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Ch19.1 – Acids and Bases Acids - corrosive, taste sour, put electrolytes in soln , react with metals Ex1) S

Ch19.1 – Acids and Bases Acids - corrosive, taste sour, put electrolytes in soln , react with metals Ex1) Single displacement reaction: H 2 SO 4( aq ) + Zn (s) →. Ch19.1 – Acids and Bases Acids - corrosive, taste sour, put electrolytes in soln , react with metals

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Ch19.1 – Acids and Bases Acids - corrosive, taste sour, put electrolytes in soln , react with metals Ex1) S

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  1. Ch19.1 – Acids and Bases Acids - corrosive, taste sour, put electrolytes in soln, react with metals Ex1) Single displacement reaction: H2SO4(aq) + Zn(s)→

  2. Ch19.1 – Acids and Bases Acids - corrosive, taste sour, put electrolytes in soln, react with metals Ex1) Single displacement reaction: H2SO4(aq) + Zn(s)→ ZnSO4(aq) + H2(g) - produce hydrogen ions when dissolved in water. Ex2) Decomposition: HCl(s)→

  3. Ch19.1 – Acids and Bases Acids - corrosive, taste sour, put electrolytes in soln, react with metals Ex1) Single displacement reaction: H2SO4(aq) + Zn(s)→ ZnSO4(aq) + H2(g) - produce hydrogen ions when dissolved in water. Ex2) Decomposition: HCl(s)→ H+(aq) + Cl-(aq) What actually happens is the H+ bonds with water: HCl(s) + H(OH) →

  4. Acids - corrosive, taste sour, put electrolytes in soln, react with metals Ex1) Single displacement reaction: H2SO4(aq) + Zn(s)→ ZnSO4(aq) + H2(g) - produce hydrogen ions when dissolved in water. Ex2) Decomposition: HCl(s)→ H+(aq) + Cl-(aq) What actually happens is the H+ bonds with water: HCl(s) + H(OH) → H3O+(aq) + Cl-(aq) - will cause some substances (called indicators) to change colors in presence of acid

  5. Naming acids 1. Salt that ends in –ide, name acid by putting hydro in front, use the root of the anion, and end it with –ic Ex1) HCl(s):

  6. Naming acids 1. Salt that ends in ide, name acid by putting hydro in front, use the root of the anion, and end it with ic Ex1) HCl(s): hydrogen chloride  hydrochloric acid 2. Polyatomic ions in salts, if ion ends in ate, then give it the ending ic Ex2) H2SO4(s):

  7. Naming acids 1. Salt that ends in ide, name acid by putting hydro in front, use the root of the anion, and end it with ic Ex1) HCl(s): hydrogen chloride  hydrochloric acid 2. Polyatomic ions in salts, if ion ends in ate, then give it the ending ic Ex2) H2SO4(s): hydrogen sulfate  sulfuric acid 3. Polyatomic ions in salts, if ion ends in ite, then give it the ending ous Ex3) H2SO3(s):

  8. Naming acids 1. Salt that ends in ide, name acid by putting hydro in front, use the root of the anion, and end it with ic Ex1) HCl(s): hydrogen chloride  hydrochloric acid 2. Polyatomic ions in salts, if ion ends in ate, then give it the ending ic Ex2) H2SO4(s): hydrogen sulfate  sulfuric acid 3. Polyatomic ions in salts, if ion ends in ite, then give it the ending ous Ex3) H2SO3(s): hydrogen sulfite  sulfurous acid 4. Polyatomic one above most common, add per in front Ex4) H2SO5(s):

  9. Naming acids 1. Salt that ends in ide, name acid by putting hydro in front, use the root of the anion, and end it with ic Ex1) HCl(s): hydrogen chloride  hydrochloric acid 2. Polyatomic ions in salts, if ion ends in ate, then give it the ending ic Ex2) H2SO4(s): hydrogen sulfate  sulfuric acid 3. Polyatomic ions in salts, if ion ends in ite, then give it the ending ous Ex3) H2SO3(s): hydrogen sulfite  sulfurous acid 4. Polyatomic one above most common, add per in front Ex4) H2SO5(s): hydrogen persulfate persulfuric acid 5. Polyatomic two below most common, add hypo in front Ex5) H2SO2(s):

  10. Naming acids 1. Salt that ends in ide, name acid by putting hydro in front, use the root of the anion, and end it with ic Ex1) HCl(s): hydrogen chloride  hydrochloric acid 2. Polyatomic ions in salts, if ion ends in ate, then give it the ending ic Ex2) H2SO4(s): hydrogen sulfate  sulfuric acid 3. Polyatomic ions in salts, if ion ends in ite, then give it the ending ous Ex3) H2SO3(s): hydrogen sulfite  sulfurous acid 4. Polyatomic one above most common, add per in front Ex4) H2SO5(s): hydrogen persulfate persulfuric acid 5. Polyatomic two below most common, add hypo in front Ex5) H2SO2(s): hydrogen hyposulfite  hyposulfurous acid

  11. Exs: HF HNO3 HNO2 H2CO3 H2S HCLO3 HCLO4 HCLO2 HCLO

  12. Bases - corrosive, taste bitter (like aspirin), produce electrolytes, - put hydroxide ions in solution Ex: Decomposition: NaOH(S)

  13. Bases - corrosive, taste bitter (like aspirin), produce electrolytes, - put hydroxide ions in solution Ex: Decomposition: NaOH(S) Na+(aq) + OH-(aq) - react with the acids to form water and a salt Ex: Double displacement (neutralization): HCl(aq) + NaOH(aq) - cause indicators to change color

  14. Bases - corrosive, taste bitter (like aspirin), produce electrolytes, - put hydroxide ions in solution Ex: Decomposition: NaOH(S) Na+(aq) + OH-(aq) - react with the acids to form water and a salt Ex: Double displacement (neutralization): HCl(aq) + NaOH(aq) NaCl(aq) + H(OH)(l) - cause indicators to change color Naming Bases Ex: Ca(OH)2:

  15. Bases - corrosive, taste bitter (like aspirin), produce electrolytes, - put hydroxide ions in solution Ex: Decomposition: NaOH(S) Na+(aq) + OH-(aq) - react with the acids to form water and a salt Ex: Double displacement (neutralization): HCl(aq) + NaOH(aq) NaCl(aq) + H(OH)(l) - cause indicators to change color Naming Bases Ex: Ca(OH)2: calcium hydroxide Ch19 HW#1 1 – 3

  16. Lab19.1 – Characteristics of Acids - due in 2 days - Ch19 HW#1 due at beginning of period

  17. Ch19 HW#1 1-3 1. ID Acid, Base, both a) bitter taste b) electrolyte c) indicator color change d) sour taste e) reacts with metal from H2(g) 2. Name a) HF b) H2PO4 c) KOH d) H2SO4 e) HNO2 f) Mg(OH)2

  18. Ch19 HW#1 1-3 1. ID Acid, Base, both a) bitter taste b) electrolyte c) indicator color change base both both d) sour taste e) reacts with metal from H2(g) acid acid 2. Name a) HF (Must get 3 b) H2PO4 out of 6 for c) KOH candy) d) H2SO4 e) HNO2 f) Mg(OH)2

  19. Ch19 HW#1 1-3 1. ID Acid, Base, both a) bitter taste b) electrolyte c) indicator color change base both both d) sour taste e) reacts with metal from H2(g) acid acid 2. Name a) HF (hydrogen fluoride)  b) H2PO4(hydrogen phosphate)  c) KOH  d) H2SO4(hydrogen sulfate)  e) HNO2(hydrogen nitrite)  f) Mg(OH)2

  20. Ch19 HW#1 1-3 1. ID Acid, Base, both a) bitter taste b) electrolyte c) indicator color change base both both d) sour taste e) reacts with metal from H2(g) acid acid 2. Name a) HF (hydrogen fluoride)  hydrofluoric acid b) H2PO4(hydrogen phosphate)  c) KOH  d) H2SO4(hydrogen sulfate)  e) HNO2(hydrogen nitrite)  f) Mg(OH)2

  21. Ch19 HW#1 1-3 1. ID Acid, Base, both a) bitter taste b) electrolyte c) indicator color change base both both d) sour taste e) reacts with metal from H2(g) acid acid 2. Name a) HF (hydrogen fluoride)  hydrofluoric acid b) H2PO4(hydrogen phosphate)  phosphoric acid c) KOH  d) H2SO4(hydrogen sulfate)  e) HNO2(hydrogen nitrite)  f) Mg(OH)2

  22. Ch19 HW#1 1-3 1. ID Acid, Base, both a) bitter taste b) electrolyte c) indicator color change base both both d) sour taste e) reacts with metal from H2(g) acid acid 2. Name a) HF (hydrogen fluoride)  hydrofluoric acid b) H2PO4(hydrogen phosphate)  phosphoric acid c) KOH  potassium hydroxide d) H2SO4(hydrogen sulfate)  e) HNO2(hydrogen nitrite)  f) Mg(OH)2

  23. Ch19 HW#1 1-3 1. ID Acid, Base, both a) bitter taste b) electrolyte c) indicator color change base both both d) sour taste e) reacts with metal from H2(g) acid acid 2. Name a) HF (hydrogen fluoride)  hydrofluoric acid b) H2PO4(hydrogen phosphate)  phosphoric acid c) KOH  potassium hydroxide d) H2SO4(hydrogen sulfate)  sulfuric acid e) HNO2(hydrogen nitrite)  f) Mg(OH)2

  24. Ch19 HW#1 1-3 1. ID Acid, Base, both a) bitter taste b) electrolyte c) indicator color change base both both d) sour taste e) reacts with metal from H2(g) acid acid 2. Name a) HF (hydrogen fluoride)  hydrofluoric acid b) H2PO4(hydrogen phosphate)  phosphoric acid c) KOH  potassium hydroxide d) H2SO4(hydrogen sulfate)  sulfuric acid e) HNO2(hydrogen nitrite)  nitrous acid f) Mg(OH)2

  25. Ch19 HW#1 1-3 1. ID Acid, Base, both a) bitter taste b) electrolyte c) indicator color change base both both d) sour taste e) reacts with metal from H2(g) acid acid 2. Name a) HF (hydrogen fluoride)  hydrofluoric acid b) H2PO4(hydrogen phosphate)  phosphoric acid c) KOH  potassium hydroxide d) H2SO4(hydrogen sulfate)  sulfuric acid e) HNO2(hydrogen nitrite)  nitrous acid f) Mg(OH)2 magnesium hydroxide

  26. 3.Formulas a) chromic acid b) iron (II) hydroxide c) hydroiodic acid d) lithium hydroxide e) chlorous acid f) perchloric acid

  27. 3.Formulas a) chromic acid chromate: CrO4-2 H2CrO4 b) iron (II) hydroxide Fe+2 (OH)-1 Fe(OH)2 c) hydroiodic acid H+ I-1 HI d) lithium hydroxide e) chlorous acid f) perchloric acid

  28. 3.Formulas a) chromic acid chromate: CrO4-2 H2CrO4 b) iron (II) hydroxide Fe+2 (OH)-1 Fe(OH)2 c) hydroiodic acid H+ I-1 HI d) lithium hydroxide Li+ OH- LiOH e) chlorous acid chlorite: ClO2-1 HClO2 f) perchloric acid perchlorate: ClO4-1 HClO4

  29. Ch19.2 – Kw (The Equilibriium Constant for Water) - Water molecules collide, sometimes hydrogens are knocked off:

  30. Ch19.2 – Kw (The Equilibriium Constant for Water) - Water molecules collide, sometimes hydrogens are knocked off: This is the self-ionization of water, doesn’t happen very much. For water @ 25˚ with a neutral pH: [H3O]+ = 1x10-7M [OH]- = 1x10-7M

  31. Ch19.2 – Kw (The Equilibriium Constant for Water) - Water molecules collide, sometimes hydrogens are knocked off: This is the self-ionization of water, doesn’t happen very much. For water @ 25˚ with a neutral pH: [H3O]+ = 1x10-7M [OH]- = 1x10-7M Their combined concentration, when multiplied = 1x10-14M [H]+. [OH]- = 1x10-14M This stays constant! Which means if one gets bigger, the other gets smaller to keep constant. Another name for [H3O]+is just [H+], which is what we recognize as an acid.

  32. Their combined concentration, when multiplied = 1x10-14M [H]+. [OH]- = 1x10-14M This stays constant! Which means if one gets bigger, the other gets smaller to keep constant. Neutral water has both acid & base in it, but they’re in small amounts and cancel each other. When [H+] > 1 x 10-7 then [OH-] < 1 x 10-7Acidic When [H+] < 1 x 10-7 then [OH-] > 1 x 10-7 Basic

  33. Ex1) A solution has [H+] = 2.7x10-3M. Is it acidic, basic, or neutral? What is the [OH-] concentration?

  34. Ex1) A solution has [H+] = 2.7x10-3M. Is it acidic, basic, or neutral? What is the [OH-] concentration? Acidic[H]+. [OH]- = 1x10-14M [2.7x10-3]. [OH]- = 1x10-14M [OH]- = 3.7x10-12M Ex2) If [H+] = 1.1x10-10M, is the solution acid, basic, neutral? Find [OH-]

  35. Ex1) A solution has [H+] = 2.7x10-3M. Is it acidic, basic, or neutral? What is the [OH-] concentration? Acidic[H]+. [OH]- = 1x10-14M [2.7x10-3]. [OH]- = 1x10-14M [OH]- = 3.7x10-12M Ex2) If [H+] = 1.1x10-10M, is the solution acid, basic, neutral? Find [OH-] Basic [H+] . [OH-] = 1x10-14 [1.1x10-10] [OH-] = 1x10-14 [OH-] = 9.1x10-5M Ex3) If [OH-] = 4.4x10-8 M, acidic, basic, neutral? find [H+]

  36. Ex1) A solution has [H+] = 2.7x10-3M. Is it acidic, basic, or neutral? What is the [OH-] concentration? Acidic[H]+. [OH]- = 1x10-14M [2.7x10-3]. [OH]- = 1x10-14M [OH]- = 3.7x10-12M Ex2) If [H+] = 1.1x10-10M, is the solution acid, basic, neutral? Find [OH-] Basic [H+] . [OH-] = 1x10-14 [1.1x10-10] [OH-] = 1x10-14 [OH-] = 9.1x10-5M Ex3) If [OH-] = 4.4x10-8 M, acidic, basic, neutral? find [H+] [H+].[OH-] = 1x10-14 [H+][4.4x10-8] = 1x10-14 [H+] = 2.3x10-7 (slightly acidic) Ch19 HW#2 4 – 7

  37. Ch19 HW#2 4 – 7 4) Concentration of [H+] & [OH-] in: a) A basic solution: b) An acidic soln: c) A neutral soln: 5) Classify: a) [H+] = 6x10-10M b) [OH-] = 3x10-2M c) [H+] = 2x10-7M d) [OH-] = 1x10-7M

  38. Ch19 HW#2 4 – 7 4) Concentration of [H+] & [OH-] in: a) A basic solution:[OH-] > 1x10-7M, [H+] < 1x10-7M b) An acidic soln: [H+] > 1x10-7M, [OH-] < 1x10-7M c) A neutral soln: [H+] = 1x10-7M, [OH-] = 1x10-7M 5) Classify: a) [H+] = 6x10-10M b) [OH-] = 3x10-2M c) [H+] = 2x10-7M d) [OH-] = 1x10-7M

  39. Ch19 HW#2 4 – 7 4) Concentration of [H+] & [OH-] in: a) A basic solution:[OH-] > 1x10-7M, [H+] < 1x10-7M b) An acidic soln: [H+] > 1x10-7M, [OH-] < 1x10-7M c) A neutral soln: [H+] = 1x10-7M, [OH-] = 1x10-7M 5) Classify: a) [H+] = 6x10-10M Basic b) [OH-] = 3x10-2M Basic c) [H+] = 2x10-7M Slightly acidic d) [OH-] = 1x10-7M Neutral

  40. 6) [OH-] = 1x10-3M. Find [H+] • 7) [H+] = 3x10-6M. Find [OH-]

  41. 6) [OH-] = 1x10-3M. Find [H+] • [H+].[OH-] = 1x10-14 • [H+][1x10-3] = 1x10-14 • [H+] = 1x10-11(Basic) • 7) [H+] = 3x10-6M. Find [OH-]

  42. 6) [OH-] = 1x10-3M. Find [H+] • [H+].[OH-] = 1x10-14 • [H+][1x10-3] = 1x10-14 • [H+] = 1x10-11(Basic) • 7) [H+] = 3x10-6M. Find [OH-] • [H]+. [OH]- = 1x10-14M • [3x10-6]. [OH]- = 1x10-14M • [OH]- = 3x10-9M (Acidic)

  43. Ch19.3 – It Time for Log! (pH Calculations)

  44. Ch19.3 – It Time for Log! (pH Calculations)

  45. Ch19.3 – It Time for Log! (pH Calculations) pH Info

  46. pH Info • Ex 1) The hydrogen-ion concentration of a solution is 1x10-10 mol/L. What is the pH of the solution • Ex 2) Given [H+] = 9.27x10-12M, find pH and pOH. • Ex3) The pH of a solution is 6.0. Find [H+] for this solution.

  47. pH Info • Ex 1) The hydrogen-ion concentration of a solution is 1x10-10 mol/L. What is the pH of the solution • pH = -log[H3O+] • pH = -log[1x10-10M] • pH = 10 (Basic) • Ex 2) Given [H+] = 9.27x10-12M, find pH and pOH. • pH = -log[H3O+] pH + pOH = 14 • pH = -log[9.27x10-12M] 11.033 + pOH = 14 • pH = 11.033 (Basic) pOH = 2.967 • This is power This is sig digs • of ten for logs • Ex3) The pH of a solution is 6.0. Find [H+] for this solution.

  48. Ex3) The pH of a solution is 6.0. Find [H+] for this solution. Ex4) Given [H3O+] = 4.28x10-7M, find pH, pOH, and [OH-].

  49. Ex3) The pH of a solution is 6.0. Find [H+] for this solution. pH = -log[H3O+] 6.0 = -log[H3O+] [H3O+] = 1x10-6M Ex4) Given [H3O+] = 4.28x10-7M, find pH, pOH, and [OH-]. pH = -log[H+] pH = -log[4.28 x10-7] pH = 6.37 pH + pOH = 14 6.37 + pOH = 14 pOH = 7.63 [H+][OH-] = 1x10-14 [4.28 x10-7][OH-] = 1x10-14 [OH-] = 2.34 x10-8 M Ch19 HW#3 8 – 11

  50. Ch19 HW#3 8 – 11 8. Determine pH: a) [H+] = 1x10-6M b) [H+] = 0.0001m pH = -log(1x10-6) pH = -log(.0001) pH = pH = c) [OH-] = 1x10-2m d) [OH-] = 1x10-11 pOH = -log(1x10-2) pOH = -log(1x10-11) pOH = pOH = pH = pH =

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