Handout Acid Base- Chapter 15
1. What is the hydronium ion concentration of a .0200 M acetic acid
(HC2H3O2) solution? (Ka 1.7 x 10 -5)
2. What is the hydronium ion concentration of a .0200 M nitric acid (HNO3)
solution?
3. What is the hydronium ion concentration of a .00100 M HCl solution?
4. If .072 grams of HCl are dissolved in 5.0 liters (total volume of solution) of
water, what is the hydronium ion concentration of the solution?
5. What is the hydronium ion concentration of a solution made by dissolving 7.2
grams of HCN in 10.0 liters (total volume of solution) of water? (Ka = 4.9 x 10-10)
6. The hydronium ion concentration of a 0.10 M of a weak acid (HA) solution is
6.3 x 10-6 M, what is the Ka for this acid?
7. An acid solution (HA) was made by dissolving .50 moles of the acid in 10.0 liters (total
volume of solution) of water. The hydronium ion concentration of the solution was found to be
3.0 x 10 -5. Determine the Ka for this acid. (assume the acid is weak and therefore not much
ionizes.)
8. What is the hydroxide ion concentration in a 0 .0020 M NaOH solution?
9. If .030 mole of NaOH are dissolved in 2.5 liters of water, what is the hydroxide ion
concentration?
10. If the Kb of ammonia (NH3) is 1.8 x 10-5, what is the hydroxide ion concentration in a .20
M NH3 solution?
11. What is the molarity of a NaOH solution if it takes 30.0 ml to neutralize 20.0 ml of .100M
HCl ?
12. What volume of .50M HCl is needed to neutralize 25.0 ml of .80 M NaOH
solution?
13. What is the molarity of an NaOH solution if it takes 15.0 ml of it to
neutralize 12.0 ml of .30 M H2SO4 solution?
14. For each of the following acids write the conjugate base
HCl ______ HNO3 __________H3PO4__________H3O+________NH4+________H2CO3________H2O_____
15. For each of the following bases, write the conjugate acid
Cl -_____ HPO42-_____ NH3_________ CO32-______ OH- ______ H2O ______ H2PO4- _______
16. Complete the following acid/base reactions using the Bronsted-Lowry definition. Identify
the acid and base on the reactant side and on the product side.
H2CO3 + SO42- --------->
NH4+ + CO3 2- ---------->
17. Given the following hydronium ion concentrations [H3O+] , determine the hydroxide
ion concentrations [OH-] and the pH of the following solutions.
[H3O+]
[ OH -]
pH
0.000100 M
1.0 x 10 -2 M
1.2 x 10 -3 M
9.0 x 10 -8 M
18. Given the following hydroxide ion concentrations [OH-], determine the hydronium ion
concentrations [H3O+] and the pH of the following solutions.
[OH-]
[H3O+]
pH
0.000100 M
1.0 x 10 -5 M
4.2 x 10 -9 M
5.0 x 10 -5 M
19. Given the pH, determine the hydronium and hydroxide concentrations of each of the
following solutions. Also indicate whether each solution is acidic or basic ( alkaline)
pH
hydronium ion concentration
hydroxide ion concentration
acidic or basic
4.0
3.5
8.0
6.2
11.9
20. If solution A has a pH of 6 and solution B has a pH of 3, which solution is more acidic?
By what factor? (How many more times acidic is it?)
21. For each of the following determine the hydronium ion concentration, the hydroxide ion
concentration and the pH
a.
.000100 M HCl solution
b . .0030 M NaOH solution?
c.
.040 mole of NaOH are dissolved in 2.0 liters of water
d.
0.0400 M acetic acid HC2H3O2 solution (Ka 1.7 x 10 -5)
22. What is the molar mass of a monoprotic acid if 1.30 grams of the acid is neutralized by
40.0 ml of .50 M NaOH solution?
23. A solution was made by dissolving 0.30 moles of NaF in 1.0 liter of a 0.40 M
solution of HF. The Ka for HF is 6.8 x10 -4 Determine the pH of this solution.
24. A solution was made by dissolving 0.50 moles of NaC2H3O2 in 2.0 liters of a
0.20 M solution of HC2H3O2. The Ka for HC2H3O2 is 1.7 x10 -5. Determine the pH of this
solution.