Term
|
Definition
| The ion H3O, consisting of a protonated water molecule and present in all aqueous acids. |
|
|
Term
|
Definition
| Any substance that donates hydrogen ion (proton). |
|
|
Term
|
Definition
| Any substance that accepts a proton. |
|
|
Term
|
Definition
Brønsted-Lowry acids and Lewis acids. It means a substance capable of donating and accepting protons, such as water and bicarbonate. Amphiprotic species must have acidic protons.
All amphiprotic substances are amphoteric; not all amphoteric species are amphiprotic. |
|
|
Term
|
Definition
Lewis acids. It means a substance capable of acting both as a lone pair acceptor and a lone pair donor, such as aluminium hydroxide and tin dioxide. Amphoteric species don't necessarily need acidic protons.
All amphiprotic substances are amphoteric; not all amphoteric species are amphiprotic. |
|
|
Term
|
Definition
| Acids form a conjugate base. |
|
|
Term
|
Definition
| Bases form a conjugate acid. |
|
|
Term
|
Definition
Ex) HNO3 + H2O -> H3O + NO3
A B CA CB |
|
|
Term
|
Definition
when H2O breaks down into H+ and OH-. the reaction is at equilibrium, because the H2O is always breaking down into H+ and OH-, which is constantly forming H2O.
It is at a pH 7 because the [H+] concentration is going back and forth at equilibrium, causing it to be neutral. |
|
|
Term
|
Definition
|
|
Term
|
Definition
| A measure of how acidic or basic (alkaline) an aqueous solution is. |
|
|
Term
| Acid Dissociation Constant, Ka |
|
Definition
| The acid dissociation constant is the equilibrium constant of the dissociation reaction of an acid and is denoted by Ka. |
|
|
Term
|
Definition
| The percentage of the weak electrolyte that ionizes in a solution of given concentration. |
|
|
Term
|
Definition
| An Acid that can form two or more hydronium ions per molecule; often a least one step of ionization is weak. |
|
|
Term
| Base Dissociation Constant, Kb |
|
Definition
| Equilibrium constant that measures the extent of dissociation for a base. |
|
|
Term
|
Definition
| When water reacts with another substance and as a result the oxygen in water makes a bond with the substance. |
|
|
Term
|
Definition
An oxyacid is an acid that contains an oxygen atom bonded to a hydrogen atom and at least one other element.
Ex) Sulfuric acid (H2SO4), phosphoric acid (H3PO4), and nitric acid (HNO3) are all oxyacids. |
|
|
Term
|
Definition
Carboxylic acid is an organic compound containing the COOH functional group.
Ex) acetic acid, CH3COOH |
|
|
Term
|
Definition
| A substance that can accept an electron pair from a base; thus, AlCl3, BF3, and SO3 are acids. |
|
|
Term
|
Definition
| A substance that can donate an electron pair; examples are the hydroxide ion, OH-, and ammonia, NH3. |
|
|
Term
|
Definition
| The lowering of the degree of ionization of a compound when another ionizable compound is added to a solution; the compound added has a common ion with the other compound. |
|
|
Term
| Buffered Solutions (Buffers) |
|
Definition
| Buffer systems contain both an acid and a base(either an acid and its conjugate base or a base and its conjugate acid). |
|
|
Term
|
Definition
| The relative ability of a buffer solution to resist pH change upon addition of an acid or a base. |
|
|
Term
| Henderson-Hasselbalch equation |
|
Definition
| An equation expressing the pH of a buffer solution as a function of the concentration of the weak acid or base and the salt components of the buffer. |
|
|
Term
|
Definition
| A curve relating pH to the equivalents of strong base added per equivalent of acid in the solution. |
|
|
Term
|
Definition
| Indicators are dyes which change colors to show acidity or alkalinity. These are qualitative because they show acidity or alkalinity by changing color. |
|
|
