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Acids and Bases Chapter 14/15

Acids and Bases Chapter 14/15. Brendan Thomas Justin Simmons Sam Choi Alina Wieprecht. Properties. Acids. Bases. Sour Taste Conduct electricity React with many metals to produce H2 Turn litmus paper red Start with H (HCl, etc) Lemons, oranges, grapefruits . Bitter taste

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Acids and Bases Chapter 14/15

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  1. Acids and Bases Chapter 14/15 Brendan Thomas Justin Simmons Sam Choi AlinaWieprecht

  2. Properties Acids Bases • Sour Taste • Conduct electricity • React with many metals to produce H2 • Turn litmus paper red • Start with H (HCl, etc) • Lemons, oranges, grapefruits • Bitter taste • Conduct electricity (dissociate in water to create ions) • Do NOT react with metals • Turn litmus paper blue • Often end in OH (hydroxide) • Ivory soap, dish detergent • Sometimes called alkalis • Smooth and slippery

  3. Scientists • Arrhenius • Arrhenius Acid: • A substance that dissociates to produce hydrogen ions (H+) in water • Arrhenius Base: • A substance that dissociates to produce hydroxide ions (OH-) in water Keyword: Dissociation

  4. Scientists (cont.) • Bronsted- Lowry • This theory assumes that H+ is a proton with no electrons. • Bronsted-Lowry Acid: • Any substance that can donate H+ ions (a proton donor) • Bronsted-Lowry Base: • Any substance that can accept H+ ions (a proton acceptor) Keyword: Donate/accept H+ ions

  5. Scientists (cont.) • Lewis • Lewis Acid: • Any substance such as the H+ ion that can accept a pair of nonbonding electrons (electron pair acceptor) • Lewis Base: • Any substance such as the OH- ion that can donate a pair of nonbonding electron (electron pair donor) Keyword: donate/accept electron pairs

  6. Naming Binary and Ternary Acids • Binary Acids • Acids that consist of two elements • 1) H+ • 2) nonmetal • Use the stem of the name of the nonmetal • hydro(stem)ic acid • Examples • HI _________________ • HBr _________________ • Tertiary • Acids that consist of three elements • 1) H+ • 2) O2- • 3) nonmetal • If the negative ion ends in “ite” • (stem)ous acid • If the negative ion ends in “ate” • (stem)ic acid • Examples • H2CO3 ________________ • H2SO3 ____________________ Hydroiodic acid Carbonic acid Hydrobromic acid Sulfurous acid

  7. Writing Acid-Base Reactions in Aqueous Solutions Acid-base aqueous reactions deal with the dissociation of strong and weak acids and bases. • HClO3 H + ClO3 • NaOH Na+1 + OH-1 • HCl _____________ • KOH _____________ +1 - H+1 + Cl-1 K+1 + OH-1

  8. Writing Neutralization Reactions The acid and base will neutralize each other and form a product of salt and water. Na3PO4 H2O H3PO4 + 3NaOH  ________ + ___________ N2CO3 2 NaOH 2 NaOH + H2CO3________ + ___________

  9. CalculatingHydronium and Hydroxide IonConcentrations Hydronium [H3O+] Hydroxide [OH-] • Given pH is 4.35, calculate the hydronium ion concentration. 4.35 = - log[H3O+] - 4.35 = log[H3O+] 10^(-4.35) = [H3O+] [H3O+] = 4.47 x 10^(-5) M • Given pOH is 8.7, calculate the hydroxide ion concentration. 8.4 = -log[OH-] - 8.4 = log[OH-] 10^(-8.4) = [OH-] [OH-] = 3.9 x 10^(-9) M Units: M

  10. More Hydronium and Hydroxide Ion Calculations Hydronium Hydroxide • Given pH is 7.3, calculate the hydronium ion concentration. 7.3 = - log[H3O+] - 7.3 = log[H3O+] 10^(-7.3) = [H3O+] [H3O+] = 5.01 x 10^(-8) M • Given pOH is 6.7, calculate the hydroxide ion concentration. 6.7 = -log[OH-] - 6.7 = log[OH-] 10^(-6.7) = [OH-] [OH-] = 2 x 10^(-7) M Units: M

  11. pH and pOH Calculations pH pOH • Given [H3O+] is 2.4 x 10^(-3) M, calculate pH. pH = - log [2.4 x 10^(-3) M] pH = 2.6 • Given [OH-] is 7.8 x 10^(-5) M, calculate pOH. pOH = - log [7.8 x 10^(-5) M] pOH = 4.1

  12. More pH and pOH Calculations pH pOH • Given [OH-] = 5.9 x 10^(-6) M, calculate pH. pOH = -log [5.9 x 10^(-6) M] pOH = 5.23 pH = 14 – 5.23 = 8.77 • Given [H3O+] = 9 x 10^(-2) M, calculate pOH. pH = -log [9 x 10^(-2)] pH = 1.05 pOH = 14 – 1.05 = 12.95

  13. Titration • Is the controlled addition and measurement of the amount of the solution of known concentration required to react completely with a measured amount of a solution of unknown concentration • So, in English: when you’re using an indicator, the solution will turn a certain color once you’ve reached the equivalence point (where the two liquids are present in chemically equivalent amounts) • *using an indicator only works with strong acids and bases

  14. Calculate the Molarity of an unknown acid or base using titration data -2 Need 20 mL of 1.0 x 10 mol NaOH to reach the end point in the titration of 10 mL of HCl HCl(aq) +NaOH(aq) NaCl(aq) + H2O(l) Calculating Moles of NaOH -2 1.0 x 10 mol NaOH x 1L x 20.0mL NaOH = 2.0 x 10-4 mol NaOH used 1L NaOH 1000mL Mole Ratio -4 -4 2.0 x 10 mol NaOH x 1 mol HCl= 2.0 x 10 mol HCl 1 mol NaOH Calculating Molarity of HCl Solution -4 -2 2.0 x 10 mol HCl x 1000mL = 2.0 x 10 mol HCl= 2.0 x 10 M HCl -2 10.0mL HCl 1L 1LHCl

  15. Calculate the Molarity of an unknown acid or base using titration data -3 Need 35.0 mL of 6.0 x 10 mol KOH to reach an end point in titration of 15.0 mL of HBr HBr(aq) +KOH(aq) KBr(aq) + H2O(l) Calculating Moles of KOH -3 6.0 x 10 mol KOH x 1L x 35.0mL = 2.1 x 10 mol KOH used -4 1L KOH 1000mL Mole Ratio -4 -4 2.1 x 10 mol KOH x 1 mol HCl= 2.1 x 10 mol HBr 1 mol KOH Calculating Molarity of HBr Solution -4 -2 2.1 x 10 mol HBr x 1000mL = 1.4 x 10 mol HBr = 1.4 x 10 M HBr -2 15.0mL HBr 1L 1LHBr

  16. Picture Websites • https://science7acidbase.wikispaces.com/Litmus+Paper • http://commons.wikimedia.org/wiki/File:PH_scale_2.png • http://www.sciencebuddies.org/science-fair-projects/project_ideas/Chem_p045.shtml

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