CHM 112
Chapter 15 Worksheet: Acids and Bases
Name: _________________________
The appropriate Ka or Kb values can be found in your textbook.
Q1.
Q2.
Q3.
What are the conjugate bases of the following acids?
a) HIO3
___IO3-______
b) NH4+
___ ________
c) H2PO4−
_____HPO42-_____
d) HC7H5O2
____ ____
What are the conjugate acids for each of the bases?
a) CN− _____HCN_______
b) C6H5COO− _____ ____
c) C2H5NH2 _____C2H5NH3+___
d) BrO− _____ ______
Identify the Bronsted-Lowry acid, the Bronsted–Lowry base, the conjugate base and the conjugate acid in the following
reactions.
a) NH4+ + CNNH3 + HCN
Acid
base
c.base c.acid
b) HNO3+ N2H4
NO3- + N2H5+
c) HCO3- + H2O
CO3 2- + H3O+
Acid
base
OH– + HS-
d) S2- + H2O
e) HCH2O+ PO43Acid
c.base c.acid
base
f) HIO3 + HC2O4-
CH2O- + HPO42c.base
c.acid
IO3- + H2C2O4
Q4.
Fill in the missing items in the following Table:
Acid
Base
↔
Conjugate Acid
(A)
H2O
O2−
↔
OH-
(B)
CH3COOH
↔
H3O+
CH3COO-
(C)
H2O
↔
HNO2
OH−
↔
HF
CO32−
F−
(D)
Q5.
(A)
Fill in the missing information in the following table:
[H+]
[OH−]
pH
pOH
Acid, Base or Neutral
0.0017
5.9 × 10-12
2.77
11.23
acidic
3.76
basic
(B)
(C)
(D)
Conjugate Base
0.0068 M
2.0 × 10-7
5.0 × 10-8
6.70
Q6.
Calculate the pH of the following strong acid or strong base solutions.
a) 0.0065 M HNO3
pH = 2.19
b) 0.0020 M NaOH
c) 0.837 g Ba(OH)2 in 1.00 L solution
pH = 11.990
Q7.
What is the pH of a solution of 0.50 M acetic acid?
pH = 2.54
Q8.
What is the pH of a 0.010 M solution of lactic acid?
pH = 2.96
Q9.
A 0.20 M solution of a weak acid (HA) has a pH of 3.22.
What is the percent ionization of this acid? What is the Ka and pKa of this acid?
0.30% ionization
Ka = 1.8 × 10-6
pKa = 5.74
Q10.
Codeine (used as a cough suppressant), is a weak base with a pKb of 5.80. What is the pH of a 0.020 M solution of
Codeine?
pH = 10.25
Q11. Hydroxylamine is a weak base. A 0.15 M solution of hydroxylamine has a pH of 10.11. What is the Kb for this base?
Kb = 1.1 × 10-7
Q12.
Draw the Lewis structures for HNO3 and HNO2 and explain which acid is stronger and why.
.
Q13.
Why is the Oxide ion O2- able to function as a Lewis base but not as a Lewis Acid?
O2- already has a full octet, so it can’t accept any more electron pairs (not a Lewis acid), but it can certainly
donate a pair (Lewis base).
Q14.
Write the hydrolysis reactions that will occur when then each of the following salts is added to water:
(Don’t forget to remove the spectator ions.) Predict whether each solution will be acidic, basic, or neutral in each case.
NH4+ + H2O → NH3 + H3O+
(A) NH4Br
acidic
(B) Na2CO3
(C) KClO4
All spectator ions: neutral
(D) NaC2H3O2
(E) CH3CH2NH3Cl
Q15.
CH3CH2NH3+ + H2O → CH3CH2NH2 + H3O+
acidic
Which is a stronger Bronsted-Lowry base, OH͞͞ or HS͞ ? Explain why.
.
Q 17. Rank from most acidic to most basic:
NaCN
__ HNO3___
Most acidic
KOH
KF
___ HCN ___
HCN
____ KF ____
HNO3
___NaCN___
___ KOH___
most basic
Q18. Fill in the missing items in the following Table: Draw the Lewis Structure for all species and show which electrons are
involved in the Lewis acid/base chemistry.
Lewis acid
Lewis Base
↔
(A)
HNO2(aq)
OH−(aq)
↔
(B)
H+(aq)
H2O(l)
↔
(C)
Zn2+
4 NH3
↔
(4 of these)
Q19.
Calculate the pH of a 0.10 M solution of NH4NO3.
pH = 5.12
Q20.
Calculate the pH of a 0.025 M solution of Na2HPO4.
pH = 9.80
Lewis Acid-Base Product
I
Zn((NH3)42+
Lewis Acid-Base Product II