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Acids and Bases: Properties, Definitions, and pH Scale

Learn about the properties, definitions, and pH scale of acids and bases. Understand the concept of neutralization and how to calculate molarity in titration.

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Acids and Bases: Properties, Definitions, and pH Scale

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  1. Warm-Up • If 22.4 g of NaOH is contained in 700. mL of solution • If 600. mL of 6.0 M HCl is diluted to 1.5 L • Find the Molarity of the following.

  2. What are Acids & Bases? Follow along in your textChapters 14 & 15

  3. electrolytes electrolytes Properties ACIDS BASES • bitter taste • sour taste • turn litmus red • turn litmus blue • react with metals to form H2 gas • slippery feel • vinegar, milk, soda, apples, citrus fruits • ammonia, lye, antacid, baking soda ChemASAP

  4. H H – + O O Cl Cl H H H H Definitions • Arrhenius - In aqueous solution… • Acidsform hydronium ions (H3O+) HCl+ H2O  H3O+ + Cl– acid

  5. H H – + N O O N H H H H H H H H Definitions • Arrhenius - In aqueous solution… • Bases form hydroxide ions (OH-) NH3+ H2O  NH4+ + OH- base

  6. conjugate base conjugate acid Definitions • Brønsted-Lowry • Acidsare proton (H+) donors. • Bases are proton (H+) acceptors. HCl + H2O  Cl– + H3O+ acid base

  7. Definitions H2O + HNO3 H3O+ + NO3– B A CA CB

  8. Definitions NH3 + H2O  NH4+ + OH- B A CA CB • Amphoteric- can be an acid or a base.

  9. F - H2PO4- H2O HF H3PO4 H3O+ Definitions • Give the conjugate base for each of the following: • Polyprotic- an acid with more than one H+

  10. Br - HSO4- CO32- HBr H2SO4 HCO3- Definitions • Give the conjugate acid for each of the following:

  11. Definitions • Lewis • Acidsare electron pair acceptors. • Basesare electron pair donors. Lewis base Lewis acid

  12. - + Strength • Strong Acid/Base • 100% ionized in water • strong electrolyte HCl HNO3 H2SO4 HBr HI HClO4 NaOH KOH Ca(OH)2 Ba(OH)2

  13. - + Strength • Weak Acid/Base • does not ionize completely • weak electrolyte HF CH3COOH H3PO4 H2CO3 HCN NH3

  14. The pH Scale Follow along in your textChapter 15 Section2Pages 539 -547

  15. Hydronium Ion H2O + H2O H3O+ + OH- Ionization of Water Kw = [H3O+][OH-] = 1.0  10-14

  16. Ionization of Water • Find the hydroxide ion concentration of 3.0  10-2 M HCl. [H3O+][OH-] = 1.0  10-14 [3.0  10-2][OH-] = 1.0  10-14 [OH-] = 3.3  10-13 M Acidic or basic? Acidic Hint: [H3O+] > [OH-]

  17. pouvoir hydrogène (Fr.) “hydrogen power” pH Scale 14 0 7 INCREASING BASICITY INCREASING ACIDITY NEUTRAL pH = -log[H3O+]

  18. pH Scale pH of Common Substances

  19. pH Scale pH = -log[H3O+] pOH = -log[OH-] pH + pOH = 14 [H3O+] = 10-pH [OH-] = 10-pOH

  20. pH Scale • What is the pH of 0.050 M HNO3? pH = -log[H3O+] pH = -log[0.050] pH = 1.3 Acidic or basic? Acidic

  21. pH Scale • What is the molarity of HBr in a solution that has a pOH of 9.6? pH + pOH = 14 pH + 9.6 = 14 pH = 4.4 pH = -log[H3O+] So [H3O+] = 10-pH [H3O+] = 10-4.4 [H3O+] = 4.0  10-5 M HBr Acidic

  22. Neutralization • Chemical reaction between an acid and a base. • Products are a salt (ionic compound) and water. ACID + BASE  SALT + WATER • Neutralization does not mean pH = 7.

  23. Neutralization • Salts can be neutral, acidic, or basic. HCl + NaOH NaCl + H2O strong strong neutral HC2H3O2 + NaOH NaC2H3O2 + H2O weak strong basic

  24. standard solution unknown solution Titration • Titration • Analytical method in which a standard solution is used to determine the concentration of an unknown solution.

  25. Titration • Equivalence point (endpoint) • Point at which equal amounts of H3O+ and OH- have been added. • Determined by… • indicator color change • dramatic change in pH

  26. pH Indicators

  27. Titration

  28. Titration moles H3O+ = moles OH- MVn = MVn M: Molarity V: volume n: # of H+ ions in the acid or # of OH- ions in the base

  29. Titration • 42.5 mL of 1.3M KOH are required to neutralize 50.0 mL of H2SO4. Find the molarity of H2SO4. H3O+ M = ? V = 50.0 mL n = 2 OH- M = 1.3M V = 42.5 mL n = 1 MV# = MV# M(50.0mL)(2) =(1.3M)(42.5mL)(1) M = 0.55M H2SO4

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