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Topic: Titration Do Now:

Topic: Titration Do Now: . Acid-Base Titration. A procedure used in order to determine the molarity of an acid or base K nown volume of a solution with a known concentration (standard solution) and k nown volume of unknown concentration and a M A V A = M B V B acid-base indicator needed.

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Topic: Titration Do Now:

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  1. Topic: Titration Do Now:

  2. Acid-Base Titration • A procedure used in order to determine the molarity of an acid or base • Known volume of a solution with a known concentration (standard solution) and known volume of unknown concentration and a • MAVA = MBVB • acid-base indicator needed

  3. Titration • Standard solution slowly added to unknown solution • As solutions mix: • neutralization reaction occurs • Eventually: • enough standard solution is added to neutralize the unknown solution Equivalence point

  4. Equivalence point total # moles H+1 ions donated by acid equals total # moles H+1 accepted by base total moles H+1 = total moles OH-1

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

  6. 14- Equivalence Pt    0 ml 20 ml Titration of a strong acid with a strong base Phenolphthalein Color change: 8.2 to 10  pH 7- 0-  Volume of 0.100 M NaOH added (ml) 40ml

  7. MH+1 VH+1= MOH-1 VOH-1 • MH+1= molarity of H+1 • MOH-1= molarity of OH-1 • VH+1= volume of H+1 • VOH-1= volume of OH-1

  8. 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

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

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

  11. 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

  12. Variables • # of H’s = 1 • Ma= X • Va = 20.0 mL • # of OH’s = 1 • Mb = 0.250 M • Vb = 50.0 mL

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

  14. 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

  15. Variables • # of H’s = 2 • Ma= X • Va = 20.0mL • # of OH’s = 1 • Mb = 0.25M • Vb = 50.0mL

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

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