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
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...
1.True or false
A. All compounds that contain
hydrogen are acids..
B. A solution with a pH of 5 has
10 times higher [H+] than a
Solution with a pH of 6.
C. SO3 in the
atmosphere is one cause of acid rain.
D. Agricultural chemicals are the
only cause of water pollution.
E. One function of an auto
catalytic converter is to convert CO2 to CO
F. The major elements in...
A. Which of the following can behave as Bronsted-Lowry bases in
aqueous solution?
NO3-
H3PO4
NH4+
HClO
None of the Above
B. Which of the following can behave as Bronsted-Lowry bases in
aqueous solution?
NH4+
NH3
Ca(OH)2
Br-
None of the Above
C. Which of the following can behave as Bronsted-Lowry bases in
aqueous solution?
HCO3-
NaOH
KOH
HF
None of the Above
* please help me I am really struggling with this concept. I
fully cannot seem to grasp...
1) Which of the following can behave as Bronsted-Lowry bases in
aqueous solution?
HNO2
H2SO3
Ca2+
I-
None of the Above
2) Which of the following can behave as Bronsted-Lowry bases in
aqueous solution?
Ba(OH)2
KOH
CN-
NH3
None of the Above
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
Ive leraned that there are three definitions of Acid and
Base.
Arrhenius, Bronsted-Lowry, and Lewis.
Why do we learn all these three?
Why can't I just use only one concept?
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
Put a circle around the Lewis Acids and a Box around
the Lewis Bases:
Ca2+
S2-
OH-
Fe3+
I-
pH
pOH
[H+], M
[OH-], M
Is it acidic, basic or a neutral soln?
2.
2.6
3.
3.4
4.
3.2 x 10-9
5.
4.7 x 10-3
6.
1 x 10-7