Which are the Brønsted–Lowry acids in the following
equilibrium?Which are the Brønsted–Lowry acids in the following
equilibrium? CH3COOH(aq) + NaOH(l)⇌ NaCH3COO(aq) +
H2O(l)CH3COOH(aq) + NaOH(l)⇌ NaCH3COO(aq) + H2O(l)
Select one:
a. CH3COO–and OH––
b. H2O and OH–
c. H2O, CH3COOH, and OH–
d. CH3COO–and CH3COOH
e. H2O and CH3COOH
Discuss in extensive detail the Brønsted-Lowry model of acids
and bases including equations for the - a. The definition of
Brønsted-Lowry acids and bases b. Application of this model to
non-aqueous solvents and gas phase reactions c. Relation between
acid-strength and solvents d. Factors that influence the strengths
of acids and bases
3.Write the formula for the conjugate acid of each of
the following bases.
Base:
Conjugate acid:
HS−
HCO3−
CO32−
HPO42−
SO42−
Acid
Conjugate base
(a) HNO2
(b)
H2SO4
(c) H2S
(d) HCN
(e) HCOOH
a. (3 pts) All Brønsted-Lowry acids contain the hydrogen ion, H+
. True False
b. (3 pts) You can use any acid/conjugate base pair in making a
buffer. True False
c. (3 pts) Concentration does not matter for acids/conjugate
bases in buffers. True False
What is the conjugate acid of each of the following bases? Write
the equilibrium reactions in aqueous solution for each base.
1) Se2-.
2) HPO42-.
3) ClO3-.
4) [Co(NH3)5(OH)]2+.
5) SeO4-.
pre lab questions:
1. Define “acid” according to the Bronsted-Lowry theory of acids
and bases.
2. Hypothesize what might occur to the sodium bicarbonate when
it reacts in Part B of this experiment. What will you see?
3. The NaI might undergo one of two different reactions when it
reacts with 18 M sulfuric acid in Part C of this experiment.
Describe what happens in both of these possibilities (in words or
with reaction equations)
4. Lookup the physical appearance...
which of these statementsis not true
All brondted-lowry acids contain hydrogen
All lewis bases are Bronsted-lawry bses
Some lewis avids contsin hydrogen
water is noth acid and base
All lweis acids are elctron acceptors
1-Common commercial
acids and bases are aqueous solutions with the following
properties: HCl, density 1.19 g/cm3 and 34% solute by
mass. Calculate the molality.
2-Common commercial
acids and bases are aqueous solutions with the following
properties: HCl, density 1.19 g/cm3 and 35% solute by
mass. Calculate the mole fraction.