THIS
IS
The correct equilibrium
expression for the
2
hydrolysis of CO3 ¯
A 200
K = ( [HCO3¯] [OH¯] ) /
2
[CO3 ¯]
A 200
H2PO4¯ + HBO32¯ ↔ HPO42¯ + H2BO3¯
The equilibrium constant for the reaction
represented by the equation above is greater than
1.0. Which of the following gives the correct
relative strengths of the acids and bases in the
reaction?
Acids
Bases
a.
H2PO4¯ > H2BO3¯ and HBO32¯ > HPO42¯
b.
H2BO3¯ > H2PO4¯ and HBO32¯ > HPO42¯
c.
H2PO4¯ > H2BO3¯ and HPO42¯ > HBO32¯
d.
H2BO3¯ > H2PO4¯ and HPO42¯ > HBO32¯
A 300
A
A 300
Which of the following
salts are basic?
Na2CO3, FeCl3, KNO3,
NH4C2H3O2, ZnSO4,
Ba(NO3)2, RbF
A 400
Na2CO3 and RbF
A 400
A solution of calcium
hypochlorite, a common additive
to swimming-pool water, is
a. basic because of the
hydrolysis of the OCl¯ ion
b. basic because Ca(OH)2 is a
weak and insoluble base
c. acidic because of the
hydrolysis of the Ca2+ ions
d. acidic because the acid HOCl
is formed
A 500
A
A 500
Consider the reaction
HNO2(aq) + H2O(l)
+
–
→ H3O (aq) + NO2
(aq). Which species is
a conjugate base?
B 100
NO2
-
B 100
The pH of a
solution at 25°C
–
in which [OH ] =
3.9 x 10–5 M is:
B 200
9.59
B 200
Calculate the
pOH of a 4.9
M solution of
HCl.
B 300
14.69
B 300
For weak acid, HX,
Ka = 6.9 x 10–6.
Calculate the pH of a
0.13 M solution of
HX.
B 400
3.02
B 400
Calculate the
pOH of a 0.12 M
solution of acetic
acid
–5
(Ka = 1.8 x 10 ).
B 500
11.17
B 500
What concentration of
acetic acid (Ka = 1.80 x
10–5) has the same pH as
–3
that of 5.33 x 10 M
HCl?
C 100
1.58M
C 100
Saccharin is a monoprotic
acid. If the pH of a 4.41 x10–3
M solution of this acid is
2.53, what is the Ka of
saccharin?
C 200
6.0 x
-3
10
C 200
A monoprotic weak acid
when dissolved in water is
0.75% dissociated and
produces a solution with a
pH of 3.11. Calculate the
Ka of the acid.
C 300
5.9 x
-6
10
C 300
Calculate the pH
of a 0.059 M
solution of
Ca(OH)2.
C 400
13.07
C 400
The pH of a 0.150 M
solution of a weak
base is 10.98.
Calculate the pH of a
0.0603 M solution of
the base.
C 400
11.28
C 500
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