| 1. |
List four characteristic properties of acids and four characteristic properties of bases. |
| |
Acids |
Bases |
sour taste |
bitter taste |
turns litmus paper red |
turn litmus paper blue |
react with metals to form H2 (g) |
slippery feel |
form electrolytic solutions |
form electrolytic solutions |
|
| 2. |
Fill in the chart below by providing simple definitions. |
| |
|
Acid |
Base |
Arrhenius’s Definition |
produce hydrogen ions in solution |
produce hydroxide ions in solution |
Brønsted-Lowry Definitions |
proton donors |
proton acceptors |
|
| 3. |
a. |
Write the correct symbol for the hydrogen ion: H+ |
| |
b. |
Write the correct symbol for the hydronium ion: H3O+ |
| 4. |
Define the term amphiprotic. |
| |
A substance that can act as an acid in some reactions and as a base in other reactions. |
| 5. |
Write balanced equations for the: |
| |
a. |
Dissociation of calcium hydroxide, Ca(OH)2 |
| |
|
Ca(OH)2 → Ca2+(aq) + 2 OH-(aq) |
| |
b. |
Ionization of nitric acid, HNO3 |
| |
|
HNO3 → H+(aq)+ NO3-(aq) |
| 6. |
Write the equation for the ionization of nitric acid, HNO 3, showing the formation of the hydronium ion. |
| 7. |
Identify the hydrogen-ion donor & acceptor (present on the reactant side of each equation) in each of the following reactions: |
| |
| |
|
H + donor
(the acid) |
H + acceptor
(the base) |
| a. |
HNO3 (l) + H2O(l) → H3O+ (aq) + NO3-(aq) |
HNO3 |
H2O |
| b. |
C2H5NH2 (l) + H2O(l) →C2H5NH3+(aq) + OH-(aq) |
H2O |
C2H5NH2 |
| c. |
CH3CO2H(l) + H2O(l) → CH3CO2-(aq) + H3O+(aq) |
CH3CO2H |
H2O |
|
| 8. |
For each acid listed in question 7, identify it’s conjugate base. |
| |
 |
Acid
(Reactant side of equation) |
Conjugate Base |
a. |
HNO3 |
NO3- |
b. |
H2O |
OH- |
c. |
CH3CO2H |
CH3CO2- |
|
| 9. |
Write the formulas for the conjugate base of each of the following acids. |
| |
Conjugate bases have one LESS hydrogen than their acids. Losing a hydrogen ion (a proton) will increase the negative charge by a value of 1. Be careful to include all charges! |
| |
|
Acid |
Conjugate Base |
| |
a. |
H2SO3 |
HSO3- |
| |
b. |
HCO3- |
CO32- |
| |
c. |
NH4+ |
NH3 |
| 10. |
Write the formulas for the conjugate acid of each of the following bases. |
| |
Conjugate acids will have one MORE hydrogen than their corresponding base. This will cause the positive charge to increase by a value of 1. |
| |
|
Base |
Conjugate Acid |
| |
a. |
H2O |
H3O+ |
| |
b. |
CO32- |
HCO3- |
| |
c. |
PH3 |
PH4+ |
| 11. |
Which of the following would you expect to act as Brønsted-Lowry bases: |
| |
a. |
Br- |
possible base. This could combine with a proton to form HBr |
| |
b. |
Li+ |
|
| |
c. |
H3PO4 |
|
| |
d. |
NH4+ |
|
| |
e. |
H2O |
possible base. This could combine with a proton to form H3O+ |
| |
f. |
NH2- |
possible base. This could combine with a proton to form NH3 |
| 12. |
For each of the following reactions, identify the Brønsted-Lowry acid and Brønsted-Lowry base on the reactant side of the equation, and the conjugate acid and conjugate base on the product side. |
| |
a. |
HSO4-(aq) |
+ |
CO32-(aq) |
→ |
SO42-(aq) |
+ |
HCO3-(aq) |
acid |
|
base |
|
conjugate base |
|
conjugate acid |
|
| |
b. |
HCO3-(aq) |
+ |
OH-(aq) |
→ |
CO32-(aq) |
+ |
H2O(l) |
acid |
|
base |
|
conjugate base |
|
conjugate acid |
|
