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Basic Chemistry Practice Test: Aspects of Aqueous Equilibria
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Some aspects of aqueous equilibria are: The common ion effect: Adding a strong electrolyte with an ion in common with a weak electrolyte decreases the dissociation of the weak electrolyte. The buffer region: Before the equivalence point, the solution contains a mixture of a weak acid and its salt. This is also known as the buffer region of the curve. The equivalence point: At the equivalence point, the moles of acid equal the moles of base. The solution contains only water and the salt from the cation of the base and the anion of the acid. Adding a strong electrolyte with an ion in common... Show more
Basic Chemistry Practice Test: Aspects of Aqueous Equilibria
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25 Questions

1. Calculate the percent ionization of formic acid (HCO2H) in a solution that is 0.219 M in formic acid. The Ka of formic acid is 1.77 × 10-4.
2. In which one of the following solutions is silver chloride the most soluble?
3. Calculate the pH of a solution prepared by dissolving 0.750 mol of NH3 and 0.250 mol of NH4Cl in watersufficient to yield 1.00 L of solution. The Kb of ammonia is 1.77 × 10-4 .
4. A 25.0 mL sample of 0.150 M hypochlorous acid is titrated with a 0.150 M NaOH solution. What is the pH after 26.0 mL of base is added? The Ka of hypochlorous acid is 3.0 × 10-8.
5. A 25.0 mL sample of 0.723 M HClO4 is titrated with a 0.273 M KOH solution. The + H3O concentration afterthe addition of 10.0 mL of KOH is __________ M.
6. The solubility of a slightly soluble salt is decreased by the presence of a second solule that provides a common ion to the system.
7. Which of the following could be added to a solution of acetic acid to prepare a buffer?sodium acetate sodium hydroxide nitric acid hydrofluoric acid
8. The pH of a solution prepared by mixing 45 mL of 0.183 M KOH and 65 mL of 0.145 M HCl is __________.
9. The solubility of lead (II) chloride (PbCl2) is 1.6 × 10-2 M. What is the Ksp of PbCl2
10. A solution is prepared by dissolving 0.23 mol of chloroacetic acid and 0.27 mol of sodium chloroacetate in watersufficient to yield 1.00 L of solution. The addition of 0.05 mol of HCl to this buffer solution causes the pH to dropslightly. The pH does not decrease drastically because the HCl reacts with the __________ present in the buffersolution. The Ka of chloroacetic acid is 1.36 × 10-3.
11. Calculate the percent ionization of nitrous acid in a solution that is 0.222 M in nitrous acid (HNO2) and 0.278 M in potassium nitrite (KNO2). The acid dissociation constant of nitrous acid is 4.50 × 10-4.
12. A solution is prepared by dissolving 0.23 mol of hydrazoic acid and 0.27 mol of sodium azide in watersufficient to yield 1.00 L of solution.The addition of 0.05 mol of NaOH to this buffer solution causes the pH to increase slightly. The pH does not increase drastically because the NaOH reacts with the __________ present in the buffer solution. The Ka of hydrazoic acid is 1.9 × 10-5.
13. What is the molar solubility of magnesium carbonate (MgCO3) in water? The solubility-product constant for MgCO3 is 3.5 × 10-8 at 25°C.
14. Calculate the pH of a solution prepared by dissolving 0.370 mol of formic acid (HCO2H) and 0.230 mol of sodium formate (NaCO2H) in water sufficient to yield 1.00 L of solution. The Ka of formic acid is 1.77 × 10-4 .
15. Which one of the following pairs cannot be mixed together to form a buffer solution?
16. A 25.0 mL sample of an HCl solution is titrated with a 0.139 M NaOH solution. The equivalence point is reached with 15.4 mL of base. The concentration of HCl is __________ M.
17. The pH of a solution that contains 0.818 M acetic acid -5 (Ka = 1.76 × 10 ) and 0.172 M sodium acetate is __________.
18. Which compound listed below has the smallest molar solubility in water?
19. The extent of ionization of a weak electrolyte is increased by adding to the solution a strong electrolyte that has an ion in common with the weak electrolyte.
20. A 25.0 mL sample of an acetic acid solution is titrated with a 0.175 M NaOH solution. The equivalence point is reached when 37.5 mL of the base is added. The concentration of acetic acid is __________ M.
21. The solubility product of a compound is numerically equal to the product of the concentration of the ions involved in the equilibrium, each multiplied by its coefficient in the equilibrium reaction.
22. Which of the following could be added to a solution of potassium fluoride to prepare a buffer?
23. Human blood is __________.
24. In which of the following aqueous solutions would you expect PbCl2 to have the lowest solubility?
25. The Kb of ammonia is 1.77 × 10-5 . The pH of a buffer prepared by combining 50.0 mL of 1.00 M ammonia and 50.0 mL of 1.00 M ammonium nitrate is __________.

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