3. Water Solutions of Acids Universal Indicator is yellow Turn phenolphthalein colorless Turn litmus paper red React with metals to give off hydrogen gas Taste Sour

4. Water Solutions of Bases Taste bitter and feel slippery Do not react with metals Conduct electricity Turn litmus paper blue Turn phenolphthalein pink Universal Indicator is blue

5. Svante Arrhenius

6. Svante Arrhenius: Acids form hydronium ions in water while bases form hydroxide ions. Hydronium ions: [H 3 O + ] (H + combined with H 2 O) Hydroxide ions: [OH  ]

7. Hydronium Ion

8. Water Molecule O H H

9. Hydronium Ion O H H H +   + + + H3OH3O

10. Water Molecules Hydronium Ion

11. Water polarity

12. Water Molecule Oxygen Hydrogen     +

13. Water Water Molecule Oxygen Atom Hydrogen Atom     +

14.    H H O

15. Hydrogen Bond Hydrogen Bonding

16. Hydrogen Bonding H 2 O

17. Water Molecules Hydronium Ion           +    +

18. NO 3  Nitric Acid in water HNO 3 + H 2 O  NO 3  + H 3 O + H3O+H3O+

19. Svante Arrhenius: Acids form hydronium ions in water while bases form Hydronium ions: [H 3 O + ] (H + combined with H 2 O) Hydroxide ions: [OH  ] hydroxide ions

20. Hydroxide Ion O H   +  OH

21. OH  Sodium Hydroxide in water NaOH + H 2 O  Na + + OH  + H 2 O Na +

22. Hydrated Al +3 H2OH2O H2OH2O H2OH2O H2OH2O H2OH2O H2OH2O

23. Strong Acid Weak Acid Neutral Strong Base Weak Base

25. O O O O S HH

27. O O O N H

28. O O O N  NO 3  Nitrate Ion

29. Cu + 4 HNO 3  Cu(NO 3 ) 2 + 2 NO 2  + 2 H 2 O

30. The brown gas is NO 2

31. The green material is Cu(NO 3 ) 2

32. Nitric Acid is an oxidizing acid

33. Acid and Base Strength Acid strength depends on the number of hydronium ions formed per mole of acid. HNO 3 is a strong acid and HF is a weak acid. The ionization of hydrofluoric is more reversible the HNO 3 ionization. HF + H 2 O F  + H 3 O + HNO 3 + H 2 O NO 3  + H 3 O + reversible

34. Hydronium Ion Nitrate Ion 100 % Ionized Strong Acid HNO 3

35. Fluoride Ion HF Hydronium Ion Weak Acid HF Reversible

37. Cl H

38. 100 % Ionized Strong Acid

39. 100 % Ionized Strong Acid

42. O O C H Bond

43. O O C C H H H H CH 3 COOH

44. Acid and Base Strength Acid strength depends on the number of hydronium ions formed per mole of acid. HCl is a strong acid and acetic acid is a weak acid. The ionization of acetic acid is more reversible the HCl ionization. CH 3 COOH + H 2 O CH 3 COO  + H 3 O + HCl + H 2 O Cl  + H 3 O + weak acid strong acid

45. Iodide Ion Hydronium Ion 100 % ionization Strong Acid HI

46. 100 % ionization Strong Base

48. Johannes Brønsted

49. Johannes Brønsted: Definition based on what happens during an acid base reaction and is not limited to aqueous solutions. Brønsted Base A substance that accepts an H + ion (proton) from another substance Brønsted Acid A substance that donates an H + ion (proton) to another substance

50. Acid – A substance that produces hydrogen ions in water solution. HCl  H + + Cl  Acids and Bases Base – A substance that produces hydroxide ions in water solution. NaOH  Na + + OH  An acid is a proton donor. A base is a proton acceptor. Brønsted states 

51. Conjugate Acid – A particle obtained after a base has gained a proton. Conjugate Base – A particle remaining after an acid has donated a proton. Conjugate Acid and Conjugate Base Brønsted Used The Acid-Base Reaction To Define The

52. NH 3 + HCl  NH 4 + + Cl  Conjugate Acid and Conjugate Base Base Can Accept a Proton Acid Can Donate a Proton Conjugate Acid Has Accepted A Proton Conjugate Base Has Donated A Proton The Proton Is Gone !

53. Conjugate Acid and Conjugate Base Acid Conjugate Acid Base Conjugate Base HNO 3 + H 2 O  H 3 O + + NO 3 

54. HCN + SO 4  2  HSO 4  + CN  Conjugate Acid and Conjugate Base Acid Conjugate Acid Base Conjugate Base

55. Base Acid Conjugate Acid Conjugate Base