Chemistry 1020 Exam 3.... acids-
bases-buffers
Strong Acids - answerHCl hydrochloric acid
HBr hydrobromic acid
HI hydroiodic acid
HNO3 nitric acid
HClO4 perchloric acid
H2SO4 sulfuric acid
HBr, HCl, HI, HNO3, HClO4, H2SO4 - answertype the strong acids
Strong Bases - answerLiOH not all that common
NaOH
KOH
Ca(OH)2 limited solubility
Sr(OH)2 limited solubility
Ba(OH)2 limited solubility
LiOH, NaOH, KOH, Ca(OH)2, Sr(OH)2, Ba(OH)2 - answertype the strong bases
As Kb gets larger... - answer[OH-] increases and [H3O+] decreases
the larger the Kb.. - answerthe stronger the base
(BL) Bases are... - answerproton (H+) acceptors
(BL) Acids are.. - answerProton (H+) donors
(AR) Bases are... - answera substance that produces OH- on dissolution in water.
MOH(aq) --> M+(aq) + OH-(aq)
(AR) Acids are... - answera substance that produces H+ on dissolution in water.
HA(aq) -->H+(aq) + A-(aq)
HCl(aq) -->H+(aq) + Cl-(aq)
Polyprotic Acid - answera substance which can donate more than one proton.
H2SO4(aq) --> 2H+(aq) + SO42-(aq)
Polyprotic Base - answera substance which can accept more than one proton.
C2O42-(aq) + 2H+(aq) --> H2C2O4(aq)
hydronium ion - answerH3O+. Product of dissociation of an acid written as H+ or H3O+
, conjugate acid base pairs - answerChemical species whose formulas differ by only one
proton are said to be
conjugate acid-base pairs.
A conjugate acid is a base plus H+.
A conjugate base is an acid minus H+.
the stronger the acid... - answerThe larger Ka.
The further the equilibrium lies toward products.
The higher the concentration of H3O+ at equilibrium.
weak acids - answerAs Ka increases, the [H3O+] increases and the pH decreases for
the same initial acid concentration.
The [H3O+] for a weak acid is less than the concentration of the original acid.
pKa= - answer-logKa
small pKa=______the acid=_______ka - answerstronger, larger
two types of weak bases... - answerammonia and amine, also NH3
finding pH given molarity and Ka or Kb - answer(x^2/given M )=ka or kb.
solve for x. take -log of x (which is M) for pH
PH= - answer-log[H+ or M] or [OH- or M]
% ionization= - answerx=sqrt(given M*ka)...then [x]/[given M] *100
Molarity= - answer10^-PH
Electronegativity - answerincreases across -->, and decreases down.
the weaker the H---A bond, the ___ the acid - answerstronger
bond strength decreases as the size of A _______ - answerincreases
when OH bonds to a nonmetal= acid or base? - answeracid
when OH bonds to a metal?= acid of base? - answerbases
as # O's increases... acidity - answerincreases
the stronger the acid or base, the ______ its conjugate - answerweaker
an aqueous solution containing only NaF is.. - answerBASIC. because F is a weak acid
and it's conjugate is a weak base.
bases-buffers
Strong Acids - answerHCl hydrochloric acid
HBr hydrobromic acid
HI hydroiodic acid
HNO3 nitric acid
HClO4 perchloric acid
H2SO4 sulfuric acid
HBr, HCl, HI, HNO3, HClO4, H2SO4 - answertype the strong acids
Strong Bases - answerLiOH not all that common
NaOH
KOH
Ca(OH)2 limited solubility
Sr(OH)2 limited solubility
Ba(OH)2 limited solubility
LiOH, NaOH, KOH, Ca(OH)2, Sr(OH)2, Ba(OH)2 - answertype the strong bases
As Kb gets larger... - answer[OH-] increases and [H3O+] decreases
the larger the Kb.. - answerthe stronger the base
(BL) Bases are... - answerproton (H+) acceptors
(BL) Acids are.. - answerProton (H+) donors
(AR) Bases are... - answera substance that produces OH- on dissolution in water.
MOH(aq) --> M+(aq) + OH-(aq)
(AR) Acids are... - answera substance that produces H+ on dissolution in water.
HA(aq) -->H+(aq) + A-(aq)
HCl(aq) -->H+(aq) + Cl-(aq)
Polyprotic Acid - answera substance which can donate more than one proton.
H2SO4(aq) --> 2H+(aq) + SO42-(aq)
Polyprotic Base - answera substance which can accept more than one proton.
C2O42-(aq) + 2H+(aq) --> H2C2O4(aq)
hydronium ion - answerH3O+. Product of dissociation of an acid written as H+ or H3O+
, conjugate acid base pairs - answerChemical species whose formulas differ by only one
proton are said to be
conjugate acid-base pairs.
A conjugate acid is a base plus H+.
A conjugate base is an acid minus H+.
the stronger the acid... - answerThe larger Ka.
The further the equilibrium lies toward products.
The higher the concentration of H3O+ at equilibrium.
weak acids - answerAs Ka increases, the [H3O+] increases and the pH decreases for
the same initial acid concentration.
The [H3O+] for a weak acid is less than the concentration of the original acid.
pKa= - answer-logKa
small pKa=______the acid=_______ka - answerstronger, larger
two types of weak bases... - answerammonia and amine, also NH3
finding pH given molarity and Ka or Kb - answer(x^2/given M )=ka or kb.
solve for x. take -log of x (which is M) for pH
PH= - answer-log[H+ or M] or [OH- or M]
% ionization= - answerx=sqrt(given M*ka)...then [x]/[given M] *100
Molarity= - answer10^-PH
Electronegativity - answerincreases across -->, and decreases down.
the weaker the H---A bond, the ___ the acid - answerstronger
bond strength decreases as the size of A _______ - answerincreases
when OH bonds to a nonmetal= acid or base? - answeracid
when OH bonds to a metal?= acid of base? - answerbases
as # O's increases... acidity - answerincreases
the stronger the acid or base, the ______ its conjugate - answerweaker
an aqueous solution containing only NaF is.. - answerBASIC. because F is a weak acid
and it's conjugate is a weak base.
