Answer the following questions on notebook paper, to be collected and graded for correctness.
1. Name the following binary acids:
a. HCl
hydrochloric acid
b. HF
hydrofluoric acid
c. H2S
hydrosulfuric acid
d. HCN
hydrocyanic acid
2. Name the following oxyacids:
a. H2SO4
sulfuric acid
b. H3PO4
phosphoric acid
c. HC2H3O2
acetic acid
d. HNO3
nitric acid
e. H2SO3
sulfurous acid
f. HNO2
nitrous acid
g. HClO4
perchloric acid
h. HClO
hypochlorous acid
3. Write formulas for the following acids:
a. Perbromic acid
HBrO4
b. Chlorous acid
HClO2
c. Phosphoric acid
H3PO4
d. Hypochlorous acid
HClO
4. What is the difference between monoprotic, diprotic, and triprotic acids and give 2
examples of each.
Monoprotic acids are acids with 1 H+1 or 1 H3O+1 ion/molecule. (HCl, HF)
Diprotic acids are acids with 2 H+1 or 2 H3O+1 ions/molecule. (H2SO4, H2S, H2CO3)
Triprotic acids are acids with 3 H+1 or 3 H3O+1 ions/molecule. (H3PO4, H3AsO4)
5. Write the equation showing the 2-step ionization of sulfuric acid in dilute aqueous
solution.
Step 1)
H2SO4 + H2O 
Step 2)
HSO4-1 +
H3O+1 + HSO4-1
H2O 
H3O+1 + SO4-2
Net eq)
H2SO4 + 2 H2O  2 H3O+1 + SO4-2
6. Explain why HCl(aq) which is monoprotic is a stronger acid than H3PO4(aq), which is
triprotic.
HCl(aq) ionizes nearly 100% while H3PO4 has a low % ionization, meaning that
there are more hydronium ions in solution with the solution of HCl than with the
phosphoric acid solution.
7. Write the formula equation, total ionic equation, and net ionic equation for the reaction
between Ca(OH)2(s) and HCl(aq).
Ca(OH)2(s) +
2 HCl(aq)  CaCl2(aq) + 2 H2O()
Ca(aq) + 2 (OH)-1(aq) + 2 H+1(aq) + 2 Cl-1(aq)  Ca+2(aq) + 2 Cl-1(aq) + 2 H2O()
H+1(aq) + (OH)-1(aq) 
H2O()
8. Name the following bases:
a. NaOH
Sodium hydroxide
b. Ca(OH)2
Calcium hydroxide
c. Li(OH)
Lithium hydroxide
d. Al(OH)3
Aluminum hydroxide
e. Mg(OH)2
Magnesium hydroxide
9. Explain why Mg(OH)2 is weaker that NaOH, even though it contains more hydroxide
ions per molecule.
Saturated solutions of both of the above solutions will end up with more moles of
hydroxide ions produced by the dissociation of sodium hydroxide as it is more
soluble in water than magnesium hydroxide. In order to be an aqueous base,
there must be hydroxide ions present and the hydroxide ions are not present in
their ionic state unless they are DISSOLVED in water.
10. Dilute HCl(aq) and KOH(aq) are mixed in chemically equivalent quantities. Write the
following:
a. Formula equation for the reaction:
HCl(aq)
+
KOH(aq)

H2O()
+
KCl(aq)
b. overall ionic equation:
H+1(aq) + Cl-1(aq) + K+1 (aq) + (OH) -1(aq)  H2O() + K+1(aq) + Cl-1(aq)
c. net ionic equation:
H+1(aq) + (OH) -1(aq)  H2O()
11. What is a conjugate base?
The species that remains after a Bronsted-Lowry acid has given up a proton.
12. What is a conjugate acid?
The species that is formed after the Bronsted-Lowry base gains a proton.
13. Determine the conjugate acid for each:
CA
H2O
H3O+1
HCO3-1
H2CO3
-1
OH
H2O
-1
H2PO4
H3PO4
-1
ClO4
HClO4
-1
SH
H2S
-1
HSO4
H2SO4
CA
HF
HSO4-1
HPO4-2
HCl
CH3COOH
HCN
NH4+1
-1
F
SO4-2
PO4-3
Cl-1
CH3COO-1
CN-1
NH3
14. Determine the conjugate base for each:
CB
H2O
HCO3-1
OH-1
H3PO4
HBrO2
H2S
HSO4-1
OH-1
CO3-2
O-2
H2PO4-1
BrO2-1
HS-1
SO4-2
CB
F-1
SO4-2
PO4-3
Cl-1
CH3COO-1
OCN-1
NH2-1
HF
HSO4-1
HPO4-2
HCl
CH3COOH
HOCN
NH3
Use the table below to identify the proton donor (Bronsted-Lowry acid), identify the proton
acceptor (Bronsted-Lowry base). Use arrows to show the conjugate acid-base pairs and circle
the arrow showing the correct direction of the proton transfer reaction.
15.
a. CH3COOH(aq) + H2O()  H3O+1(aq) + CH3COO-1(aq)
Acid
Base
CA
CB
b. HCl(aq)
Acid
+
c. NH3(g)
Acid
+
NH3(g)
Base
H2O()
Base


NH4+1(aq)
CA
NH2-1 (aq)
CB
Cl-1(aq)
CB
+
+
H3O+1(aq)
CA
d. HCO3-1(aq)
Base
+
H2O()
Acid

H2CO3(aq)
CA
+
OH-1(aq)
CB
16. What is the term used to refer to any substance that can be an acid or a base?
amphoteric
What are two examples of such a substance?
1. Water H2O
2. Ammonia NH3
17. Complete the matching section below testing your general knowledge on acids & bases
A = Acid
B = Base
S = Salt
A / B = Acids & Bases
A / S = Acids & Salts
B / S = Bases & Salts
A / B / S = Acids, Bases & Salts
B
Has the Hydroxide ion (OH-) as its only anion.
A
Ionizes in water to produce hydronium ions.
S
Does not contain a H+ or OH- ion.
A
Tastes sour (examples are vinegar and citrus fruits).
AB
Can change the color of indicators.
B
Feels slippery (example being soaps).
S
CaCO3 is an example (chalk).
B
Dissociates in water to produce hydroxide ions.
B
Has a pH > (greater than) 7.
A
Has a pH < (less than) 7.
B
Is a proton (H+) acceptor.
A
Is a proton (H+) donor.
A
Is an electron pair acceptor.
B
Is an electron pair donor.
ABS Can be corrosive.
18. What is the product of all Neutralization reaction between aqueous acids and bases?
Water is always produced in neutralization reactions.
19.
What is the product of all acid anhydrides and basic anhydrides?
Acid anhydrides (nonmetal oxide) produce an acid when re-hydrated.
Basic anhydrides (metal oxide) produce a base when re-hydrated.
20.
Show that carbon dioxide is an acid anhydride of carbonic acid.
CO2(g)
21.
+
H2O()

H2CO3(aq)
Show that magnesium oxide is a basic anhydride of magnesium hydroxide.
MgO2(s)
+
H2O()

Mg(OH)2(s)
22. Complete the following neutralization reactions, making certain the balance the end
product.
a. 3 HNO3(aq) + Al(OH)3(s)
b. 2 H3PO4(aq)

+ 3 Mg(OH)2(s)
c. 2 HCl(aq) + Ca(OH)2(aq)

3 HOH()

2 HOH()
+
Al(NO3)3(aq)
6 HOH()
+
+
CaCl2(aq)
Mg3(PO4)2(s)