396 CHAPTER 10: Reactions in Aqueous Solutions I: Acids, Bases, and Salts
Acidic and Basic Salts
0 65.What are polyprotic acids? Write names and formulas for
five polyprotic acids.
0 66.What are acidic salts? Write balanced equations to show
how the following acidic salts can be prepared from the
appropriate acid and base: NaHSO 3 ; KHCO 3 ; NaH 2 PO 4 ;
Na 2 HPO 4 ; NaHS.
0 67.Indicate the mole ratio of acid and base required in each
case in Exercise 66.
0 68.The following salts are components of fertilizers. They are
made by reacting gaseous NH 3 with concentrated solu-
tions of acids. The heat produced by the reactions
evaporates most of the water. Write balanced formula unit
equations that show the formation of each. (a) NH 4 NO 3 ;
(b) NH 4 H 2 PO 4 ; (c) (NH 4 ) 2 HPO 4 ; (d) (NH 4 ) 3 PO 4 ;
(e) (NH 4 ) 2 SO 4.The Lewis Theory
0 75.Define and illustrate the following terms clearly and con-
cisely. Write an equation to illustrate the meaning of each
term. (a) Lewis acid; (b) Lewis base; (c) neutralization
according to Lewis theory.
0 76.What are the advantages and limitations of the Brønsted–
Lowry theory?
0 77.Explain the differences between the Brønsted–Lowry and
the Lewis acid–base theories, using the formation of the
ammonium ion from ammonia and water to illustrate your
points.
0 78.Write a Lewis formula for each species in the following
equations. Label the acids and bases using Lewis theory
terminology.
(a) H 2 OH 2 O 34 H 3 OOH
(b) HCl(g)H 2 O nH 3 OCl
(c) NH 3 (g)H 2 O 34 NH 4 OH
(d) NH 3 (g)HCl(g) nNH 4 Cl(s)
0 79.What is the term for a single covalent bond in which both
electrons in the shared pair come from the same atom?
Identify the Lewis acid and base and the donor and accep-
tor atoms in the following reaction.0 80.Identify the Lewis acid and base and the donor and accep-
tor atoms in each of the following reactions.0 81.Iodine, I 2 , is much more soluble in a water solution of
potassium iodide, KI, than it is in H 2 O. The anion found
in the solution is I 3 . Write an equation for the reaction
that forms I 3 , indicating the Lewis acid and the Lewis
base.
0 82.A group of very strong acids are the fluoroacids, HmXFn.
Two such acids are formed by Lewis acid–base reactions.
(a) Identify the Lewis acid and the Lewis base.HFSbF 5 88nH(SbF 6 ) (called a “super” acid,
hexafluoroantimonic acid)
HFBF 3 88nH(BF 4 ) (tetrafluoroboric acid)Cl Pt^4 Cl ClCl Cl Cl Pt Cl2 (b) 6H
HO HH
HHO(a)F
HHHBN
FFHHHN
FF B F0 69.What are polyhydroxy bases? Write names and formulas
for five polyhydroxy bases.
0 70.What are basic salts? (a) Write balanced equations to show
how each of the following basic salts can be prepared from
the appropriate acid and base: Ca(OH)Cl; Al(OH) 2 Cl;
Al(OH)Cl 2. (b) Indicate the mole ratio of acid and base
required in each case.
0 71.What are amphoteric metal hydroxides? (a) Are they bases?
(b) Write the names and formulas for four amphoteric
metal hydroxides.
0 72.Chromium(III) hydroxide and lead(II) hydroxide are typ-
ical amphoteric hydroxides. (a) Write the formula unit,
total ionic, and net ionic equations for the complete reac-
tion of each hydroxide with nitric acid. (b) Write the same
kinds of equations for the reaction of each hydroxide with
an excess of potassium hydroxide solution. Reference to
Table 10-1 may be helpful.
0 73.Write the chemical equations for the stepwise ionization
of oxalic acid, (COOH) 2 , a diprotic acid.
0 74.Write the chemical equations for the stepwise ionization
of citric acid, C 3 H 5 O(COOH) 3 , a triprotic acid.Common lawn fertilizer.