Please select a Team.
Team 1
Team 2
Team 3
Team 4
Team 5
am
Te
am
Te
5
0%
4
0%
3
am
Te
am
Te
am
0%
2
0%
1
0%
Te
1.
2.
3.
4.
5.
A solution that is mildly acidic
would have a pH of approximately
0%
0%
12
0%
6.
0%
4.
0%
8.
2.
4.
6.
8.
12
2.
1.
2.
3.
4.
5.
A solution that is most strongly acidic
would have a pH of approximately
0%
0%
12
0%
6.
0%
4.
0%
8.
2.
4.
6.
8.
12
2.
1.
2.
3.
4.
5.
A solution that is most strongly basic
would have a pH of approximately
0%
0%
12
0%
6.
0%
4.
0%
8.
2.
4.
6.
8.
12
2.
1.
2.
3.
4.
5.
A solution that is weakly basic
would have a pH of approximately
0%
0%
12
0%
6.
0%
4.
0%
8.
2.
4.
6.
8.
12
2.
1.
2.
3.
4.
5.
The label on a bottle indicates that the
substance inside has a pH of 13. This tells you
that the substance is
1. neutral.
2. strongly acidic.
3. mildly basic.
4. strongly basic.
as
ic .
yb
ng
l
st
ro
ild
ly
m
ya
ng
l
st
ro
0%
ba
c id
ic .
tra
ne
u
0%
sic
.
0%
l.
0%
Team Scores
0
Team 1
0
0
0
0
Team 2
Team 3
Team 4
Team 5
The label on a bottle indicates that the
substance inside has a pH of 1. This tells you
that the substance is
1. neutral.
2. strongly acidic.
3. mildly basic.
4. strongly basic.
as
ic .
yb
ng
l
st
ro
ild
ly
m
ya
ng
l
st
ro
0%
ba
c id
ic .
tra
ne
u
0%
sic
.
0%
l.
0%
When a solution of an acid reacts with a
solution of a base, hydronium ions react with
hydroxide ions to form
1. a salt.
2. a stronger acid.
3. a weaker base.
4. water.
rb
ke
ea
aw
w
.
ac
id
as
tro
ng
er
as
0%
at
er
.
0%
as
e.
0%
alt
.
0%
When a solution of an acid reacts with a
solution of a base, if the water is evaporated
____ will form.
1. a salt.
2. a stronger acid.
3. a weaker base.
4. water.
rb
ke
ea
aw
w
.
ac
id
as
tro
ng
er
as
0%
at
er
.
0%
as
e.
0%
alt
.
0%
Which is an example of a
neutralization reaction?
1. NaOH  Na++ OH2. HNO3 + H2O  H3O+ + NO33. 2H2 + O2  2H2O
4. H3O+ + OH-  2H2O
0%
0%
&#
17
4;
2H
+
2O
OH
-&
#1
74
;2
H2
O
H3
O+
+O
2
H3
O.
..
0%
2H
2
&#
17
4;
+H
2O
HN
O3
Na
O
H
&#
17
4;
N
a+
+O
H-
0%
Ions that do not change during a
chemical reaction are called
spectator ions.
hydroxide ions.
monatomic ions.
hydronium ions.
0%
ns
.
m
ni
u
hy
dr
o
m
on
a
to
m
ic
io
io
on
s.
hy
dr
o
xid
ei
io
to
r
ct
a
0%
ns
.
0%
ns
.
0%
sp
e
1.
2.
3.
4.
Team Scores
0
Team 1
0
0
0
0
Team 2
Team 3
Team 4
Team 5
Which are the spectator ions in the following
reaction?
H3O+ + Br- + K+ + OH–  K+ + Br- + 2H2O
1. H3O+ and K+
2. Br- and OH3. Br- and K+
4. H3O+ and OH-
OH
-
0%
d
an
H3
O+
nd
Br
-a
OH
Br
-a
nd
d
an
H3
O+
0%
K+
0%
K+
0%
Which equation shows a strong
acid dissolving in water?
4.
0%
.. .
74
;+
H3
O+
74
;
17
4;
N
0%
..
0%
a.
..
0%
74
;..
.
3.
2.
&#
1
1.
A base forms a greater concentration
of which ions in solution than an acid?
oxygen
hydroxide
hydronium
hydrogen
m
ni
u
hy
dr
o
xid
hy
dr
o
0%
ge
n
0%
hy
dr
o
0%
e
0%
ox
yg
en
1.
2.
3.
4.
Which phrase is not true about
strong acids?
conduct electricity well
ionize completely in water
turn blue litmus paper red
form OH- ions in solution
fo
rm
n
0%
tio
so
lu
OH
-
io
ns
i
us
p
it m
el
bl
u
tu
rn
n
ap
er
wa
t
in
et
el
y
pl
co
m
0%
re
d
l
el
yw
ici
t
io
ni
ze
du
ct
el
ec
tr
0%
er
0%
co
n
1.
2.
3.
4.
Which phrase is not true about
strong bases?
are metal hydroxides
have pH ranges from 8 to 14
dissociate in water
poor electricity conductor
r
yc
on
el
ec
tri
c it
te
po
or
di
ss
oc
ia
0%
du
ct
o
w
in
m
fro
ge
s
ra
n
H
ep
ha
v
at
..
8
yd
ro
xid
al
h
et
m
0%
er
0%
es
0%
ar
e
1.
2.
3.
4.
Team Scores
0
Team 1
0
0
0
0
Team 2
Team 3
Team 4
Team 5
What does the pH of a solution
measure?
concentration of H3O+ ions
molarity of the solute
concentration of metal ions
solubility of the solute
so
l
te
ft
he
ub
i
n
tio
ce
nt
ra
co
n
0%
so
lu
io
ns
of
m
et
al
so
l
ft
he
r it
yo
m
ol
a
0%
lit
yo
ns
io
H3
O+
of
n
tio
tra
ce
n
0%
ut
e
0%
co
n
1.
2.
3.
4.
Which solution is the most acidic?
apple juice, pH = 3
pure water, pH = 7
hand soap solution, pH = 10
drain cleaner solution, pH = 14
0%
p.
..
10
H
n,
tio
ol
u
rs
ne
so
l
ut
io
n,
pH
er
,p
at
w
pu
re
0%
=
=
=3
H
ce
,p
ej
ui
0%
7
0%
ap
pl
1.
2.
3.
4.
Which solution is the least acidic?
0%
rs
ol
u
tio
n,
n,
pH
ut
io
an
e
so
l
p
in
c le
so
a
d
ha
n
p.
..
10
H
er
,p
at
w
pu
re
0%
=
=
=3
H
ce
,p
ej
ui
ap
pl
0%
7
0%
dr
a
1. apple juice, pH = 3
2. pure water, pH = 7
3. hand soap solution,
pH = 10
4. drain cleaner
solution, pH = 14
Which solution is the most basic?
0%
rs
ol
u
tio
n,
n,
pH
ut
io
an
e
so
l
p
in
c le
so
a
d
ha
n
p.
..
10
H
er
,p
at
w
pu
re
0%
=
=
=3
H
ce
,p
ej
ui
ap
pl
0%
7
0%
dr
a
1. apple juice, pH = 3
2. pure water, pH = 7
3. hand soap solution,
pH = 10
4. drain cleaner
solution, pH = 14
A 0.00001 M solution of the strong
acid HCl has a pH of
2
3
4
5
0%
5
0%
4
0%
3
0%
2
1.
2.
3.
4.
Team Scores
0
Team 1
0
0
0
0
Team 2
Team 3
Team 4
Team 5
A 0.001 M solution of the strong
acid HCl has a pH of
2
3
4
5
0%
5
0%
4
0%
3
0%
2
1.
2.
3.
4.
What is the molarity of H3O+ in a
strong acid solution with a pH of 2?
2M
2 x 10–1 M
1 x 10–2 M
1 x 10–4 M
M
0%
#8
21
1;
4
#1
80
;1
0&
#8
21
1;
2
1&
#1
80
;1
0&
#8
21
1;
1
M
0%
M
0%
1&
#1
80
;1
0&
2M
0%
2&
1.
2.
3.
4.
A 0.1 M solution of the strong acid
NaOH has a pH of
2
13
14
1
0%
1
0%
14
0%
13
0%
2
1.
2.
3.
4.
A 0.00001 M solution of the strong acid
HCl. What is the pOH of this solution?
3
9
7
5
0%
5
0%
7
0%
9
0%
3
1.
2.
3.
4.
What is the molarity of [OH]- in a
strong base solution with a pOH of 2?
2M
1 x 10–12 M
1 x 10–2 M
1 x 10–4 M
0%
0%
0%
&#
18
0;
2M
10
&#
82
11
1&
;1
#1
2
80
M
;1
0&
#8
21
1&
1;
#1
2
80
M
;1
0&
#8
21
1;
4
M
0%
1
1.
2.
3.
4.
Team Scores
0
Team 1
0
0
0
0
Team 2
Team 3
Team 4
Team 5
Choose the correct equation for
the reaction of HBr with Ca(OH)2.
1. 2H+ + 2Br– + Ca2+ + 2OH–  4H2O + BrCa
2. HBr + Ca(OH)2  CaH + Br(OH)2
3. 2H+ + 2Br– + Ca2+ + 2OH– 4H2O+2Br– +Ca2+
0%
Ca
2+
.
+
&#
82
11
;
2H
++
2B
r
&
OH
)2
Ca
(
+
HB
r
2H
++
2B
r
&#
82
11
;
+
#1
74
;C
a.
..
Ca
2+
.
.
0%
.
0%
Choose the correct equation for
the reaction of HNO3 with KOH.
1. H3O+ + NO3– + K+ + OH–  2H2O + K+ + NO3–
2. H3O+ + NO3– + K+ + OH–  2H2O + KNO3
3. HNO3 + KOH  HK + NO3OH
0%
74
;H
K.
.
K.
..
0%
1;
+
1;
+
K+
.
.
0%
Identify the salt that would form from the
neutralization reaction of HCl(aq) with LiOH(aq) .
LiCl
H2O
LiH
Li+
0%
Li+
0%
LiH
0%
H2
O
l
0%
LiC
1.
2.
3.
4.
Which acid and base would you
combine to form the salt Na2SO4?
H2SO4 and NaOH
H2SO4 and NaCl
NaOH and H2SO3
NaCl and H2SO3
0%
Na
C
la
nd
H2
SO
3
H2
SO
3
0%
an
d
H
Na
O
H2
SO
4
an
d
H
Na
O
an
d
0%
Na
Cl
0%
H2
SO
4
1.
2.
3.
4.
Which acid and base would you
combine to form the salt CaCl2?
HCl and NaOH
HCl and Ca(OH)2
NaCa and H2Cl
CaCl and HOH
0%
Ca
Cl
a
nd
H2
Cl
aa
Na
C
Ca
nd
HC
la
nd
(O
H)
OH
Na
nd
0%
HO
H
0%
2
0%
HC
la
1.
2.
3.
4.
Team Scores
0
Team 1
0
0
0
0
Team 2
Team 3
Team 4
Team 5
At the equivalence point of a strong
acid–strong base titration the pH is
0
7
10
14
0%
14
.
0%
10
.
0%
7.
0%
0
1.
2.
3.
4.
Bleach should never be mixed with a(n)
___________ because it would release a deadly
chlorine gas.
1. acid.
2. detergent.
3. water.
4. soap.
p.
0%
so
a
at
e
w
t.
er
ge
n
de
t
ac
id
0%
r.
0%
.
0%
Which statement is not true about
antacids?
pH
0%
an
ge
ch
nd
ea
bo
n
ir
ca
n
ac
h
re
pa
he
lp
0%
.
id
0%
ac
st
om
liz
e
ne
ut
ra
ar
e
ba
s
ic
su
bs
ta
n
ce
s
0%
ca
r..
1. are basic substances
2. neutralize stomach
acid
3. help repair bone
and cartilage
4. can change pH
What is the pH of a 0.01 M solution of
the strong acid HNO3 in water?
1
2
3
4
0%
4
0%
3
0%
2
0%
1
1.
2.
3.
4.
What is the pH of a 0.0001 M solution
of the strong acid HNO3 in water?
1
2
3
4
0%
4
0%
3
0%
2
0%
1
1.
2.
3.
4.
Team Scores
0
Team 1
0
0
0
0
Team 2
Team 3
Team 4
Team 5
The salt sodium sulfate, Na2SO4,
can be formed by a reaction
between
1. NaOH and HCl.
2. NaCl and H2O.
3. NaOH and H2SO4.
4. NaCl and NH3.
Na
C
la
nd
H2
SO
an
d
Na
O
H
la
Na
C
0%
4.
H2
O.
nd
HC
l
an
d
H
Na
O
0%
NH
3.
0%
.
0%
Solution A has a pH of 6. Solution B has a pH
of 8. What is true about these solutions?
Solution A has 10 times as many H+ ions as Solution B.
Solution A has 100 times as many H+ ions as Solution B.
Solution A has 1000 times as many H+ ions as Solution B.
Solution A has 0.10 times as many H+ ions as Solution B.
tim
e.
..
0%
0.
10
e.
..
0%
tim
00
0
00
t
im
..
es
t im
0%
es
. ..
0%
10
1.
2.
3.
4.
Solution A has a pH of 2. Solution B has a pH
of 5. What is true about these solutions?
Solution A has 10 times as many H+ ions as Solution B.
Solution A has 100 times as many H+ ions as Solution B.
Solution A has 1000 times as many H+ ions as Solution B.
Solution A has 0.10 times as many H+ ions as Solution B.
0%
.1
0
tim
e.
..
tim
e.
..
0%
s0
00
t
s1
10
00
..
es
im
0t
0%
im
es
. ..
0%
as
1
1.
2.
3.
4.
Acid rain is caused by:
1. cloud seeding.
2. silver iodide particles in
clouds.
3. by-products of the
combustion of fossil fuels.
4. carbon tetrachloride
0%
0%
rid
ch
lo
tra
te
n
of
th
e
co
m
si
. ..
n.
..
e
0%
rti
cle
pa
e
clo
ud
se
ed
i
ng
.
0%
If the hydroxide ion concentration of a solution is 1 x 10-10,
the hydronium ion concentration =________________.
Is this solution that is acidic, basic (alkaline), or neutral?
1. acidic
2. alkaline (basic)
3. neutral
l
as
ic )
alk
al
in
e
(b
ac
id
0%
ne
ut
ra
0%
ic
0%
Team Scores
0
Team 1
0
0
0
0
Team 2
Team 3
Team 4
Team 5
What is the best description for a
solution with a hydroxide-ion
concentration of 1 10-4M?
1. acidic
2. basic
3. neutral
tra
l
0%
ne
u
0%
ba
sic
ac
id
ic
0%
A 0.1 M solution of an acid that ionizes only
slightly in solution would be termed ____.
st
ro
ng
0%
an
d
d
te
di
lu
te
an
d
di
an
d
ng
st
ro
ce
nt
ra
k
ea
w
an
d
te
d
tra
ce
n
co
n
0%
we
ak
0%
lu
te
0%
co
n
1. concentrated and
weak
2. strong and dilute
3. dilute and weak
4. concentrated and
strong
The reaction
HCl + KOH  KCl + H2O
tio
ac
tio
re
ac
io
n
on
re
re
io
n
de
c
om
liz
at
ne
ut
ra
za
t
io
ni
0%
n
n
tio
ac
ct
re
a
is
sy
nt
he
s
0%
n
0%
io
n
0%
po
sit
i
1. synthesis reaction
2. ionization reaction
3. neutralization
reaction
4. decomposition
reaction
is a
FINAL Team Scores
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Team 1
0
0
0
0
Team 2
Team 3
Team 4
Team 5