00 x 10-14 |
| Weak base | Formula | Ionization constant |
|---|---|---|
| Ammonia | NH3 | 1.75 x 10-5 |
| Methylamine | CH3NHtwo | 4.38 x 10-4 |
| Ethylamine | CtwoH5NHtwo | 5.60 x 10-4 |
| Aniline | C6H5NHtwo | 3.80 x 10-10 |
| Pyridine | C5H5N | 1.70 x 10-9 |
| Benzylamine | C7H9N | 2.20 x 10-5 |
| Sodium bicarbonate | NaHCO | 2.00 x 10-4 |
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