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Acid/Base

Acid/Base. Properties of Acids. Sour taste, Change color of dyes, Conduct electricity in solution, React with many metals, React with bases to form salts. Properties of Bases. Bitter taste, Feel slippery, Change color of dyes, Conduct electricity in solution, React with acids to form salts.

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Acid/Base

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  1. Acid/Base

  2. Properties of Acids • Sour taste, Change color of dyes, Conduct electricity in solution, React with many metals, React with bases to form salts

  3. Properties of Bases • Bitter taste, Feel slippery, Change color of dyes, Conduct electricity in solution, React with acids to form salts

  4. Arrhenius • Acids: release H+ or H3O+ in solution • Bases: release OH- in solution

  5. Arrhenius • Acid: HA --> H+ + A- • HCl --> H+ + Cl- • Base: MOH --> M+ + OH- • NaOH -->Na+ + OH-

  6. Bronsted-Lowry • Acid: Proton donor • Base: Proton Acceptor

  7. Bronsted-Lowry • HA + H2O --> H3O+ + A- • HI + H2O --> H3O+ + I- • Acid Base CACB • NH3 + H2O --> NH4+ + OH- • Base Acid CA CB

  8. Lewis Acid/Base • Acid: Electron Acceptor • Base: Electron Donor

  9. Lewis Acid/Base • H3N: + BF3 --> H3N-BF3 • Base Acid Neutral

  10. Common Names • H+ Hydrogen ion • H3O+ Hydronium ion • H- Hydride ion • OH- Hydroxide ion • NH3 Ammonia • NH4+ Ammonium ion

  11. Amphoterism • Can act like an acid or a base • Can donate or accept protons

  12. Define acids & bases by each of the three methods

  13. Naming Acids • All acids are H-anion • If the anion is: • -ides  hydro___ic acids • -ates  ___ic acids • -ites  ___ous acids

  14. Naming Bases • Almost all bases are metal hydroxides • Name by normal method • Ammonia (NH3) as well as many amines are bases

  15. Strong Acids or Bases • Strong acids or bases ionize 100 % in solution • Weak acids or bases ionize <100 % in solution

  16. Strong Acids • HClO4 Perchloric acid • H2SO4 Sulfuric acid • HNO3 Nitric acid • HCl Hydrochloric acid • HBr Hydrobromic acid • HI Hydroiodic acid

  17. Strong Bases • All column I hydroxides • Ca(OH)2 Calcium hydroxide • Sr(OH)2 Strontium hydroxide • Ba(OH)2 Barium hydroxide

  18. Name & give the formula for at least 4 each of strong acids & strong bases

  19. Binary Acids • Acids containing only 2 elements • HCl Hydrochloric acid • H2S Hydrosulfuric acid

  20. Ternary Acids • Acids containing 3 elements • H2SO4 Sulfuric acid • H2SO3 Sulfurous acid • HNO3 Nitric acid

  21. Monoprotic Acids • Acids containing only one ionizable hydrogen • HBr Hydrobromic acid • HCN Hydrocyanic acid • HC2H3O2 Acetic acid

  22. Diprotic Acids • Acids containing 2 ionizable hydrogens • H2SO4 Sulfuric acid • H2SO3 Sulfurous acid • H2CO3 Carbonic acid

  23. Triprotic Acids • Acids containing 3 ionizable hydrogens • H3PO4 Phosphoric acid • H3PO3 Phosphorus acid • H3AsO4 Arsenic acid

  24. Polyprotic Acids • Acids containing more than one ionizable hydrogens • H2SO4 Sulfuric acid • H4SiO4 Silicic acid • H2CO2 Carbonous acid

  25. Monohydroxic Base • A base containing only one ionizable hydroxide • NaOH Sodium hydroxide • KOH Potassium hydro. • LiOH Lithium hydroxide

  26. Neutralization Rxn • A reaction between an acid & a base making salt & H2O • HA(aq) + MOH(aq) •  MA(aq) + H2O(l)

  27. Neutralization Rxn • HCl(aq) + NaOH(aq) •  • NaCl(aq) + H2O(l)

  28. Drill: Identify: acid, base, CA, & CB • HCO3- + H2O • H2CO3 + OH-

  29. Work problems 1 – 6 on page 395

  30. Titration • A method of determining the concentration of one solution by reacting it with a standard solution • MAVA = MBVB for monoprotics

  31. Standard Solution • A solution with known concentration

  32. Titration • When titrating acids against bases, the end point of the titration is at the equivalence point

  33. Make Calculations • Calculate the molarity of 25.0 mL HCl when it’s titrated to its equivalence point with 50.0 mL 0.200 M NaOH

  34. Equivalence Point • The point where the H+ concentration is equal to the OH- concentration

  35. Indicator • An organic dye that changes color when the pH changes

  36. Make Calculations • Calculate the mL of 12.5 M HCl required to make 2.5 L of 0.200 M HCl

  37. Molarity • Moles of solute per liter of solution (M)

  38. Normality • Number of moles of hydrogen or hydroxide ions per liter of solution (N)

  39. Titration Formula • NAVA = NBVB • Elliott’s Rule: • #HMAVA = #OHMBVB

  40. Make Calculations • Calculate the molarity of 30.0 mL H2CO3 when it’s titatrated to its equivalence point with 75.0 mL 0.200 M NaOH

  41. Make Calculations • Calculate the molarity of 40.0 mL H3PO4 when it’s titatrated to its equivalence point with 30.0 mL 0.20 M Ba(OH)2

  42. Calculate the volume of 0.250 M HCl needed to titrate 50.00 mL 0.200 M NaOH to its equivalence point

  43. Calculate the molarity 25.0 mL H3PO4 that neutralizes 50.00 mL 0.200 M Ca(OH)2 to its equivalence point

  44. Drill: Calculate the volume of 0.10 M H3PO4 that neutralizes 50.00 mL 0.200 M Ca(OH)2 to its equivalence point

  45. pH • The negative log of the hydrogen or hydronium ion concentration • pH = -log[H+] • pOH = -log[OH-]

  46. Calculate the pH of:1) [H+] = 0.040 M2) [HCl] = 0.0025 M3) [HBr] = 0.080 M

  47. Calculate the pOH of: 1) [OH-] = 0.030 M2) [KOH] = 0.0025 M3) [NaOH] = 4.0 x 10-5 M

  48. Titration Curve:Strong acid vs strong base

  49. Titration Curve:Strong acid vs strong base; then weak acid vs strong base

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