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Topic: Neutralization Reaction Do Now:

Topic: Neutralization Reaction Do Now: . Neutralization Reactions. +. Base. →. Salt + Water. Acid. HX( aq ) + MOH( aq ) → MX( aq ) +H 2 O(l ). DR rxn. Acid-Base Titration. A procedure used in order to determine the unknown molarity of an acid or base M A V A = M B V B

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Topic: Neutralization Reaction Do Now:

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  1. Topic: Neutralization Reaction Do Now:

  2. Neutralization Reactions + Base → Salt + Water • Acid HX(aq) + MOH(aq)→ MX(aq) +H2O(l) • DR rxn

  3. Acid-Base Titration • A procedure used in order to determine the unknown molarity of an acid or base • MAVA= MBVB • (molarityof acid)(volume of acid) = (molarity of base)(volume of base) • You will know 3 out of the 4 variable • Standard solution slowly added to unknown solution • As solutions mix: • neutralization reaction occurs • Eventually: • enough standard solution is added to neutralize the unknown solution

  4. pH < 7 pH  pH = 7 pH > 7 pH  pH = 7 pH changes during neutralization • Start with an acid • Add a base • At neutralization • Start with a base • Add an acid • At neutralization When pH = 7 called equivalence point [H+] = [OH-] • acid-base indicator needed • WHY? • Usually use phenolphalein • WHY?

  5. Titration • End-point = point at which indicator changes color • if indicator chosen correctly: • end-point very close to equivalence point

  6. MH+1 VH+1= MOH-1 VOH-1 • If you titrate H2SO4 and NaOH 1OH+- 2H+

  7. Titration Problem #1 • In a titration of 40.0 mL of a nitric acid solution, the end point is reached when 35.0mL of 0.100M NaOH is added Calculate the concentration of the nitric acid solution HNO3 + NaOH H2O + NaNO3

  8. Variables • # of H’s = 1 • Ma= ? • Va = 40.0 mL • # of OH’s = 1 • Mb = 0.100 M • Vb = 35.0 mL

  9. (1)(X) (40.0 mL) = (0.100 M )(35.0mL)(1) X = 0.875 M HNO3

  10. Titration Problem #2 • What is the concentration of a hydrochloric acid solution if 50.0 mL of a 0.250M KOH solution is needed to neutralize 20.0mL of the HCl solution of unknown concentration? KOH + HCl H2O + KCl

  11. (1)(X)(20.0 mL) = (0.250 M) (50.0 mL)(1) X = 0.625 M HCl

  12. Titration Problem #3 • What is the concentration of a sulfuric acid solution if 50.0mL of a 0.25 M KOH solution is needed to neutralize 20.0mL of the H2SO4 solution of unknown concentration? H2SO4 + 2 KOH  2 H2O + K2SO4

  13. (2)(X)(20.0ml) = (0.25M)(50.0ml)(1) X = 0.3125 M H2SO4(sulfuric acid)

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