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Acids and Bases

Acids and Bases. Acids & Bases Ionization of Water pH Acid-Base Reactions. C 6 H 12 O 6. NaCl. C 6 H 12 O 6. Cl -. Na +. C 6 H 12 O 6. Na +. Cl -. Remember Electrolytes. Ionic. Covalent. H-Cl. HC 2 H 3 O 2. C 2 H 3 O 2 1-. Cl -. H +. H +. H +. H +. C 2 H 3 O 2 1-. Cl -.

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Acids and Bases

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  1. Acids and Bases • Acids & Bases • Ionization of Water • pH • Acid-Base Reactions

  2. C6H12O6 NaCl C6H12O6 Cl- Na+ C6H12O6 Na+ Cl- Remember Electrolytes Ionic Covalent

  3. H-Cl HC2H3O2 C2H3O21- Cl- H+ H+ H+ H+ C2H3O21- Cl- Acids Weak Strong Only a few Ions Lots of Ions

  4. HCl H+ + Cl- H-Cl Cl- H+ H+ Cl- Acids • Acid = gives hydrogenions in water hydrogen ion

  5. H-Cl Cl- Acids • Acid = gives hydrogenions in water H-Cl + H-O-H + Cl- hydronium ion

  6. CommonAcids • H2SO4 • HCl • H3PO4 • H2CO3 • HC2H3O2 • H3C6O7H8 • HC6O6H7 • H2C4O6H4 • H2C9O4H8 • SulfuricAcid • HydrochloricAcid • PhosphoricAcid • CarbonicAcid • AceticAcid • CitricAcid • AscorbicAcid • TartaricAcid • Acetyl SalicylicAcid • Battery Acid • Stomach Acid • Coca Cola • Carbonated Water • Vinegar • Citrus fruits • Vitamin C • Grapes • Aspirin

  7. Naming Acids • Binary Acids: • Hydrogen & non metal. • ex. HCl HBr H2S • hydro- ______________-ic Acid • HCl Hydrochloric acid • H2S Hydrosulfuric acid

  8. Naming Oxygen containing acids • Oxoacids: • Hydrogen, oxygen, and a nonmetal • ex. HNO3 HNO2 H2SO4 • The higher number of O’s • ______________-icAcid • HNO3 = Nitric Acid • The lower number of O’s • ______________ -ousending. • HNO2 = NitrousAcid

  9. THE COMMON -IC ACIDS • H2SO4SULFURIC ACID • HNO3 NITRIC ACID • H2CO3 CARBONIC ACID • H3PO4 PHOSPHORIC ACID • HClO3 CHLORIC ACID

  10. CommonAcids • H2SO4 • HCl • H3PO4 • H2CO3 • HC2H3O2 • H3C6O7H8 • HC6O6H7 • H2C4O6H4 • H2C9O4H8 Battery Acid Stomach Acid Coca Cola Carbonated Water Vinegar Citrus fruits Vitamin C Grapes Aspirin • Strong • 100% ionization • Strong electrolyte • Weak • Partial ionization • Weak electrolyte • Taste sour

  11. H-Cl HC2H3O2 Cl- HC2H3O2 H+ C2H3O21- Acids H-Cl + H-O-H + Cl- H-C2H3O2 + H-O-H + C2H3O2-

  12. H-Cl HC2H3O2 Cl- HC2H3O2 H+ H+ H+ C2H3O21- Cl- Acids Weak Strong Only a few Ions Lots of Ions

  13. NaOH Na+ + OH- NaOH Na+ OH- OH- Na+ Bases • Base=gives hydroxideions in water. • (Arrhenius definition) • =takes hydrogen ionsin water. • (Bronsted-Lowry definition)

  14. Common Bases Lye, Drano Potash Cleaners Milk of Magnesia Baking soda Tums /Rolaids Limestone, shells Soaps Detergents • NaOH • KOH • NH3 orNH4OH • Mg(OH)2 • NaHCO3 • CaCO3 • NaC16O2H31 • NaC12O4H25S • Sodium Hydroxide • Potassium Hydroxide • Ammonia • Magnesium Hydroxide • Sodium Bicarbonate • Calcium Carbonate • Sodium Palmitate • Sodium Lauryl Sulfate

  15. Common Bases Lye, Drano Potash Cleaners Milk of Magnesia Baking soda Tums /Rolaids Limestone, shells Soaps Detergents • NaOH • KOH • NH3 orNH4OH • Mg(OH)2 • NaHCO3 • CaCO3 • NaC16O2H31 • NaC12O4H25S • Strong • 100% ionization • Strong electrolyte • Weak • Partial ionization • Weak electrolyte • Taste bitter • Feel Slippery

  16. Strong Acids HClO4 H2SO4 HI HBr HCl HNO3 Perchloric Acid Sulfuric Acid HydroIodic Acid Hydrobromic Acid Hydrochloric Acid Nitric Acid Strong Bases LiOH NaOH KOH Ca(OH)2 Lithium Hydroxide Sodium Hydroxide Potassium Hydroxide Calcium Hydroxide

  17. Water is Amphoteric HNO3 • HNO3 + H2O H3O++ NO3- Acid donates a proton Base takes a proton Acid Base NH3 • NH3 + H2O NH4+ + OH- Base takes a proton Acid donates a proton Acid donates a proton Base takes a proton

  18. NH3 + H2O NH4+ + OH-

  19. Conjugate Acid - Base Pairs • H2CO3 + H2O H3O+ + HCO3- conj acid BASE conj base ACID conjugate pair conjugate pair

  20. Conjugate Acid - Base Pairs H2CO3 HCO31- CO32- Acid - Base Acid - Base H3O+ H2O HO1- Acid - Base Acid - Base H2PO41- H3PO4 HPO42- PO43- Acid - Base Acid - Base Acid - Base

  21. Ionization of Water • H2O + H2O HO- + H3O+ conjugate pair BASE conj base conj acid ACID conjugate pair

  22. Ion product constant of Water H2O + H2O HO- + H3O+ BASE conj base conj acid ACID 0.000,000,1M = 1 x 10-7M 0.000,000,1M = 1 x 10-7M Neutral: if [H3O+] = [OH-] Acidic: if [H3O+] > [OH-] Basic: if [H3O+] < [OH-]

  23. Ion product constant of Water H2O + H2O HO- + H3O+ BASE conj base conj acid ACID 0.000,000,1M = 1 x 10-7M 0.000,000,1M = 1 x 10-7M [H3O+] [OH-] = (1 x 10-7)(1 x 10-7) =1 x 10-14 Kw = [H3O+] [OH-] = 1 x 10-14

  24. pH [H+] = 1 x 10 -pH pH = - log [H+] 100 M = 1 x 10 2 M -2 Acidic 0.000,1 M = 1 x 10 -4 M 4 7 Neutral 0.000,000,001 M = 1 x 10 -9 M NH3 9 Basic 0.000,000,000,001 M = 1 x 10 -12 M 12

  25. pH [H+] = 1 x 10 -pH pH = - log [H+] 100 M = 1 x 10 2 M -2 Acidic 0.000,76 M = 7.6 x 10 -4 M Citric Acid 0.000,1 M = 1 x 10 -4 M 4 7 Neutral 0.000,000,001 M = 1 x 10 -9 M NH3 9 Basic 0.000,000,000,001 M = 1 x 10 -12 M 12

  26. pH [H+] = 1 x 10 -pH pH = - log [H+] 0.001 M = 1 x 10 -3 M 3 3 - 4 0.000,76 M = 7.6 x 10 -4 M pH = - log (7.6 x 10 -4) Citric Acid = 3.1 0.000,1 M = 1 x 10 -4 M 4

  27. pH [H+]= 1 x 10 -pH pH = - log [H+] Baking Soda = 1 x 10 -8.5 M = 3.2 x 10 -9 M 8.5 = 1 x 10 -9.4 M = 5.0 x 10 -10 M Cleaner 9.3 pH = - log (4.0 x 10 -8) 0.000,000,04 M = 4.0 x 10 -8 M Blood = 7.4

  28. pH of somecommon materials • Substance pH • 1 M HCl 0.0 • Lemon juice 2.3 • Coffee 5.0 • Pure Water 7.0 • Blood 7.35-7.45 • Milk of Magnesia 10.5 • 1M NaOH14.0

  29. pH Indicators • pH meter: Pigments: • pH paper: • Litmuspaper: • Anthocyanins: • red cabbage, cranberries, roses… • Phenolphthalein: • Turmeric:

  30. Indicator examples • Acid-base indicators undergo a color change at a known pH. phenolphthalein methyl red bromthymol blue

  31. Acid Reactions ZnCl2 + H2 • HCl + Zn  Acid Metal Salt H+ Cl- Zn

  32. potassium sodium calcium magnesium aluminum zinc chromium iron nickel tin lead copper silver platinum gold Activity series of metals Reacts violently with cold water Reacts slowly with cold water Reacts very slowly with steam but quite reactive in acid increasing reactivity Reacts moderately with high levels of acid Unreactive in acid

  33. Acid-Base Reactions NaCl + HOH • HCl + NaOH Water Acid Base Salt Neutralization: Strong Acid + Strong Base H+ Cl- Na+ OH-

  34. Acid-Base Reactions 2 2 H2SO4 + KOH K2SO4 + HOH Water Acid Base Salt SO4-2 H+ K+ OH-

  35. Acid-Base Reactions Vinegar & Baking Soda HC2H3O2 + NaHCO3 Acid Base NaC2H3O2 + H2CO3 Salt C2H3O21- H+ H2O + CO2(g) Na+ HCO31-

  36. Acid-Base Reactions Cream of Tartar & Baking Soda HC2H3O2 + NaHCO3 NaC2H3O2 + H2CO3 Acid Base Salt H2O + CO2(g) Acid Rain on Marble H2SO4 + CaCO3 CaSO4 + H2CO3 Acid Base Salt H2O + CO2(g)

  37. Acid-Base Reactions Lemon on Fish H3C6H8O7 + R-NH2 C6H8O71- + R-NH31+ Acid Base Salt

  38. Buffers • Weak acid + Weak base • Resists change in pH HC2H3O2 NaC2H3O2 HCl NaOH NaC2H3O2 + H2O NaCl + HC2H3O2

  39. pOH examples • Determine the following: • pOH = -log[OH-] • or 14 - pH • 1. pOH of 1.7x10-4 M NaOH • pOH = 3.8 pH = 10.2 • 2. pOH of 5.2x10-12 M H+ • pH = 11.2 pOH = 2.8 • 3. [OH-] , if the pH is 4.5 • pOH = 9.5 • [OH-] = 3.2x10-10 M

  40. pH scale • A log based scale used to keep track of the large change important to acids and bases. 14 7 0 10-14 M 10-7 M 1 M Very Neutral Very Basic Acidic When you add an acid, the pH gets smaller. When you add a base, the pH gets larger.

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