Acids and Bases Flashcards
pH of acids
less than 7
pH of bases
greater than 7
properties of acids
sour taste
able to change color of acid-base indicators
reactive with metals to release hydrogen gas
reactive with bases to produce salts and water
conductive of electricity
binary acid
acid that contains only 2 different elements
composed of hydrogen and more-electronegative element
binary acid nomenclature
begins with “hydro-“
contains root of name of second element
ends with “-ic”
oxyacid
acid that contains hydrogen, oxygen, and a 3rd element (usually a nonmetal)
oxyacid nomenclature
usually based on anion in compound
ternary acid
acid that contains 3 different elements
properties of bases
taste bitter
able to change color of acid-base indicators
feels slippery when in dilute aqueous solutions
reactive with acids to produce salts and water
conductive of electricity
Arrhenius acid
chemical compound that increases concentration of hydrogen (or hydronium) ions in aqueous solution
hydronium ion formula
H3O1+
Arrhenius base
chemical compound that increases concentration of hydroxide ions in aqueous solution
hydroxide ion formula
OH1-
strong acid
acid which ionizes completely in aqueous solution
acid which is strong electrolyte
relationship between strength of acid and strength of electrolyte
possitive
both depend on degree of ionization
weak acid
acid that does not ionize completely in aqueous solution
acid which is weak electrolyte
contents of aqueous solution of weak acid
hydronium ions
anions
dissolved acid molecules
alkaline
solution produced when a base completely dissociates in water to yield aqueous hydroxide ions
relationship between strength of base and strength of electrolyte
direct
both depend on degree of dissociation
strong base
base which dissociates completely in aqueous solution
base which is strong electrolyte
weak base
base which does not dissociate completely in aqueous solution
base which is weak electrolyte
Brønsted-Lowry acid
molecule or ion that is a proton donor
Brønsted-Lowry base
molecule or ion that is a proton acceptor
Brønsted-Lowry acid-base reaction
reaction where protons are transferred from acid to base
monoprotic acid
acid that can donate only 1 proton per molecule
polyprotic acid
acid that can donate more than 1 proton per molecule
diprotic acid
acid that can donate 2 protons per molecule
triprotic acid
acid that can donate 3 protons per molecule
Lewis acid
atom, ion, or molecule that accepts an electron pair to form a covalent bond
Lewis base
atom, ion, or molecule that donates an electron pair to form a covalent bond
Lewis acid-base reaction
formation of 1 or more covalent bonds between electron pair donor and electron pair acceptor
conjugate base
species that remains after Brønsted-Lowry acid has donates a proton
conjugate acid
species that remains after Brønsted-Lowry base accepts a proton
deciding factor of extent of Brønsted-Lowry acid-base reaction
relative strengths of acids and bases involved
relationship between strength of acid and strength of conjugate base
inverse
relationship between strength of base and strength of conjugate acid
inverse
product of proton-transfer reactions
weaker acid and weaker base
amphoteric compound
compound that can react as either acid or base
compound containing hydroxyl group
compound covalently bonded to -OH group
can be acidic or amphoteric
neutralization
chemical reaction wherein acids and bases react quantitatively with each other
produces no excess of hydrogen or hydroxide ions present in solution when in water
salt
ionic compound composed of cation from base and anion from acid
neutralization reaction between acid and hydroxide base

neutralization reaction between acid and carbonate base

neutralization reaction between acid and metal

hydrofluoric acid formula
HF
hydrochloric acid formula
HCl
hydrobromic acid formula
HBr
hydrosulfuric acid formula
H2S
acetic acid formula
CH3COOH
carbonic acid formula
H2CO3
chloric acid formula
HClO3
nitric acid formula
HNO3
phosphoric acid formula
H3PO4
sulfuric acid formula
H2SO4