acids generally release H2 gas when they react with
acids to produce salts and water
bases react with
conduct electric current
aqueous solutions of bases
Which is a binary acid?
Which is chlorous acid?
an acid ending with the suffix -ic produces anion with the
the traditional definition of acids is based on the observations of
they increase the concentration of hydroxide ions in aqueous solution
Which statement about Arrhenius acids is false?
Which is a strong acid?
Which is a diprotic acid?
a Bronsted-Lowry acid is a(n)
a species that remains when an acid has lost a proton is a
How many conjugate acid-base pairs participate in a Bronsted-Lowry acid-base reaction?
Whose theory of acids and bases do conjugate acids and bases belong to?
the 2 members of a conjugate acid-base pair differ by a
in the reaction represented by the equation CH3COOH + H2O --> <-- H3O + CH3COO, the conjugate acid of CH3COO is
in the reaction represented by the equation NH3 + H2O --> <-- NH4 + OH, the conjugate base of water is
the conjugate of a strong acid is a
the conjugate of a weak acid is a
in the equation HI + H2O --> H3O + I, HI is a strong acid and I is a
in the equation CH3COOH + H2O --> <-- H3O + CH3COO, H2O is a weak base and H3O is a
a species that can react as either an acid or a base is a(n)
Which is amphoteric?
in the reaction represented by the equation H3PO4 + H2O --> <-- H3O + H2PO4, the molecule H2O acts as a(n)
NaOH and RbOH
which are strong bases?
an acid that contains only 2 different elements
an acid that is a compound of hydrogen, oxygen, and a 3rd element (usually a nonmetal)
a chemical compound that increases the concentration of hydrogen ions (H+) in aq. solution
a substance that increases the concentration of hydroxide ions (OH-) in aq. solution
an acid that ionizes completely in aq. solution
an acid that releases few H+ in aq. solution
a proton donor
a proton acceptor
Bronsted-Lowry acid-base reaction
protons are transferred from one reactant (the acid) to another (the base)
an acid that can donate only 1 proton (H+) per molecule
an acid that can donate more than 1 proton (H+) per molecule
an atom, ion, or molecule that accepts an electron pair to form a covalent bond
an atom, ion, or molecule that donates an electron pair to form a covalent bond
Lewis acid-base reaction
the formation of 1 or more covalent bonds b/w an electron-pair donor and an electron-pair acceptor
the species that is formed when a Bronsted-Lowry base gains a proton
acidic and basic compounds react, neutralizing the other
the reaction of hydronium ions and OH- to form water molecules
an ionic compound composed of a cation from a base an an anion from an acid
self-ionization of water
2 water molecules produce a hydronium ion and a OH- by a transfer of a proton
the negative of the common logarithm of the hydronium ion concentration, [H3O+]
the negative of the common logarithm of the hydroxide ion concentration, [OH-]
compounds whose colors are sensitive to pH
the pH range over which an indicator changes color
determines the pH of a solution by measuring the voltage b/w 2 electrodes that are placed in the solution
using a solution of known concentration to determine the concentration of an unknown solution
the point when there are equal molar amounts of acid and base
the point in a titration at which an indicator changes color
solution of known concentration
a highly purified solid compound used to check the concentration of the known solution