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Which of the following is NOT a valid definition of an acid?
Which of the following is a Bronsted base?
One major difference between the Bronsted-Lowry and the Arrhenius
definitions of acids and bases is
which of the following?
The K
a for hypochlorous acid does not contain which of the
following terms?
If the K
a of sulfurous acid is 1.54 x 10-2, what is
the K
b of
its conjugate base?
What is the value of K
w at 333 K?
What is the K
a of a 0.320 M solution of nitrous acid? Nitrous
acid has a
pK
a of 3.34.
What is the pOH of a 0.350 M solution of Nitric Acid?
What is the pK
b of an acid with a K
a of 6.20
x
10-4?
If the pOH of a solution is 6, what is the pH?
Which of the following is true?
Which of the following has the most impact on the acidity of a halogen
acid, HX?
Which of the following contributes to an increase in pK
a for
an
oxyacid of the type
A(OH)nOm?
Which of the following is the weakest acid?
What is the [H+] in a 0.1 M solution of Nitric Acid into which
0.2 moles per liter of
HCl is dissolved?
What is the pH of a solution of 0.50 moles of nitric acid and 1.0 mole of
sulfuric acid dissolved into
2.0 L of water?
Why can we equate the [H+] and the [strong acid]?
Why is Ba(OH)2 not a strong base whereas other alkaline earth
metal hydroxides are?
What is the pH of a 0.520 M solution of NaOH?
What happens to the pH of a solution of NaOH when BaSO4 is added?
What is the pH of a 1.10 M solution of hydrazoic acid? HN3 has a
pK
a of
4.72.
What is the percent dissociation of a 0.010 M solution of acetic acid? The
K
a of acetic
acid is 1.76 x 10-5.
What is the pH of 2 L of a 1.0 M HF solution to which 42 g of NaF are added,
causing no net change
in volume? The K
a of HF is 6.6 x 10-4.
What is the pK
a of a monoprotic weak acid that gives a pH of
6.2
when you prepare a
0.56 M solution of that acid?
What is the pH of a 0.230 M solution of NH3? The
pK
b of
NH3 is 4.75.
How much pyridine (C5H5N) is needed to raise the pH
of 500 mL of
water by 2 units? The pK
a of the pyridinium ion is 5.25.
What is the pOH of a mixture of 5 g of Ba(OH)2 in 100 mL of
water given its
K
spis 5.0 x 10-3.
What is the pH of a 1.0 M solution of NaCl in water?
When a weak base dissolves in water to form a 1.0 M solution, it gives a pH
of 9.0. What is the
pK
a of its conjugate acid?
What is the pH of a 0.25 M solution of NaOAc (sodium acetate) in water if the
pK
a
of AcOH (acetic acid) is 4.75?
What is the pH of a 3.60 M solution of ammonium chloride
(NH4
+Cl) in water if the
pK
b of
ammonia is 4.75?
Which of the following is a characteristic of a polyprotic acid?
What is the pH of a 3.0 M solution of phosphoric acid in water?
pK
a1 is 2.12,
pK
a2 is 7.21, and pK
a3 is 12.67.
What is the pH of a 0.10 M solution of sodium hydrogensulfate? For
sulfuric acid,
pK
a1 is -2, pK
a2 is 1.92.
What condition must be satisfied to make a good buffer?
Which of the following is the Henderson-Hasselbalch equation?
What is the pH of an equimolar mixture of acetic acid and sodium acetate?
The K
a of
acetic acid is 1.76 x 10-5.
What is the pH of a solution of 5.00 g acetic acid, 7.00 g sodium acetate, and
2.00
g HCl in 200 mL of water?
If the pH of a solution you wish to control using a buffer is 8.0, which of
the following buffer
compositions would you prefer?
On a titration curve, at what point does the titrant exactly neutralize the
unknown?
How much HCl should be added to 500 mL of a 1.0 M NaOH solution achieve the
highest pH on a
titration curve?
Which of the following is required to measure the pH of the unknown
solution during a titration?
What is the pH at the equivalence point for a titration of a strong acid by
a strong base?
While performing the titration of a weak acid by a strong base, Annie Oaf
and Peter Fool became
discouraged when they reached a pH of 4 and noticed that it takes a
large amount of base to
change the pH significantly. They figured that they had "messed up" and needed
to start over. What
feature of the titration curve fooled them?
What will be the pH at the equivalence point for a weak base being titrated
with a strong acid?
What is the molecular weight of a weak acid solution (5.0 g in 100 mL) that
is neutralized by 50 mL of
a 1.0 M NaOH solution?
What volume of 1.016 M NaOH is required to completely titrate 45.00 mL of a
0.6532 M
H2SO4 solution?
What property of an indicator is essential for its function?
What is the difference between the equivalence point and the endpoint of a
titration?
