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Entry Task : Sept 17 th Monday

Entry Task : Sept 17 th Monday. Question: Provide the 7 strong acids. You have 5 minutes!. Agenda. Sign off and discuss 4.3 notes. Agenda. Discuss Acid/Base notes and along the way- answer the exercise questions Self check- if you can’t do it you need to seek help!

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Entry Task : Sept 17 th Monday

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  1. Entry Task: Sept 17th Monday Question: Provide the 7 strong acids. You have 5 minutes!

  2. Agenda Sign off and discuss 4.3 notes

  3. Agenda • Discuss Acid/Base notes and along the way- answer the exercise questions • Self check- if you can’t do it you need to seek help! • Might finish lecture- if not, continue next time • HW: Acid/Gas formation reaction ws.

  4. Acid-Base Reactions All this acid rain is killing my complexion! Acids: • Ionize in H2O, causes increase in H+ ions. • H+ ions are bare protons. • Acids are proton donors.

  5. Monoprotic Acids: (HCl, HNO3) • Acids that can only yield one H+ per molecule upon ionization. HCl  H+ + Cl-

  6. Diprotic Acids: (H2SO4) • Ionization occurs in 2 steps. • Only the first ionization is complete.

  7. Is HF a weak or strong acid? weak acid Although it is a weak acid, this acid is extremely reactive because of the F- ion. Must be kept in special polypropylene container because it eats through glass. Used to etch glass. Has caused major accidents in lab.

  8. Bases • Substances that increase the OH- when added to water. (NaOH) • NH3 is a base. In water it accepts an H+ ion from HOH, leaving an OH- in solution. • NH3 is a weak electrolyte • About 1% ionizes to form NH4+/OH-

  9. Strong acids and bases • Acids and bases that ionize completely in solution are strong acids and bases. • Those that only ionize partially are weak acids and bases. • You must memorize these.

  10. Strong Acids Hydrochloric Acid – Hydrobromic Acid – Hydroiodic Acid – Nitric Acid – Sulfuric Acid – Chloric Acid – Perchloric Acid – HCl HBr HI HNO3 H2SO4 HClO3 HClO4

  11. Strong Bases All group 1 Metal Hydroxides (LiOH, NaOH, KOH, RbOH, CsOH) Heavy Group 2 Metal Hydroxides Ca(OH)2, Sr(OH)2, Ba(OH)2

  12. Once you memorize the strong acids and bases, you will have enough information to determine if a substance is a strong or weak electrolyte.

  13. Dichotomous key to Electrolyte • Ionic or Molecular • Has a metal in front (ionic)……………….. Strong electrolyte • Nonmetal in front (including H)………………….. Go to 2 • Has Hydrogen in front • Yes- acid……………………………………………………….Go to 3 • No- not an acid…………………………………………….Go to 4 • Acids • On the strong acid list…………………….. Strong electrolyte • Not a strong acid……………………….………Weak electrolyte • Other • Is NH3……………………………………….. Weak electrolyte • Not NH3………………………………………Non-electrolyte

  14. Example problems: KF Na3PO4 NH3 CH3CH2OH HCl NO2 HC2H3O2 CH4 NH4Cl CH3Cl strong electrolyte strong electrolyte weak electrolyte nonelectrolyte strong electrolyte nonelectrolyte weak electrolyte nonelectrolyte strong electrolyte nonelectrolyte

  15. 4-19 Classify the following as Strong acid, Strong base, weak acid or base SB c. LiOH SA a. HClO4 WB d. NH3 WA b. HClO2 4-20 Classify the following as Strong acid, Strong base, weak acid or base SA c. HBr WA a. H2CO3 d. HC7H3O2 WA SB b. Ca(OH)2

  16. 4-25 Classify the following as a non-electrolyte, weak electrolyte or strong electrolyte in water WE c. NH3 SE a. H2SO4 SE e. Cu(NO3)2 SE d. KClO3 No E • C2H5OH 4-26 Classify the following as Strong acid, Strong base, weak acid or base SE No E c. KOH e. C12H22O11 WE a. HBrO No E f. O2 d. CoSO4 WE SE b. HNO3

  17. Acid Properties Sour taste Turn blue litmus red pH < 7 Base properties Bitter taste Turns red litmus blue pH >7 slippery Some Properties of Acids and Bases

  18. Acid + Base Neutralization • Products of a neutralization reaction have none of the properties of an acid or a base. • An acid reacts with a metal hydroxide to form a salt plus water.

  19. Neutralization Reactions • Acid + Base (Metal Hydroxide) Salt + Water • HCl(aq) + NaOH(aq)  NaCl(aq) + H2O(l) • H+ + Cl- + Na+ + OH-  Na+ + Cl- + H2O(l) H+ + OH-  H2O(l)

  20. Write the molecular equation, then complete ionic and finally the net ionic equations Potassium Hydroxide + Sulfuric Acid • Ionic equation: • Net Ionic equation:

  21. Neutralization Reaction of Weak Acid *Remember, only strong electrolytes are written as ions.* Acetic Acid + Sodium Hydroxide  HC2H3O2(aq) + NaOH(aq)  NaC2H3O2(aq) + H2O(l) Weak acid strong base soluble salt water HC2H3O2 + Na+ + OH- Na+ + C2H3O2- + H2O(l) HC2H3O2(aq) + OH-(aq)  C2H3O2-(aq)+ H2O(l)

  22. 4.27 a. 2HBr (aq) + Ca(OH)2 (aq)  CaBr2 (aq) + 2H2O (l) 2H+(aq) + OH-(aq)  2H2O (l) b. Cu(OH)2(s) + 2HClO4 (aq)  Cu(ClO4)2 (aq) + 2H2O (l) Cu(OH)2(s) + 2H+(aq)  2H2O (l) + Cu+2(aq) c. Cr(OH)3(s) + 3HNO3 (aq)  Cr(NO3)3 (aq) + 3H2O (l) Cr(OH)3(s) + 3H+(aq)  3H2O (l) + Cr+2 (aq)

  23. 4.28 a. HC2H3O3(aq) + KOH (aq)  K2C2H3O2 (aq) + 2H2O (l) H+(aq) + OH-(aq)  H2O (l) b. Ca(OH)2(s) + 2HNO3 (aq)  Ca(NO3)2 (aq) + 2H2O (l) Ca(OH)2(s) + 2H+(aq)  2H2O (l) + Ca+2(aq) c. Fe(OH)3(s) + 3HClO4 (aq)  Fe(ClO4)3 (aq) + 3H2O (l) Fe(OH)3(s) + 3H+(aq)  3H2O (l) + Fe+3 (aq)

  24. Acid/Base Rx’s with gas formation • Other bases besides OH- react with H+ to form molecular compounds.Two common bases are CO3-2 and S-2. • Carbonates and bicarbonates react with acid to form CO2.

  25. Hydrochloric acid + Sodium Sulfide  2HCl (aq) + Na2S(aq)  H2S(g) + 2NaCl(aq) 2H+ (aq) + S2-(aq)  H2S(g) Hydrochloric acid + Sodium Hydrogen Carbonate  HCl (aq) + NaHCO3(aq)  NaCl(aq) + H2CO3(aq) unstable H2CO3(aq) H2O(l) + CO2(g) Overall HCl (aq) + NaHCO3(aq)  NaCl(aq) + H2O(l) + CO2(g) Net H+ (aq) + HCO3-(aq)  H2O(l) + CO2(g)

  26. 4.29 a. CdS (s) + H2SO4 (aq)  CdSO4 (aq) + H2S (g) CdS (s) + 2H+(aq)  H2S (g) + Cd+2 b. MgCO3(s) + 2HClO4 (aq)  Mg(ClO4)2 (aq) + H2O (l) + CO2 (g) MgCO3(s) + 2H+(aq)  2H2O (l) + CO2 (g) Mg+2(aq)

  27. 4.30 a. CaCO3(s) + 2HNO3 (aq)  Ca(NO3)2 (aq) + H2O (l) + CO2 (g) CaCO3(s) + 2H+(aq)  H2O (l) + CO2 (g) + Ca+2 (aq) b. FeS (s) + 2HBr2 (aq)  FeBr2 (aq) + H2S (g) FeS (s) + 2H+(aq)  2H2S (g) + Fe+2(aq)

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