Honors Chemistry Study Guide for Acids and Bases 1. Calculate the ph, poh, and [H3O + ] for a solution that has a [OH - ] = 4.5 x 10-5? 2. An aqueous solution has a ph of 8.85. What are the [H + ], [OH - ], and poh? 3. Identify the acid, base, conjugate acid, and conjugate base in the following reaction. NH4 + (aq) + H2O(l) H3O + (aq) + NH3(aq) 4. Identify each of the following acids or bases as strong or weak. Next, write the reaction of each with water. a)hno3 b) NH3 5. Provide the chemical formulas for the reactants in each of the following, then write the chemical formulas for each of the products. Finally, balance each reaction. a) aqueous sulfuric acid + aqueous potassium hydroxide b) aqueous ammonia + aqueous hydrosulfuric acid (H2S) 6. Calculate the molarity of 3500. ml of solution that contains 45.0 grams of phosphoric acid, H3PO4. 7. If 45.0 ml of 0.010 M hydrochloric acid is required to neutralize 25.0 ml of an unknown base, what is the molarity of the base? 8. How many milliliters of 0.500 M sulfuric acid are required to neutralize 50.0 ml of 0.200 M potassium hydroxide?
9. 45.0 grams of calcium hydroxide is dissolved into 100. ml of water. This solution is neutralized by 145 milliliters of a nitric acid solution of unknown concentration. What is the molarity of the nitric acid solution? 10. Provide the conjugate acid or the conjugate base for each of the following. a)cl - b)h2co3 c)no2 - d)hcn 11. Determine the experimental equilibrium constant, Ka, of an acetic acid solution if 0.100 mole of acetic acid is dissolved in enough water to make 1.00 liter of solution which has a hydronium ion concentration of 0.00135 mole/liter. 12. Determine the concentration of both dissociated ions in a bottle which contains 1.000 M HC2H3O2. The Ka is 1.74 x 10-5. 13. Calculate the ph of a 0.500 M solution of aqueous ammonia. The Kb of NH3 is 1.74 x 10-5. 14. Methyl amine, CH3NH2, is a weak base that has a Kb = 4.4 x 10-6. What is the ph of a 2.00 M solution of methyl amine? 15. 75.0 milliliters of 0.345 M HCl is mixed with 50.0 milliliters of 0.456 M NaOH. What is the ph of the resulting solution?
18. According to Arrhenius Theory, acids generally: a. Turn litmus red b. release H2 gas when they react with active metals. c. React with bases to make a salt and water d. All of the above. 19. Strong acids are a. strong electrolytes. b. nonelectrolytes. c. weak electrolytes. d. nonionized 20. Which of the following is a triprotic acid? a. H2SO4 b. HCl c. CH3COOH d. H3PO4 21.Hydroxides of Group 1 metals a. are all strong bases. b. are all acids. c. are all weak bases. d. might be either strong or weak bases. 22.A Brønsted-Lowry acid is: a. an electron-pair acceptor. b. a proton acceptor. c. an electron-pair donor. d. a proton donor. 23. In the equation HCl(g) + H2O(l) H3O + aq) + Cl (aq), which species is a Brønsted-Lowry acid? a. HCl c. Cl b. H2O d. none of the above 24. A Brønsted-Lowry base is a(n) a. producer of OH ions. c. electron-pair donor. b. proton acceptor. d. electron-pair acceptor. 25. A conjugate base is the species that a. remains after a base has given up a proton. b. is formed by the addition of a proton to a base. c. is formed by the addition of a proton to an acid. d. remains after an acid has given up a proton.
26. A species that is formed when a base gains a proton is a a. conjugate base. c. strong base. b. conjugate acid. d. strong acid. 27. In a conjugate acid-base pair, the acid typically has a. one more proton than the base. c. two fewer protons than the base. b. one fewer proton than the base. d. the same number of protons as the base. 28. In the reaction HF + H2O H3O + + F -, a conjugate acid-base pair is a. HF and H2O c. H3O + and H2O b. F and H3O + d. HF and H3O + 29. In the reaction HClO3 + NH3 NH4 + + ClO3, the conjugate acid of NH3 is a. HClO3 c. NH4 + b. ClO3 d. not shown 30. In the reaction CH3COOH + H2O H3O + + CH3COO, the conjugate acid of CH3COO is a. H2O c. H3O + b. CH3COOH d. not shown 31. If a substance has a great tendency to give up protons, its conjugate has a a. great tendency to give up protons. c. slight tendency to give up protons. b. great tendency to accept protons. d. slight tendency to accept protons. 33. A species that can react as either an acid or a base is a(n) a. Lewis acid. c. oxyacid. b. amphoteric substance. d. organic substance. 34. The substances produced when KOH(aq) neutralizes HCl(aq) are a. HClO(aq) and KH(aq). c. H2O(l) and KCl(aq). b. KH2O + (aq) and Cl (aq). d. H3O + (aq) and KCl(aq). 36. A salt is NOT a. an ionic compound composed of a metal cation from a base. b. an ionic compound composed of an anion from an acid. c. a product of neutralization. d. a spectator ion. 37.Which expression represents the ph of a solution? a. log[h3o + ] c. log[oh ] b. log[h3o + ] d. log[oh ] 38. If [H3O + ] of a solution is greater than [OH ], the solution a. is always acidic. c. is always neutral. b. is always basic. d. might be acidic, basic, or neutral.
39. A water solution whose ph is 10 a. is always neutral. c. is always acidic. b. is always basic. d. might be neutral, basic, or acidic. 40. What process measures the amount of a solution of known concentration required to react with a measured amount of a solution of unknown concentration? a. autoprotolysis c. neutralization b. hydrolysis d. titration 41. Which of the following indicate the basic solution? a. [H+] = 1 x 10-1 M c. [H+] = 1 x 10-12 M b. [OH-] = 1 x 10-5 M d. [OH-] = 1 x 10-11 M 42. The conjugate base of formic acid, HCOOH, is. a. OH b. CH3COO c. HCOO d. CO2 2 43. In the reaction a. HPO4 2 is a conjugate acid b. HPO4 2 is a conjugate base c. NH3 is an acid d. NH4 + is a conjugate base 44. The conjugate acid of HSO4 is. a. H2SO4 b. SO4 2 c. SO3 2 d. HSO3 45. The conjugate base of HIO4 is. a. HIO3 b. IO4 + c. IO4 d. H2IO3 + 46. Which of the following is correct relating [H + ] and [OH ] in solution at 25 C? a. [H + ] + [OH ] = 1 10 14 c. [H + ] [OH ] = 1 10 14 b. [H + ] + [OH ] = 14.0 d. [H + ] [OH ] = 1 10 14