chem 116 quiz 6 Flashcards
Arrhenius definition
acid is a substance that produces H+ ions in aqueous solution
Bronsted-Lowry definition
acid is a proton donor and becomes a conjugated base
Lew definition
acid is an electron pair acceptor (it has an empty orbit that can accept an electron pair)
strong acids
ionize 100%; also strong electrolytes
to show the ionization goes to completion, a (single-headed/double-headed) arrow is used b/w the reactants and products
single-headed
weak acid
ionizes less than 100%; classified as weak electrolytes
double-headed arrow is used to show
a reaction is reversible/some kind of equilibrium is involved
the stronger the acid, the (weaker/stronger) the conjugate base
weaker
if the forward reaction has a high tendency to occur, then the
reverse reaction has a low tendency to occur
? is unique to a particular acid/solvent combination
degree of ionization
? is a way to quantify acidity and basicity; ? is defined as ?
pH; pH is defined as -log[H+]
pH < 7
pH > 7
pH = 7
acidic
basic
neutral
pOH is very similar to the pH scale but is defined as ?; the relationship is ?
pOH = -log[OH-]
pH + pOH = 14
from pH, [H+] =
10^(-pH)
pKa =
-log(Ka)
the pKa of a weak acid is
high
the smaller the pKa, the (weaker/stronger) the acid
stronger
the smaller the Ka, the (weaker/stronger) the acid
weaker
the equilibrium constant for the ionization reaction of a weak acid
Ka
the point of exact neutralization can be visually determined through the use of
an indicator
an indicator is
a chemical that is sensitive to pH and is one color in a basic solution and another color in an acidic solution
the equivalence point allows you to calculate
the unknown concentration of the acid
one half the volume at the equivalence point allows you to calculate
the Ka (acid ionization constant)
Ka =
10^(-pKa)
