Acids and bases Chemistry

Hydroxide ion

Hydroxide is a diatomic anion with chemical formula OH−. It consists of an oxygen and hydrogen atom held together by a covalent bond

Hydronium ion

the ion H3O+, consisting of a protonated water molecule and present in all aqueous acids.

acidic solution

An acidic solution is any aqueous solution which has a pH < 7.0

basic solution

A basic solution is a liquid mixture that has a pH level greater than 7, which typically means there are a greater number of hydroxide ions than hydrogen ions

conjugate acid

A conjugate acid, within the Brønsted-Lowry acid-base theory, is a species formed by the reception of a proton (H+) by a base—in other words, it is a base with a hydrogen ion added to it.

Conjugate base

A conjugate base is the particle that is left over after the acid loses its hydrogen ion

Strong acid

A strong acid is one that completely ionizes (dissociates) in a solution

Weak acid

A weak acid is an acid that dissociates incompletely, releasing only some of its hydrogen atoms into the solution

Ion produced constant - KW

In fact, pure water only has a pH of 7 at a particular temperature - the temperature at which the Kw value is 1.00 x 10-14 mol2 dm. KW = [H+][OH-]

Neutral solution

PH of 7. neither acidic or base

Strong base

Strong bases are bases which completely dissociate in water into the cation and OH- (hydroxide ion).

PH scale

The pH scale ranges from 0 to 14. A pH of 7 is neutral. A pH less than 7 is acidic. A pH greater than 7 is basic.

Weak Base

a weak base is a chemical base that does not ionize fully in an aqueous solution. As Brønsted-Lowry bases are proton acceptors

Neutralization reaction

neutralization is a chemical reaction in which an acid and a base react quantitatively with each other. Results in there being no excess of hydrogen or hydroxide ions present in solution

amphoteric

of a compound, especially a metal oxide or hydroxide able to react both as a base and as an acid.