Unit 9: Acid and Base Multiple Choice Practice

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1 Unit 9: Acid and Base Multiple Choice Practice Name June 14, Consider the following acidbase equilibrium: HCO3 H2O H2CO3 OH In the reaction above, the BrönstedLowry acids are: A. H2O and OH B. HCO3 and OH C. H2O and H2CO3 D. HCO3 and H2CO3 2. The solution with the lowest electrical conductivity is: A. 0.10M H2S B. 0.10M HNO2 C. 0.10M H2SO3 D. 0.10M NH4Cl 3. The solution with the lowest ph is: A. 1.0M HF B. 1.0M HCN C. 1.0M H2CO2 D. 1.0M HC2H3O2 4. As the [H3O in a solution decreases, the [OH A. increases and the ph increases. B. increases and the ph decreases. C. decreases and the ph increases. D. decreases and the ph decreases. 5. What is the poh of 2.5 M NaOH? A B C D Which of the following salts dissolves to produce a basic aqueous solution? A. LiF B. KClO4 C. NaHSO3 D. NH4NO3 7. Which titration curve represents the titration of HCl with NaOH?

2 8. A buffer solution can be formed by dissolving equal moles of: A. HF and NaF B. HCl and NaOH C. KBr and Na 3PO 4 D. HC 2H 3O 2 and NaCl 9. Consider the following: The term amphiprotic can be used to describe: A. I only. B. II and III only. C. I, II and III only. D. II, III and IV only. 10. Calculate the [H 3O in a solution prepared by mixing 25.0mL of 1.0M HCl with 50.0mL of 0.50M KOH. A. 1.0 M B M C M D M 11. Which of the following is a property of sodium hydroxide? A. feels slippery B. releases H 3O in aqueous solution C. changes litmus paper from blue to red D. reacts with magnesium to produce hydrogen gas 12. The conjugate acid of HAsO 4 2 is A. H 3O B. AsO 4 3 C. H 3AsO 4 D. H 2AsO Which of the following 0.10M solutions has the highest electrical conductivity? A. HF B. HCN C. H 2CO 3 D. H 3BO Which of the following describes the relationship between [H 3O and [OH? A. [H 3O OH B. [H 3O OH C. [H 3O OH D. [H 3O OH Calculate the [H 3O in a 0.010M solution of Sr(OH) 2. A M B M C M D M 16. The value of Kb for HCO 3 is: A B C D A buffer solution is formed by adding which of the following to water? A. HCl and KOH B. HCN and RbCN C. NaBr and NaOH D. HNO 3 and LiNO 3 2

3 18. Consider the following BrönstedLowry equilibrium system: HSO 3 H 2PO 2 4 SO 3 H 3PO 4 What are the two BrönstedLowry bases in the equilibrium above? 2 A. HSO 3 and SO 3 B. H 2PO 2 4 and SO 3 C. HSO 3 and H 3PO 4 D. H 2PO 4 and H 3PO The equation representing the predominant reaction of sodium ethanoate, NaCH 3COO, with water is: A. CH 3COO H 2O CH 3COOH OH B. CH 3COO H 2O H 3O CH 2COO 2 C. CH 3COOH H 2O H 3O CH 3COO D. CH 3COOH H 2O CH 3COOH 2 OH 20. Which of the following solutions will have the lowest electrical conductivity? A. 0.1M HF B. 0.1M NaF C. 0.1M H 2SO 3 D. 0.1M NaHSO Which of the following is the strongest BrönstedLowry base? A. NH 3 B. CO 3 2 C. HSO 3 D. H 2BO Addition of HCl to water causes: A. both [H 3O and [OH to increase. B. both [H 3O and [OH to decrease. C. [H 3O to increase and [OH to decrease. D. [H 3O to decrease and [OH to increase. 23. Which of the following graphs describes the relationship between [H 3O and [OH in aqueous solutions at a constant temperature: 3

4 24. Consider the following: Which of the above is/are present in a reagent bottle labeled 1.0M H 2SO 4? A. I only B. I and II only C. II and III only D. I, II and III 25. The ph of a 0.10M KOH solution is: A B C D Which of the following salts will dissolve in water to produce a neutral solution? A. LiF B. CrCl 3 C. KNO 3 D. NH 4Cl 27. Calculate the H 3O of a solution prepared by adding 10.0mL of 2.0M HCl to10.0ml of 1.0M NaOH. A M B M C. 1.0 M D. 2.0 M 28. Which of the following, when dissolved in water, will produce an acidic solution? A. SrO B. NO 2 C. CaO D. Na 2O 29. An Arrhenius acid is defined as a chemical species that: A. is a proton donor. B. is a proton acceptor. C. produces hydrogen ions in solution. D. produces hydroxide ions in solution. 30. Consider the acidbase equilibrium system: HC 2O 4 H 2BO 3 H 3BO 3 C 2O 2 4 Identify the BrönstedLowry bases in this equilibrium. A. H 2BO 3 and H 3BO 3 B. HC 2O 4 and H 3BO 3 C. HC 2O 4 and C 2O 2 4 D. H 2BO 3 and C 2O The ph of a solution changes from 3.00 to By what factor does the [H 3O change? A. 2 B. 3 C. 100 D The [OH in a solution of ph 3.00 is: A M B M C M D M 33. Which of the following titrations will have the highest ph at the equivalence point? A. HBr with NH 3 B. HNO 2 with KOH C. HCl with Na 2CO 3 D. HNO 3 with NaOH 4

5 34. Which of the following graphs describes the relationship between [H 3O + ] and ph? 35. When the [H 3O + ] in a solution is increased to twice the original concentration, the change in ph could be from A. 1.7 to 1.4 B. 2.0 to 4.0 C. 5.0 to 2.5 D. 8.5 to Which of the following describes the relationship between acid strength and Ka value for weak acids? 37. The value of Kb for HPO 4 2 is A. 2.2 X B. 6.2 X 10 8 C. 1.6 X 10 7 D. 4.5 X What volume of 0.100M NaOH is required to completely neutralize 15.00mL of 0.100M H 3PO 4? A. 5.00mL B. 15.0mL C. 30.0mL D. 45.0mL 39. What is the ph of the solution formed when moles NaOH is added to 1.00L of 0.050M HCl? A B C D

6 40. Which of the following graphs describes the relationship between the ph of a buffer and the volume of NaOH added to the buffer? 41. Consider the following reaction: H 3BO 3 (aq) + HS (aq) H 2BO 3 (aq) + H 2S (aq) The order of BrØnstedLowry acids and bases in this equation is: A. acid, base, base, acid. B. acid, base, acid, base. C. base, acid, acid, base. D. base, acid, base, acid. 42. The conjugate base of an acid is produced by: A. adding a proton to the acid. B. adding an electron to the acid. C. removing a proton from the acid. D. removing an electron from the acid. 43. Which of the following represents the predominant reaction between HCO 3 1 and water? A. 2HCO 3 H 2O + 2CO 2 B. HCO 3 + H 2O H 2CO 3 + OH C. HCO 3 + H 2O H 3O CO 3 D. 2HCO 3 + H 2O H 3O CO 3 + OH + CO Water acts as an acid when it reacts with which of the following? A. I and IV only B. II and III only C. I, II and IV only D. II, III and IV only 6

7 45. Which of the following graphs describes the relationship between ph and poh? 46. Which of the following solutions has a ph less than 7.00? A. NaCl B. LiOH C. NH 4NO 3 D. KCH 3COO 47. Which of the following will form a basic aqueous solution? A. HSO 3 B. HSO 4 C. HPO 4 2 D. HC 2O What is the ph of the solution formed when 0.040mol NaOH (s) is added to 2.00L of 0.020M HCl? A B C D Which of the following titrations will always have an equivalence point at a ph > 7.00? A. weak acid with a weak base B. strong acid with a weak base C. weak acid with a strong base D. strong acid with a strong base 50. What is the concentration of Sr(OH)2 in a solution with a ph = 11.00? A. 2.0 x B. 1.0 x C. 5.0 x 10 4 D. 1.0 x When comparing 1.0M solutions of bases, the base with the lowest [OH ] is the: A. weakest base and it has the largest Kb value. B. strongest base and it has the largest Kb value. C. weakest base and it has the smallest Kb value. D. strongest base and it has the smallest Kb value. 52. The value of K b for HC 2O 4 is: A. 1.7 X B. 1.6 X C. 6.4 X 10 5 D. 5.9 X What is the ph of the solution formed when mol NaOH (s) is added to 1.00L of 0.050M HCl? A B C D

8 54. Which of the following titrations will have an equivalence point with a ph less than 7.00? A. H 2SO 4 with NH 3 B. HNO 3 with LiOH C. H 3PO 4 with KOH D. HCOOH with NaOH 55. Which of the following statements applies to 1.0M NH 3 (aq) but not to 1.0M NaOH (aq)? A. partially ionizes B. neutralizes an acid C. has a ph greater than 7 D. turns bromcresol green from yellow to blue 56. What is the poh of a solution prepared by adding 0.50mol of NaOH to prepare 0.50L of solution? A B C D What is the [H 3O + ] in a solution with a poh = 5.20? A. 1.4 X M B. 1.6 X 10 9 M C. 6.3 X 10 6 M D. 7.1 X 10 1 M 58. K a for the acid H 2AsO 4 is X What is the value of K b for HAsO 4 2? A. 5.6 X B. 3.2 X C. 1.8 X 10 7 D. 2.4 X In a titration, which of the following has a ph = 7.00 at the equivalence point? A. NH 3 and HNO 3 B. KOH and HCN C. NaOH and HCl D. Ca(OH) 2 and CH 3COOH 60. Which of the following salts dissolves to produce a basic solution? A. KCl B. NH 4Br C. Fe(NO 3) 3 D. LiCH 3COO 61. During a titration, what volume of 0.500M KOH is necessary to completely neutralize 10.0mL of 2.00M CH 3COOH? A. 10.0mL B. 20.0mL C. 25.0mL D. 40.0mL 62. A buffer solution will form when 0.10M NaF is mixed with an equal volume of: A. 0.10M HF B. 0.10M HCl C. 0.10M NaCl D. 0.10M NaOH 63. A solution is prepared by mixing 1.50 X 10 3 mol HCl with 3.00 X 10 3 mol KOH. Calculate the moles of OH present after mixing. A. 0 mol B X 10 3 mol C X 10 3 mol D X 10 3 mol 64. The conjugate acid of C 6H 5NH 2 is: A. C 6H 5NH B. C 6H 5NH 3 C. C 6H 5NH 2 + D. C 6H 5NH Which of the following is a property of 1.0M HCl but not a property of 1.0M HC 2H 3O 2? A. turns litmus red B. ionizes completely C. has a ph less then 7.0 D. produces H 3O + in solution 8

9 66. When a solution has poh = 5.30, the [OH ] is: A. 5.0 X 10 6 M B. 2.0 X 10 9 M C M D M 67. Which of the following will be the most basic? A. 1.0M NO 3 B. 1.0M SO 4 C. 1.0M CO 3 D. 1.0M PO Which of the following titrations would have a ph > 7 at the equivalence point? A. HI with KOH B. HClO 4 with NH 3 C. HCl with Sr(OH) 2 D. HCOOH with NaOH 9

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