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Neutralization – Day 1

Neutralization – Day 1. Neutralization Reactions. A neutralization reaction is a reaction in which an acid and a base react to produce a salt and water Acid + Base  Salt + H 2 O A salt is an ionic compound made up of a cation and an anion. 3 Types of Acid-Base Reactions.

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Neutralization – Day 1

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  1. Neutralization – Day 1

  2. Neutralization Reactions • A neutralization reaction is a reaction in which an acid and a base react to produce a salt and water • Acid + Base  Salt + H2O • A salt is an ionic compound made up of a cation and an anion

  3. 3 Types of Acid-Base Reactions

  4. Neutralization Reaction • HCl + NaOH  + H2O water NaCl salt acid base

  5. Neutralization Reactions MgCl2 + H2O 2 • Mg(OH)2(aq) + 2HCl(aq)  base acid Write a balanced formula equation for the following acid base neutralization reaction Nitric acid and sodium hydroxide HNO3 + NaOH  Salt Water NaNO3 + H2O Salt Water

  6. Practice Neutralization Reactions Write a balanced formula equation for the following acid base neutralization reactions: Barium hydroxide and hydrochloric acid Ba(OH)2 + HCl  Sulfuric acid and cesium hydroxide H2SO4 + CsOH  Nitirc acid and potassium hydroxide HNO3 + KOH  2 H2O + BaCl2 2 Cs2SO4 2 2 H2O + H2O + KNO3

  7. Question Time • What is a neutralization reaction? • What is a salt? • Where does the cation in the salt come from? • Where does the anion in the salt come from?

  8. Titration Day 2

  9. Titration • Purpose - To find the unknown concentration of a solution. • Procedure – Add a known amount of solution of known concentration to a solution of unknown concentration.

  10. Titration Vocabulary • Buret – A piece of glassware used for dispensing accurate volumes of a solution. • The solution of known concentration is in the buret.

  11. Titration Vocabulary • Analyte/Unknown Solution - The solution that is being analyzed. It is the solution of unknown concentration • Titrant/Standard Solution - The solution of known concentration that is added to the analyte

  12. Titration Vocabulary • Equivalence Point - when the acid and base are mixed and the number of hydrogen ions equal the number of hydroxide ions. • [H+] = [OH-]

  13. Titration • Acid–base indicator – A chemical dye whose colors are affected by acidic and basic solutions. A common acid base indicator for titration is phenolphthalein. • End point is the point which the indicator used in titration changes color.

  14. Equivalence Point vs. End Point • The equivalence point is when [H+] = [OH-]. You cannot see this. • The end point is when you see a change in color in the indicator. • The equivalence point should be very close to the end point. To make sure this happens, an appropriate indicator needs to be chosen.

  15. Question Time • What is the purpose of titration? • What is a standard solution? What is another name for the standard solution? • What is the equivalence point? • What is phenolphthalein? • What is the end point? • What is the difference between the equivalence point and end point

  16. You Tube Titrations • http://www.youtube.com/watch?v=g8jdCWC10vQ • (1min 10 sec) • http://www.youtube.com/watch?v=8UiuE7Xx5l8&feature=related • (3 min 15 sec) • http://www.youtube.com/watch?v=Y-5QJIr7Xm4 • (4 min 51 sec) • http://www.youtube.com/watch?v=9DkB82xLvNE • (5min 3 sec) • http://www.youtube.com/watch?v=LvXQc0M1grQ • (8min 50 sec-student video)

  17. Titration Calculation Example • HC2H3O2 + NaOH  H2O + NaC2H3O2 • In a titration, the volume of base needed was 9.50mL of 0.500 M NaOH to reach equivalence point. The volume of HC2H3O2 acid titrated was 5.89 mL. Find the molarity of the acid.

  18. HC2H3O2 + NaOH  H2O + NaC2H3O2 What is the standard solution?(the acid or the base) 9.50mL NaOH 1 L 0.500 mol NaOH 1 mol HC2H3O2 1000 mL 1 mol NaOH 1 L NaOH 0.00475 mol HC2H3O2 = 0.00475 mol HC2H3O2 1000 mL 0.806 mol HC2H3O2 L = 5.89 mL HC2H3O2 1 L 0.806 M HC2H3O2

  19. Neutralization with Polyprotic Acids • If you are doing a neutralization where there is more than one hydrogen on the acid, your mole ratio will not be one to one. • Example: • H2SO4 + 2RbOH  2H2O + Rb2SO4 43.21mL RbOH 1 L 0.03020 mol NaOH 1 mol H2SO4 1000 mL 2mol RbOH 1 L NaOH 0.0006525 mol H2SO4 = 0.0006525 mol H2SO4 1000 mL 0.02175 mol H2SO4 L = 30.00 mL H2SO4 1 L or 0.02175 M H2SO4

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