Chemistry Reference
In-Depth Information
9. [B. NH
3
]—An Arrhenius base must contain the hydroxide (OH
-
) ion.
10. [B. a proton donor]—HF donates a proton to become F
-
.
Lesson 9-5 Review
1. [A. K
b
= 1.0 × 10
-2
]—The strongest base will have the highest value for K
b
.
Remember that the exponents are all negative, so the largest negative
exponent shows the smallest value.
2. [D. K
a
= 1.0 × 10
-2
]—The strongest acid will have the highest value for K
a
.
3. [A. K
b
= 1.0 × 10
-6
]—Remember that the weakest base will have the
strongest conjugate acid, so we look for the lowest value for K
b
.
Lesson 9-6 Review
1.
[1.0 L]—The sulfuric acid (H
2
SO
4
) releases 2 moles of H
+
per mole of acid,
so multiply the molarity of the acid by 2.
Given: M
a
= 6.0 M; V
b
= 2.0 L; M
b
= 3.0M
Find: V
a
V
b
M
b
M
a
(2.0 L)(3.0 M)
(6.0 M)
V
a
=
=
= 1.0 L
2.
[1.0 M]—Work shown following.
Given: V
a
= 450 ml; V
b
= 150 ml; M
b
= 3.0 M
Find: M
a
V
b
M
b
V
a
(150 ml)(3.0 M)
(450 ml)
M
a
=
=
= 1.0 M
3.
[4.0 M]—The sulfuric acid (H
2
SO
4
) releases 2 moles of H
+
per mole of acid,
so multiply the molarity of the acid by 2.
Given: V
a
= 25 ml; M
a
= 4.0 M; V
b
= 25 ml
Find: M
b
V
a
M
a
V
b
(25 ml)(4.0 M)
(25 ml)
M
b
=
=
= 4.0 M
4.
[0.67 M]—Now, the Ca(OH)
2
will release 2 moles of OH
-
per mole of base.
When we find the molarity, we will divide by 2, because this base is twice as
effective as a base that only releases 1 mole of OH
-
per mole of base.
Given: V
a
= 1.0 L; M
a
= 4.0 M; V
b
= 3.0 L
Find: M
b
V
a
M
a
V
b
(1.0 L)(4.0 M)
(3.0 L)
M
b
=
=
= 1.33 M
1.33 M
2
= 0.67 M
Chapter 9 Examination
1.
[d. Brønsted-Lowry acid]—Proton donors are Brønsted-Lowry acids.
2.
[f. Lewis base]—Remember that they can neutralize H
+
ions.
3.
[h. Arrhenius base]—Each OH
-
can neutralize an H
+
ion.
4.
[c. indicator]—Litmus paper and phenolphthalein are examples of
indicators.
