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Chapter 14 Test Review

Chapter 14 Test Review. Acids and Bases 14.1-14.3, 14.5-14.8. 1. According to the Arrhenius concept, if HNO 3 were dissolved in water, it would act as ___. A) a base B) an acid C) a proton acceptor D) a source of H- ions E) a source of hydroxide ions.

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Chapter 14 Test Review

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  1. Chapter 14 Test Review Acids and Bases 14.1-14.3, 14.5-14.8

  2. 1. According to the Arrhenius concept, if HNO3 were dissolved in water, it would act as ___. A) a base B) an acid C) a proton acceptor D) a source of H- ions E) a source of hydroxide ions

  3. 2. The name given to an aqueous solution of HBrO2 is ___. A) bromous acid B) hydrobromic acid C) hypobromous acid D) hydrogen bromide E) bromic acid

  4. 3. The name of HClO is ___. A) Chloric acid B) Hypochlorous acid C) Hydrochlorous acid D) Hydrogen chloride E) Perchloric acid

  5. 4. The I.U.P.A.C. name of the following ___ acid.CH3COOH A) carbonic B) chloric acid C) ethanoic D) acetic E) carboxylic

  6. 5. According to the Brønsted-Lowery definition, a proton-donor is a(n) ___. A) H+ acceptor B) OH- acceptor C) salt D) base E) acid

  7. 6. Which of the following compounds would be an Arrhenius base? A) NaClO B) Na2SO4 C) NaOH D) CuCl2 E) H3P

  8. 7. Identify the B-L acid in forward direction of the following reaction. A) H2O(l) B) CO32-(aq) C) OH-(aq) D) H2CO3 (aq) E) HCO32- (aq) H2O(l) + CO32-(aq) HCO32- (aq) + OH-(aq)

  9. 8. Identify the B-L base in reverse direction of the following reaction. A) CH3CH2NH3+(aq) B) CH3CH2NH2(aq) C) H2S(aq) D) CH3CH2NH4-(aq) E) HS-(aq) CH3CH2NH3+(aq) + HS-(aq) CH3CH2NH2(aq) + H2S(aq)

  10. 9. For KW, the product of [H3O+] and [OH-] is __. A) 1 x 10-1 B) 1 x 1014 C) 1 x 107 D) 1 x 101 E) 1 x 10-14

  11. 10. What is the [H3O+] in a solution with [OH-] = 1 x 10-12 M? A) 1 x 102 M B) 1 x 10-12 M C) 1 x 10-7 M D) 1 x 10-8 M E) 1 x 10-2 M

  12. 11. What is the [OH-] in a solution with [H3O+] = 1 x 10-6 M? A) 1 x 10-6 M B) 1 x 10-2 M C) 1 x 10-12 M D) 1 x 10-10 M E) 1 x 10-8 M

  13. 12. A solution with a pH of 4 is ___. A) extremely acidic B) neutral C) moderately acidic D) extremely basic E) slightly basic

  14. 13. The [H3O+] of a solution with a pH = 2.0 has a concentration of ___. A) 10 M B) 1 x 10-2 M C) - 10M D) 1 x 10-12 M E) 1 x 102 M

  15. 14. Which of the following has the pH values correctly arranged from the most basic to the least basic? A) 6, 7, 8, 9, 10 B) 14, 13, 12, 11, 10 C) 3, 7, 9, 11, 13 D) 13, 6, 10, 5, 1 E) None of these are correct.

  16. 15. Which of the following is one of the 7 strong acids? A) NH4+ B) HF C) H3O+ D) HClO3 E) NaOH

  17. 16. Which of the following has been correctly identified? A) HClO4, strong acid B) Al(OH)3, strong base C) H3O+, strong acid D) NH3, strong acid E) NaOH, weak base

  18. 17. Ammonia is a weak base because __. A) it is completely ionized in aqueous solution B) it is only slightly soluble in water C) it cannot hold on to its hydroxide ions D) it produces few hydroxide ions in water E) it is a dilute solution NH3(aq) + H2O(l) NH4+ (aq) + OH-(aq)

  19. 18. Water is an example of a(n) ___ compound. A) organic B) nonpolar C) amphoteric D) ionic E) carboxylic acid

  20. 19. One example of an Arrhenius base is ___. A) H2SO4 B) KOH C) NaCl D) H2O2 E) C2H4O2

  21. 20. Acetic acid is an example of a(n) ___. A) inorganic compound B) weak acid C) strong acid D) oxy acid E) binary acid

  22. 21. In water solution, the conjugate base of HF is ___. A) H2O B) H+ C) F- D) OH- E) H2 HF(aq) + H2O(l) H3O+ (aq) + F-(aq)

  23. 22. The conjugate acid of NO2- is ___. A) OH- B) H2O C) HNO3 D) HNO2 E) H+

  24. 23. Bicarbonate ion, HCO3-, is an example of a(n) ___ substance. A) gaseous B) neutral C) strongly acidic D) amphoteric E) strongly basic

  25. 24. The conjugate acid of NH3 is ___. A) NH2- B) NH4+ C) H3O+ D) H2O E) OH-

  26. 25. The pH of a 0.05 M solution of KOH is ___. A) 12.7 B) 1.3 C) 13.5 D) 5.0 E) 9.0 0.05 M KOH = 0.05 M OH- 2) pOH = -log(0.05) → 1.3 3) 14.00 – 1.3 = 12.7

  27. 26. The pH of a solution is 4.50. The pOH of this solution is ___. A) 14.00 B) 4.50 C) 2.00 D) 9.50 E) 7.00 pH + pOH = 14.00 14.00 – 4.50 = 9.50

  28. 27. What is the pOH of a solution with a pH of 3.77? A) 2.5 B) 0.25 C) 10.3 D) 0.115 E) 14.0 pH + pOH = 14.00 14.00 – 3.77 = 10.3

  29. 28. A solution with a pH of 10.00 is basic. TRUE or FALSE

  30. 29. What are the products of the following reaction between an active metal and a strong acid? A) SrHNO3 B) SrH + NO3 C) NOH + SrO2 D) O2 + SrNO2 + H E) H2 + Sr(NO3)2 Sr(s) + HNO3(aq) ???? The products are always hydrogen gas and the metal salt of the acid.

  31. 30. In an acidic solution ___. A) [H+] = 0 B) [OH-] = 0 C) [OH-] > [H+] D) [OH-] = [H+] E) [H+] > [OH-]

  32. 31. A solution with a pH of 2.0 is ___ times more acidic than a solution with a pH of 5.0. A) 2 B) 5 C) 10 D) 1,000 E) 100

  33. 32. According to the table at the right, which of the following is the weakest acid? A) HF B) H2O C) H2PO4- D) HCl E) NH4+

  34. 33. According to the table at the right, when H2S and HF are reacted, what will be the proton donor? A) HF B) H2O C) H2S D) F- E) HS- The stronger of the two acids will be the H+ donor.

  35. 34. Which of the following acids has the strongest conjugate base? A) HF B) H2O C) H2S D) HCl E) H3O+ The acid with the conjugate which is furthest down on the right.

  36. 35. Are reactants or products favored in the following acid-base equilibrium? HF(aq) + H2O(l) H3O+ (aq) + F-(aq) A) reactants B) products

  37. 36. Predict the products of the following reaction between a strong acid and a metal carbonate. Balance the equation when you are done. Li2CO3 + HNO3 2 2 LiNO3 + CO2(g) + H2O(l) ???? The products are always carbon dioxide gas, water, and the metal salt of the acid.

  38. 37. 50.0 mL of HNO3 were titrated to the end point with 25.0 mL of 0.35 M KOH solution. Write a balanced chemical equation for this acid-base neutralization reaction. HNO3 (aq) + KOH(aq) → H2O(l) + KNO3 Remember: the products of the neutralization reaction between a strong acid and a strong base are always water and the metal salt of the acid.

  39. 38. 50.0 mL of HNO3 were titrated to the end point with 25.0 mL of 0.35 M KOH solution. Calculate the number of moles of KOH needed to completely neutralize the HNO3. 0.35 mole KOH / L x 0.0250 L = 0.0088 mol KOH Determine the number of moles of HNO3 which were neutralized by the KOH. 1 : 1 stoichiometry between HNO3 and KOH, so 0.0088 mol KOH used = 0.0088 mol HNO3 neutralized Calculate the Molarity of the acid solution. 0.0088 mol HNO3 / 0.0500 L = 0.18 M

  40. 39. 50.0 mL of HNO3 were titrated to the end point with 25.0 mL of 0.35 M KOH solution. Which solution was the standardized solution? KOH If phenolphthalein indicator had been added to the acid, what color would the solution be at the endpoint of the titration? Pink

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