Chemistry Reference
In-Depth Information
Lesson 9-3 Review
1. [phosphoric acid]—This is a ternary acid, and the PO
4
3-
is the phosphate ion,
so “ate” becomes “ic.”
2. [hydrobromic acid]—This is a binary acid, so we add the prefix of “hydro-”
and the ending of “ide” becomes “ic.”
3. [sulfuric acid]—This is a ternary acid, and the SO
4
2-
is the sulfate ion, so
“ate” becomes “ic.”
4. [hypochlorous acid]—This is a ternary acid that contains chlorine, and the
least number of oxygen atoms per formula unit.
5. [nitrous acid]—This is a ternary acid, and the NO
2
-
is the nitrite ion, so the
“ite” becomes “ous.”
6. [chloric acid]—This is a ternary acid that contains chlorine. The ClO
3
-
is the
chlorate ion, so “ate” becomes “ic.”
7. [HF]—The prefix of “hydro-” tells us that it is a binary compound
beginning with hydrogen. The “fluoric” must be derived from “fluoride.”
8. [HClO
2
]—The acid doesn't start with “hydro-” so it must be a ternary acid.
The “chloro” tells us that it contains chlorine. The ending of “ous” tells us
that the polyatomic ion must end in “ite,” like the chlorite ion, ClO
2
-
.
9. [H
2
SO
3
]—The name doesn't start with “hydro-,” so it must be a ternary acid,
and it must contain a polyatomic ion. The ending of “ous” means that the
polyatomic ion must end in “ite,” like sulfite, SO
3
2-
.
10. [HNO
3
]—The name doesn't start with “hydro-,” so it must be a ternary acid,
and it must contain a polyatomic ion. The ending of “ic” means that the
polyatomic ion must end in “ate,” like nitrate, NO
3
-
.
Lesson 9-4 Review
1.
[Brønsted-Lowry]—This definition is slightly broader than the Arrhenius
definition, as it isn't limited to aqueous solutions.
2.
[amphoteric]—Water and ammonia are common examples.
3.
[conjugate]—OH
-
is the conjugate base of water.
4.
We simply remove H
+
from each of the formulas.
A. [I
-
]
B. [H
2
PO
4
-
]
C. [NH
2
-
]
D. [OH
-
]
5.
We add H
+
to each of the formulas.
A. [H
2
O]
B. [HCl]
C. [NH
4
+
]
D. [H
3
O
+
]
6.
[D. HCl and H
3
O
+
]—Brønsted-Lowry acids are proton donors.
7.
[C. OH
-
and NH
3
]—Brønsted-Lowry bases are proton acceptors.
8.
[A. HF and F
-
]—Conjugate acid-base pairs differ from each other by a
single proton.
