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| Acid | a compound that produces hydrogen ions when dissolved in water. Chemical Formula usually HX(X = monatomic or polyatomic ion). Chemical formula = H+ |
| Base | a compound that produces hydroxide ions when dissolved in water. Bases are named as if they were ionic compounds (the name of the cation followed by the name of the anion). |
| Hydroxide Ion | A water molecule that loses a hydrogen ion and thus becomes negatively charged. Hydroxide ions are denoted OH-. (Do not conf. with hydronium ion) |
| Hydronium Ion | A water molecule that gains a hydrogen ion and thus becomes positively charged. Hydronium ions are denoted H3O+. (Do not conf. with hydroxide ion) |
| Self-Ionization | the reaction in which two water molecules react to give ions (for water.) The reaction is written as dissociation. |
| Neutral Solution | any aqueous solution in which [H+] and [OH-] are equal. For example pure water is a neutral substance. pH = 7.0 ([H+] = 1.0 x 10-7 mol/L) |
| Ion Production Constant for Water | The product of the concentrations of the hydrogen ions and hydroxide ions in water. It is denoted as Kw. |
| Acidic Solution | When the [H+] is greater than the [OH-]. Thus, the [H+] of an acidic solution is always greater than 1.0 x 10-7 mol/L. (don’t mix up with basic) |
| Basic Solution | When the [H+] is less than the [OH-]. Thus, the [H+] of an acidic solution is always less than 1.0 x 10-7 mol/L. (don’t mix up with Acidic) |
| Alkaline Solutions | another name for a basic solution. |
| pH | the negative logarithm of the hydrogen-ion concentration. pH=-log[H+]. Always express in scientific notation. |
| Svante Arrhenius’s Theory (1887) | Said that acids are compounds containing hydrogen that ionize to yield hydrogen ions (H+) in aqueous solution. In addition he said, bases are compounds that ionize to yield hydroxide ions (OH-) in aqueous solution. |
| Monoprotic Acid | any acid that contains one ionizable hydrogen. An example is Nitric Acid (HNO3). (conf. diprotic and triprotic) |
| Diprotic Acid | any acid that contains two ionizable protons. An example is Sulfuric Acid (H2SO4). (conf. monoprotic and triprotic) |
| Triprotic | any acid that contains three ionizable protons. An example is Phosphoric Acid (H3PO4). (conf. monoprotic and diprotic) |
| Bronsted’s-Lowry’s Theory | the theory defines an acid as a hydrogen-ion donor. As well a base is a hydrogen-ion acceptor. All of the acids and bases included in Arrenius theory are also acids and bases according to the Bronsted-Lowry theory. |
| Hydrogen-ion donor | a compound that produces hydrogen ions in solution, is a hydrogen-ion donor, or an electron- pair acceptor. (Conf. Hydrogen-ion acceptor) |
| Hydrogen-ion Acceptor | a compound that produces hydroxide ions in solution, is a hydrogen-ion acceptor, or an electron-pair donor. (Conf. Hydrogen-ion donor) |
| Conjugate Acid | the particle formed when a base gains a hydrogen ion. |
| Conjugate Base | the particle that remains when an acid has donated a hydrogen ion. |
| Conjugate Acid-Base Pair | two substances that are related by the loss or gain of a single hydrogen ion. |
| Amphoteric | a substance that can act as both an acid and a base. Water is amphoteric. |
| Indicator | a weak acid or base that undergoes dissociation in a known pH range. In this range the acid (or base) is a different color from its conjugate base (or acid). |
| Lewis Acid | a substance that can accept a pair of electrons to form a covalent bond. Theory was founded by Gilbert Lewis. |
| Lewis Base | a substance that can donate a pair of electrons to form a covalent bond. |
