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Acids Lesson 22 Subtle Items

Acids Lesson 22 Subtle Items. 1. Weak bases neutralize a strong acid as well as a strong base would. Subtle Acid Items 1. Weak bases neutralize a strong acid as well as a strong base would.  HCl + NaOH . Subtle Acid Items

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Acids Lesson 22 Subtle Items

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  1. Acids Lesson 22 Subtle Items

  2. 1.Weak bases neutralize a strong acid as well as a strong base would.

  3. Subtle Acid Items 1.Weak bases neutralize a strong acid as well as a strong base would.  HCl + NaOH

  4. Subtle Acid Items 1.Weak bases neutralize a strong acid as well as a strong base would. HCl + NaOH → NaCl + HOH

  5. Subtle Acid Items 1.Weak bases neutralize a strong acid as well as a strong base would.  HCl + NaOH → NaCl + HOH HCl + HCO3-

  6. Subtle Acid Items 1.Weak bases neutralize a strong acid as well as a strong base would. HCl + NaOH → NaCl + HOH HCl + HCO3- → H2CO3 + Cl-

  7. Subtle Acid Items 1.Weak bases neutralize a strong acid as well as a strong base would. HCl + NaOH → NaCl + HOH HCl + HCO3- → H2CO3 + Cl- Both reactions go to completion because of the strong acid.

  8. 2. H3BO3

  9. 2. H3BO3triprotic

  10. 2. H3BO3triprotic H3BO3⇌ H+ + H2BO3-

  11. 2. H3BO3triprotic H3BO3⇌ H+ + H2BO3- H2CO3

  12. 2. H3BO3triprotic H3BO3⇌ H+ + H2BO3- H2CO3diprotic

  13. 2. H3BO3triprotic H3BO3⇌ H+ + H2BO3- H2CO3diprotic H2CO3 ⇌ H+ + HCO3-

  14. 2. H3BO3triprotic H3BO3⇌ H+ + H2BO3- H2CO3diprotic H2CO3 ⇌ H+ + HCO3- HCl

  15. 2. H3BO3triprotic H3BO3⇌ H+ + H2BO3- H2CO3diprotic H2CO3 ⇌ H+ + HCO3- HCl monoprotic

  16. 2. H3BO3triprotic H3BO3⇌ H+ + H2BO3- H2CO3diprotic H2CO3 ⇌ H+ + HCO3- HCl monoprotic HCl → H+ + Cl-

  17. 2. H3BO3triprotic H3BO3⇌ H+ + H2BO3- H2CO3diprotic H2CO3 ⇌ H+ + HCO3- HCl monoprotic HCl → H+ + Cl- Only lose one proton when in water! However,

  18. 2. H3BO3triprotic H3BO3⇌ H+ + H2BO3- H2CO3diprotic H2CO3 ⇌ H+ + HCO3- HCl monoprotic HCl → H+ + Cl- Only lose one proton when in water! However, H3BO3 + NaOH

  19. 2. H3BO3triprotic H3BO3⇌ H+ + H2BO3- H2CO3diprotic H2CO3 ⇌ H+ + HCO3- HCl monoprotic HCl → H+ + Cl- Only lose one proton when in water! However, loses all three because of the strong base! H3BO3 + 3NaOH → Na3BO3 + 3HOH

  20. 2. H3BO3triprotic H3BO3⇌ H+ + H2BO3- H2CO3diprotic H2CO3 ⇌ H+ + HCO3- HCl monoprotic HCl → H+ + Cl- Only lose one proton when in water! However, loses all three because of the strong base! H3BO3 + 3NaOH → Na3BO3 + 3HOH HCl + NaOH →

  21. 2. H3BO3triprotic H3BO3⇌ H+ + H2BO3- H2CO3diprotic H2CO3 ⇌ H+ + HCO3- HCl monoprotic HCl → H+ + Cl- Only lose one proton when in water! However, loses all three because of the strong base! H3BO3 + 3NaOH → Na3BO3 + 3HOH HCl + NaOH → NaCl + HOH

  22. 2. H3BO3triprotic H3BO3⇌ H+ + H2BO3- H2CO3diprotic H2CO3 ⇌ H+ + HCO3- HCl monoprotic HCl → H+ + Cl- Only lose one proton when in water! However, loses all three because of the strong base! H3BO3 + 3NaOH → Na3BO3 + 3HOH HCl + NaOH → NaCl + HOH Which neutralizes more NaOH, H3BO3 or HCl?

  23. 2. H3BO3triprotic H3BO3⇌ H+ + H2BO3- H2CO3diprotic H2CO3 ⇌ H+ + HCO3- HCl monoprotic HCl → H+ + Cl- Only lose one proton when in water! However, loses all three because of the strong base! H3BO3 + 3NaOH → Na3BO3 + 3HOH HCl + 1NaOH → NaCl + HOH Which neutralizes more NaOH? H3BO3 or HCl?

  24. 3. Which determines acid strength? Molarity pH = Ka

  25. 3. Which determines acid strength? Molarity is concentration. pH = Ka

  26. 3. Which determines acid strength? Molarity is concentration. pH = -Log[H+] Ka

  27. 3. Which determines acid strength? Molarity is concentration. pH = -Log[H+] Ka is strength as indicated in the acid chart

  28. 4. Which determines the pH. Ka Molarity Temperature

  29. 4. Which determines the pH = -Log[H+] Ka Molarity Temperature

  30. 4. Which determines the pH = -Log[H+] Ka determines the [H+] and the pH Molarity Temperature

  31. 4. Which determines the pH = -Log[H+] Ka determines the [H+] and the pH Molarity determines the [H+] and the pH Temperature

  32. 4. Which determines the pH = -Log[H+] Ka determines the [H+] and the pH Molarity determines the [H+] and the pH Temperaturedetermines the [H+] and the pH

  33. 5. Pick the best conductor. 1 M NaOH 0.1 M HCl 0.01 M KOH

  34. 5. Pick the best conductor. 1 M NaOH 0.1 M HCl 0.01 M KOH All strong- highest Molarity!

  35. 6. Pick the worst conductor. NaOH HCl NaCN NH3

  36. 6. Pick the worst conductor. NaOH HCl NaCN NH3

  37. 6. Pick the worst conductor. NaOH HCl NaCN NH3 Good Conductors are….. Strong acids Strong Bases Soluble Salts

  38. 1 mole H2CO3 and 1mole NaHCO3 are dissolved in • 0.5 L of water.   What kind of solution results in the above mixture? Buffer Write an equation for the equilibrium. H2CO3⇋ H+ + HCO3- Label each chemical species with a concentration. 2 M Low 2 M What limits the ability to buffer against acid? [HCO3-] What limits the ability to buffer against base? [H2CO3]

  39. 8. Acid Base   HF

  40. 8. Acid Base   HF F-

  41. 8. Acid Base   HF F- H2BO3-

  42. 8. Acid Base   HF F- H3BO3 H2BO3-

  43. 8. Acid Base   HF F- H3BO3 H2BO3- HCN

  44. 8. Acid Base   HF F- H3BO3 H2BO3- HCN CN-

  45. 8. Acid Base   HF F- H3BO3 H2BO3- HCN CN- Put an asterisk next to the strongest acid and base

  46. 8. Acid Base * HF F- H3BO3 H2BO3- HCN CN- Put an asterisk next to the strongest acid and base

  47. 8. Acid Base * HF F- H3BO3 H2BO3- HCN CN- * Put an asterisk next to the strongest acid and base

  48. 8. Acid Base * HF F- H3BO3 H2BO3- HCN CN- * Put an asterisk next to the strongest acid and base What is the relationship between acid strength and strength of conjugate base?

  49. 8. Acid Base * HF F- H3BO3 H2BO3- HCN CN- * Put an asterisk next to the strongest acid and base What is the relationship between acid strength and strength of conjugate base? Inverse

  50. 9. What ions are in H2SO4 solution? H2SO4

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