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- 1. Multiple Choice
The stronger the acid, the stronger its conjugate base.
True
False
- 2. Multiple Choice
CCl3COOH is a weaker acid than CH3COOH.
True
False
- 3. Multiple Choice
The term Ka for NH4+ refers to which equation?
NH4+(aq) + H2O(l) ⇌ NH3(aq) + H3O+(aq)
NH4+(aq) + OH-(l) ⇌ NH3(aq) + H2O(l)
NH3(aq) + H2O(l) ⇌ NH3(aq) + OH-(aq)
NH3(aq) + H3O+(aq) ⇌ NH4+(aq) + OH-(aq)
- 4. Multiple Choice
Which solution has the lowest concentration of hydroxide ions?
pH = 3.21
pH = 12.59
pH = 9.82
pH = 7.00
- 5. Multiple Choice
What is the conjugate acid of NH3?
NH4+
NH3+
NH2-
NH3
- 6. Multiple Choice
HF(aq) + H2O(l) ⇌ H3O+(aq) + F-(aq)
Which of the following shows what would happen to the % ionization of HF when, in two separate
experiments, 1.0 mL of distilled water and 1.0 mL of 1.0 M KF are added to a 10. mL sample of 1.0 M HF(aq)?
A
B
C
D
- 7. Multiple Choice
Which of the following aqueous solutions has the lowest [H+]?
a 1.0 x 10−3 M solution of NaOH
a 1.0 x 10−4 M solution of HNO3
pure water
a solution with a pOH of 10.0
- 8. Multiple Choice
Values of pKw at various temperatures are listed in
the table. Based on the information, which of the following statements is true?
The dissociation of water is an exothermic process.
The pH of pure water is 7.00 at any temperature.
As the temperature increases, the pH of pure water increases
As the temperature increases, the pH of pure water decreases.
- 9. Multiple Choice
Which of the following indicators would be the best choice for determining the endpoint in this titration?
methyl orange (pH range: 2.1-3.6)
methyl red (pH range: 4.2-6.5)
thymol blue (pH range: 8.0-9.6)
alizarin yellow (pH range: 10.0-12.0)
- 10. Multiple Choice
A solution is prepared by adding 1.0 M HC2H3O2 to 1.0 M NaC2H3O2. The solution's pH is measured to be 4.73. After 3 drops of 1.0 M HCl are added to the solution, the pH of the solution is still 4.73. Which equation accounts for the fact that acid was added but there was no detectable change in pH?
H3O+(aq) + OH–(aq) → 2 H2O(l)
H3O+(aq) + Cl–(aq) → HCl(g) + H2O(l)
H3O+(aq) + C2H3O2–(aq) → HC2H3O2(aq) + H2O(l)
H3O+(aq) + HC2H3O2(aq) → H2C2H3O2+(aq) + H2O(l)
- 11. Multiple Choice
A solution contains equimolar amounts of HOCl and NaOCl and has a pH of 7.5. Then KOH is added to this solution. Which of the following most accurately identifies the species present in greater concentration and the pH of the solution after KOH is added?
HOCl; pH < 7.5
HOCl; pH > 7.5
OCl-; pH < 7.5
OCl-; pH > 7.5
- 12. Multiple Choice
A sample of a weak acid, HA, is titrated, with 0.100 M NaOH added. Which of the following is the best particulate representation of the species (other than H2O) that are present in significant concentrations in the solution at point U in the titration?
- 13. Fill in the Blank
Which particle diagram best represents the acid with the least stable conjugate base?
- 14. Fill in the Blank
On the basis of the pH curve, the pKa value of the acid used in the titration is closest to
- 15. Fill in the Blank
A 0.070 M base solution eventually reaches a pOH of 5.00, what is the percent ionization?
- 16. Fill in the Blank
Benzoic acid, C6H5COOH, is 1.0 % ionized in a 0.010 M aqueous solution according the equation: C6H5COOH(aq) ⇌ H+(aq) + C6H5COO-(aq)
What is the value of Ka for aqueous benzoic acid?
- 17. Open Ended
Which curve represents the titration of a weak base? Include 2 reasons.
- 18. Open Ended
Buffers were created using a weak acid, HA, (pKa = 3.20) and LiA.
Buffer X = 1.00 M of HA + 0.50 M of LiA.
Buffer Y = 0.50 M of HA + 1.00 M of LiA.
Buffer Z = 2.00 M of HA and 4.00 M of LiA.
Which buffer will be best at resisting a change to the pH when a base is added? Justify your answer.
- 19. Open Ended
Based on the data, which species is dominant at a pH of 5? The acid or the conjugate base? Explain your reasoning.
- 20. Open Ended
A solution contains 150.0 g of Ba(OH)2 in 12.5 L of solution. Calculate the pH of the solution.
- 21. Open Ended
The pOH of 50.0 mL of a solution of H2SO4 is 12.44. How many moles of H2SO4 are in the solution?
- 22. Open Ended
At 50°C the Kw of pure water is 5.476 x 10-14. Calculate the H3O+ concentration.
- 23. Open Ended
A 50.0 mL sample of a weak acid is titrated with 0.10 M NaOH. What is the concentration of the weak acid?
- 24. Open Ended
What is the concentration of acetic acid, HC2H3O2, in a buffer solution with a pH of 5.293. The solution contains 0.530 M C2H3O2-. Acetic acid has a Ka of 1.80 x 10-5.
- 25. Open Ended
You heated a sample of pure water and measured that the pH was 6.767. What is the concentration of the hydroxide ion?
- 26. Open Ended
Calculate the pH of a solution that is composed of 90.0 mL of 0.345 M NaOH and 50.0 mL of 0.123 M lactic acid, HC3H5O3. (Ka of lactic acid = 1.38x10-4)
- 27. Open Ended
What is the hydronium ion concentration of a solution formed from 150.0 mL of 0.200 M NH3 and 150.0 mL of 0.200 M HCl? (Kb for NH3 is 1.80x10-5)
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