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
_______________
b) NH4+
_______________
c) H2PO4−
________________
d) HC7H5O2
________________
What are the conjugate acids for each of the bases?
a) CN− ____________________
b) C6H5COO− ________________
c) C2H5NH2 ________________
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
b) HNO3+ N2H4
NO3- + N2H5+
c) HCO3- + H2O
CO3 2- + H3O+
d) S2- + H2O
OH– + HS-
e) HCH2O+ PO43-
CH2O- + HPO42-
f) HIO3 + HC2O4-
IO3- + H2C2O4
Q4.
Fill in the missing items in the following Table:
Acid
Base
↔
(A)
H2O
O2−
↔
(B)
CH3COOH
(C)
F−
(D)
Q5.
(B)
(C)
(D)
↔
H3O+
↔
HNO2
Conjugate Base
OH−
CO32−
↔
Fill in the missing information in the following table:
[H+]
(A)
Conjugate Acid
[OH−]
pH
pOH
0.0017
0.0068 M
6.70
3.76
Acid, Base or Neutral
Q6.
Calculate the pH of the following strong acid or strong base solutions.
a) 0.0065 M HNO3
b) 0.0020 M NaOH
c) 0.837 g Ba(OH)2 in 1.00 L solution
Q7.
Q8.
What is the pH of a solution of 0.50 M acetic acid?
What is the pH of a 0.010 M solution of lactic acid?
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 pKaof this acid?
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?
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?
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?
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.
(A) NH4Br
(B) Na2CO3
(C) KClO4
(D) NaC2H3O2
(E) CH3CH2NH3Cl
Q15.
Which is a stronger Bronsted-Lowry base,
or HS ? Explain why.
Q 17. Rank from most acidic to most basic:
NaCN
__________
Most acidic
KOH
KF
___________
HCN
___________
HNO3
___________
___________
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
↔
Q19.
Calculate the pH of a 0.10 M solution of NH4NO3.
Q20.
Calculate the pH of a0.025 M solution of Na2HPO4.
Lewis Acid-Base Product I
Zn((NH3)42+
Lewis Acid-Base Product II