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.