Reactions, Acids And Bases Flashcards
(24 cards)
Salt?
A substance in which the hydrogen of an acid has been replaced by a cation.
Hydrolysis of a salt?
A reaction of an ion (from a salt) with water. The pH of the salt solution is determined by the strength of the acid and base that have been used to form the salt.
Bronsted-Lowry Definition of an acid-base reaction?
A reaction that involves the transfer of protons (H+).
Bronsted-Lowry Definition of an acid?
An acid is a proton donor.
Strong acid?
An acid that ionises completely in an aqueous solution.
Weak acid?
An acid that only ionises partially in an aqueous solution. All organic acids are classified as weak acids.
Conjugate base?
The product formed or whatever is left over after an H+ has been donated. Compare from the acid reactant.
Bronsted-Lowry Definition of a base?
A base is a proton acceptor.
Strong base?
A base that dissociates completely in an aqueous solution. All Group 1 hydroxides are classified as strong bases.
Weak base?
A base that only dissociates partially in an aqueous solution.
Conjugate acid?
The product formed when an H+ is accepted. Compare using the base reactant.
Ionization?
The reaction of a molecular substance with water to produce ions. The ionization of a strong acid is written with a single arrow while that of a weak acid is written with a double arrow.
Dissociation?
The splitting of an ionic compound into its ions. The dissociation of a strong base is written with a single arrow while that of a weak base is written with a double arrow.
Neutralization (equivalence point)?
The point where both an acid and a base have reacted so that neither is in excess.
Redox Reaction?
A reaction involving the transfer of electrons.
Oxidation?
The loss of electrons.
Reduction?
The gain of electrons.
Oxidizing agent?
A substance that accepts electrons.
Reducing agent?
A substance that donates electrons.
What is an amphoteric (amphiprotic) substance and list 2 examples?
A substance that can act as either an acid or a base. It depends on the circumstances and examples: H2O, HSO4-, HCO3- and H2PO4-
Electron Richness?
The extent to which an atom completely or partially gains electrons.
Oxidation Number?
Is a measure of an atom’s or molecule’s electron richness.
What is the auto ionization constant for water and what does it apply to?
It is Kw = 1 x 10-14 and it applies to all aqueous solutions. The auto-ionisation of water is an endothermic reaction.
What does pH stand for what does it measure?
Stands for potential of hydrogen, and it measures the concentration of H3O+ ions in solution.
