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Chapter 16 Jeopardy Review: Acid-Base Equilibria

Chapter 16 Jeopardy Review: Acid-Base Equilibria. Question #1. Which of the following is a property of an acid? Feel like water Turn litmus paper blue React vigorously with metals higher on the activity series Taste bitter Conduct electric current *You may choose more than one option.

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Chapter 16 Jeopardy Review: Acid-Base Equilibria

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  1. Chapter 16 Jeopardy Review:Acid-Base Equilibria

  2. Question #1 Which of the following is a property of an acid? • Feel like water • Turn litmus paper blue • React vigorously with metals higher on the activity series • Taste bitter • Conduct electric current *You may choose more than one option

  3. Answer: • Feel like water c) React vigorously with metals higher on the activity series e) Conduct electric current

  4. Question #2 In a neutralization reaction, acids combine with bases so that the properties of both are lost. What are the 2 products of a neutralization reaction?

  5. Answer: water + salt

  6. Question #3 Which statement below is true? • An Arrhenius acid accepts hydrogen ions when dissolved in water. • A Bronsted-Lowry base generates hydroxide ions when dissolved in water. • A Lewis acid can accept a pair of electrons.

  7. Answer: c) A Lewis acid can accept a pair of electrons.

  8. Question #4 Name two problems with the Arrhenius definition of acids and bases.

  9. Answer: • It is restricted to aqueous solutions. • It does not explain why some bases do not contain OH- ions (ex: NH3)

  10. Question #5 Give the name AND formula for the seven strong acids we discussed in class.

  11. Answer: Hydrochloric Acid, HCl Hydrobromic Acid, HBr Hydroiodic Acid, HI Chloric Acid, HClO3 Perchloric Acid, HClO4 Sulfuric Acid, H2SO4 Nitric Acid, HNO3

  12. Question #6 All of the alkali metals, when combined with hydroxide, are considered to be strong bases. Which three alkaline earth metals are also classified as strong bases when combined with hydroxide? *Give name AND symbol

  13. Answer: Calcium (Ca) Strontium (Sr) Barium (Ba)

  14. Question #7 Name the following acids: HCN H2SO3 H2CO3

  15. Answer: HCN – hydrocyanic acid H2SO3 – sulfurous acid H2CO3– carbonic acid

  16. Question #8 Give the formulas for the following acids: Acetic acid Hydrofluoric Acid Phosphorous Acid

  17. Answer: Acetic acid – HC2H3O2 Hydrofluoric Acid – HF Phosphorous Acid – H3PO3

  18. Question #9 Name this ion: H3O+

  19. Answer H3O+ - hydronium ion

  20. Question #10 What word do we use to describe a substance that is capable of acting as either an acid or a base?

  21. Answer: Amphiprotic or amphoteric

  22. Question #11 The stronger an acid or a base, the _________ its conjugate acid or conjugate base. Therefore, an acid and its conjugate base or a base and its conjugate acid have a(n) __________ relationship.

  23. Answer: The stronger an acid or a base, the weaker its conjugate acid or conjugate base. Therefore, an acid and its conjugate base or a base and its conjugate acid have a(n) inverse relationship.

  24. Question #12 Give the conjugate base for the following Bronsted-Lowry acids: PH4+ H2O CH3COO-

  25. Answer: PH3 OH- CH2COO2-

  26. Question #13 Give the conjugate acid for the following Bronsted-Lowry bases: HSO4- H2O CO32-

  27. Answer: H2SO4 H3O+ HCO3-

  28. Question #14 In the reaction below, which substance is acting as the conjugate base? H2SO4 + NH3 HSO4- + NH4+

  29. Answer: Conjugate base = HSO4-

  30. Question #15 Write two chemical equations for the reaction of HSO3- with water: one in which HSO3- acts as an acid, and one in which it acts as a base. Be sure to include states of matter.

  31. Answer: HSO3- (aq) + H2O (l)  SO32- (aq) + H3O+ (aq) HSO3- (aq) + H2O (l)  H2SO3 (aq) + OH- (aq)

  32. Question #16 What word do we use to describe an acid that has more than one ionizable H atom?

  33. Answer: Polyprotic

  34. Question #17 H2SO4 is a polyprotic acid. Show how this acid can go through consecutive removals of a hydrogen ion when added to water. Be sure to include states of matter.

  35. Answer: H2SO4 (aq) + H2O (l)  HSO4- (aq) + H3O+ (aq) HSO4- (aq) + H2O (l)  SO42- (aq) + H3O+ (aq)

  36. Question #18 Calculate the [OH-] concentration when the [H+] = 5.35 x 10-11 M, and determine if the solution is acidic, basic or neutral.

  37. Answer: [OH-] = 1.87 x 10-4 M; basic

  38. Question #19 A solution has the exact same [H+] and [OH-]. What is the only possible concentration for this solution? Would you classify this solution as acidic, basic or neutral?

  39. Answer: [H+] = [OH-] = 1.0 x 10-7 M; neutral

  40. Question #20 A solution has a pOH of 8.87. What is its [H+]? Would you classify this solution as acidic, basic or neutral?

  41. Answer: [H+] = 7.41 x 10-6 M; acidic

  42. Question #21 Find the pH of a 0.00476 M hydrochloric acid solution.

  43. Answer: pH = 2.32

  44. Question #22 Find the pOH of a solution that contains 3.25 g of H2SO4 dissolved in 2.75 L of solution.

  45. Answer: pOH = 12.08

  46. Question #23 If the pH = 9.85, what is the concentration of a solution of Sr(OH)2?

  47. Answer: [Sr(OH)2] = 3.54 x 10-5 M

  48. Question #24 Calculate the pOH when 12.5 mL of a 0.015 M Ca(OH)2 is diluted to 0.5 L.

  49. Answer: pOH = 3.12

  50. Question #25 An acid has a Ka value that is equal to 2.5 x 10-11. Is this acid most likely a strong acid or a weak acid? Why?

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