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Drill:

1A + 2B  1C + 1D Calculate the equilibrium concentrations of each species when 150 mL 2.5 M A is mixed with 100.0 mL 2.5 M B. K c = 2.0 x 10 -10. Drill: 1A + 2B  1C + 1D Calculate the equilibrium concentrations of each species when a solution is made with 1.0 M A &

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Drill:

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  1. 1A + 2B  1C + 1DCalculate the equilibrium concentrations of each species when 150 mL 2.5 M A is mixed with 100.0 mL 2.5 M B. Kc = 2.0 x 10-10

  2. Drill: 1A + 2B  1C + 1DCalculate the equilibrium concentrations of each species when a solution is made with 1.0 M A & 1.0 M B. Kc = 2.0 x 10-12

  3. Acid/Base

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

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

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

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

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

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

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

  11. Lewis Acid/Base H3N: + BF3 H3N-BF3 Base Acid Neutral

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

  13. Amphiprotism • Can act like an acid or a base • Can donate or accept protons

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

  15. Drill: Name each of the following:KOH HBrAl(OH)3 H2CO3HClO4 NH3

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

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

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

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

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

  21. Strong Acid/Base Ionizes 100 % (1 M) HA H+ + A- 1 M – all 1 1

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

  23. Ternary Acids • Acids containing 3 elements • H2SO4 Sulfuric acid • HNO3 Nitric acid

  24. Monoprotic Acids • Acids containing only one ionizable hydrogen • HBr Hydrobromic acid • HC2H3O2 Acetic acid

  25. Diprotic Acids • Acids containing 2 ionizable hydrogens • H2SO4 Sulfuric acid • H2CO3 Carbonic acid

  26. Triprotic Acids • Acids containing 3 ionizable hydrogens • H3PO4 Phosphoric acid • H3AsO4 Arsenic acid

  27. Polyprotic Acids • Acids containing more than one ionizable hydrogens • H4SiO4 Silicic acid • H2CO2 Carbonous acid

  28. Monohydroxic Base • A base containing only one ionizable hydroxide • NaOH Sodium hydroxide • LiOH Lithium hydroxide

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

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

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

  32. Calculate the pH of each of the following:1) [H+] = 0.040 M2) [HCl] = 0.0025 M 3) [HBr] = 0.080 M

  33. Calculate the pOH of each of the following: 1) [OH-] = 0.030 M2) [KOH] = 0.0025 M3) [NaOH] = 4.0 x 10-7 M

  34. Standard Solution • A solution with known concentration

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

  36. Titration • A method of determining the concentration of one solution by reacting it with a standard solution

  37. Titration Formula for monoprotic solutions MAVA = MBVB

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

  39. Equivalence Point • The point where the concentrations of the two solutions in the titration are equal

  40. Acid/Base Equivalence Point The point where the H+ concentration is equal to the OH- concentration

  41. Titration Fact No changes will be observed when titrating acids against bases; thus, one must use an indicator to see changes

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

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

  44. Titration Formula for monoprotic solutions MAVA = MBVB

  45. Dilution Formula M1V1 = M2V2

  46. Calculate the mL of 16.0 M HNO3 it takes to make 4.0 L of 0.100 M HNO3

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

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

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

  50. Titration Formulafor Acid/Base • NAVA = NBVB • Elliott’s Rule: • #HMAVA = #OHMBVB

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