Acid and Bases Review
1. List some similarities and differences between Bronsted-Lowry acids and bases.
2. List some indicators and the colours they turn in acid and base solutions.
3. Which of the following is considered to be a weak base, strong base, strong acid, weak acid?
a) C2H5NH2(aq) + H2O(l) ↔ C2H5NH3+(aq) + OH-(aq) ______
c) NaOH(s)  Na+(aq) + OH-(aq) _____
+
b) HNO3(aq) + H2O(l) ↔ H3O (aq) + NO3 (aq) _______
d) HCl(aq)  H+(aq) + Cl-(aq) _______
4. In which of the following, is HCO21-(aq) acting as an acid?
a) HCO21-(aq) + H2O(l) ↔ CO22-(aq) + H3O+(aq) b) HCO21-(aq) + H2O(l) ↔ H2CO2(aq) + OH-(aq)
5. You have the substance HPO42-(aq).
a) What is its conjugate base? _________
b) What is its conjugate acid? ____________
6. Which of the following could you write a Ka for?
a) HCl  H+ (aq) + Cl- (aq)
c) C2H5NH2(aq) + H2O(l) ↔ C2H5NH3+(aq) + OH-(aq)
b) H2SO4(aq) + H2O(l) ↔ HSO41-(aq) + H3O+(aq) d) NaOH(s)  Na+(aq) + OH-(aq)
7. What is the correct Ka for the second ionization of sulfuric acid?
a) Ka =
[HSO4-(aq)]
c) Ka= [H2SO4(aq)]
-2
+
[SO4 (aq)][ H3O (aq)]
[HSO4-(aq)][ H3O+(aq)]
b) Ka = [SO4-2(aq)][ H3O+(aq)]
[HSO4-(aq)]
d) Ka=[HSO4-(aq)] [ H3O+(aq)]
[H2SO4(aq)]
8. What does amphiprotic/amphoteric mean?
9. Label the acid, base, conjugate acid and conjugate base in the following reactions:
a) A- + H2O ↔ HA + OH-
b) HF + H2O  F- + H3O+
c) I- + H2O ↔ HI + OH-
10. Write out the complete steps in the ionization of the diprotic acid, hydrosulfuric acid, H2S.
11. Write out the acid ionization equation and the Ka for the weak acid iodic acid, HIO3.
12. Write out the base ionization equation and the Kb for the weak base, HCO3-.
13. Write out the base ionization equation and the Kb for the weak base, NH2.
14. What is the difference between strength and concentration of acids and bases?
15. Fill in the following table:
pH
[H+]
pOH
[OH-]
Acid, base,
neutral?
1.6 x 10-3
3.00
11.50
neutral
3.4 x 10
-9
16. What is the [OH-] of the following STRONG bases?
a) 5.0M KOH ________ b) 2.0M Mg(OH)2 _____________
c) 1.5M Al(OH)3 __________
17. You have a solution of 0.036 M KOH (a strong base).
a) What is the [OH-] of your KOH solution? __________________
b) Calculate the pOH, pH and [H+] of your KOH solution.
18. You have an aqueous solution of 0.064M (a strong acid).
a) What is the [H+] of the HCl? ______________________
b) Calculate the pH, pOH and [OH-].
19. HNO2 is a weak acid. In a 0.0400 M solution of HNO2, the equilibrium pH is 1.80.
a) Write out the balanced equation for the ionization of nitrous acid.
b) Calculated the equilibrium concentrations using an ICE chart.
c) Calculate the Ka for HNO2.
20. What is the difference between an “endpoint” and the “equivalence point” of a titration?
21. If you titrated 110 mL of sulfuric acid to completely neutralize 55mL of 2.0M potassium hydroxide,
a) Write out the balanced neutralization reaction.
b) What is the concentration of sulfuric acid used in the titration?
22. If you titrated 50.0 mL of 2.00 M Ba(OH)2 to completely neutralize a 2.5M solution of hydrochloric
acid,
a) Write out the balanced neutralization reaction.
b) What is the volume of acid used in the titration?