Acids, Bases, and pH
Practice Test
1.
In general, electronegativity ___________ atomic number within a period.
a.
remains constant with
b.
is inversely proportional to
c.
decreases with
d.
increases with
2.
A solute __________________ of the solvent.
a.
lowers the boiling point
b.
raises the freezing point
c.
raises the boiling point
d.
does not affect
3.
Oxides of this element are usually involved in producing acid rain.
a.
sodium
b.
bromine
c.
boron
d.
sulfur
4.
A pH 13 solution is ______________ times more basic than a pH 9 solution.
a.
10 000
b.
1000
c.
100
d.
10
5.
Hard water contains significant concentrations of these.
a.
iron atoms
b.
chloride ions
c.
calcium and magnesium ions
d.
sodium ions
6.
At STP, one molar volume is __________.
a.
10.0 L
b.
32.0 L
c.
6.02 × 10
23
L
d.
22.4 L
7.
Which of these formulas does NOT represent a strong acid?
a.
HI
b.
HBr
c.
HBrO
d.
H
2
SO
4
8.
The type of analysis based on the movements of a stationary phase and a mobile phase is called _____________.
a.
chromatography
b.
photography
c.
titration
d.
phase movement
9.
What will a nonmetallic anhydride produce in aqueous solution?
a.
base
b.
acid
c.
salt
d.
solid precipitate
10.
What element has the electron configuration [Ar]4s
2
3d
3
?
a.
arsenic
b.
nitrogen
c.
vanadium
d.
scandium
11.
a.
green
b.
violet
c.
blue
d.
red
12.
What is the molar mass of arsenic?
a.
74.9 g/mol
b.
33 kg/mol
c.
74.9 u/mol
d.
33 lb/mol
13.
The arrangement of electron pairs around the nitrogen atom in the ammonia molecule, NH
3
, is best described as _______________.
a.
linear
b.
tetrahedral
c.
pyramidal
d.
square planar
14.
The light emitted by the gas in a neon sign is _________________.
a.
an incandescent light
b.
a filament
c.
an electron
d.
an emission spectrum
15.
Atoms that share electrons form __________ bonds.
a.
quartets
b.
covalent
c.
ionic
d.
quantitative
16.
According to the equation 2HBr + Na
2
CO
3
NaBr + H
2
O + CO
2
, what volume of CO
2
at 1.230 atm and 325 K is produced by 50.0 g of HBr reacting with an excess of Na
2
CO
3
?
a.
1.52 L
b.
22.4 L
c.
50.0 L
d.
6.70 L
17.
How many moles of chlorine are in 100 g chlorine (Cl)?
a.
64.6
b.
2.82
c.
100
d.
0.355
18.
The atoms in the water molecule are linked by ___________ bonds.
a.
triple
b.
pure covalent
c.
ionic
d.
polar covalent
19.
The number of valence electrons in a sulfur atom is __________.
a.
eight
b.
six
c.
two
d.
four
20.
The water molecule is polar partly because of its _____________.
a.
geometry
b.
weight
c.
volume
d.
mass
