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Titration

Titration. Unit 12: Acids and Bases Section 4: Titration. Titration. Titration : The controlled addition and measurement of the amount of a solution of known concentration required to react completely with a measured amount of a solution of unknown concentration

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Titration

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  1. Titration Unit 12: Acids and Bases Section 4: Titration

  2. Titration • Titration: The controlled addition and measurement of the amount of a solution of known concentration required to react completely with a measured amount of a solution of unknown concentration • - It provides a means to determine the concentration of an unknown solution.

  3. Titration • End Point:

  4. Equivalence Point:

  5. Titration Sample Problem In a titration 27.4 mL of 0.0154 M Ba(OH)2 is added to a 20.0 mL sample of HCl solution of unknown concentration until the equivalence point is reached. What is the molarity of the acid solution? Ba(OH)2 + HCl  BaCl2 + H2O

  6. Titration Step One – Balancing Ba(OH)2 + 2HCl BaCl2 + 2 H2O Step Two – Given and Unknown G: 27.4 mL of 0.0154 M Ba(OH)2 20.0 mL of HCl U: # M of HCl

  7. Titration Step Three – Convert M to Mole 1L 1000 mL 0.0154 mol Ba(OH)2 1 L 27.4 mL 4.22 x 10-4 mol Ba(OH)2

  8. Titration Step Four – Convert Ba(OH)2 to mol HCl 2 mol HCL 1 mol Ba(OH)2 4.22 x 10-4 mol Ba(OH)2 8.44 x 10-4 mol HCl

  9. Titration Step Five – Use the mL of HCl to find concentration of HCl 8.44 x 10-4 mol HCl 20.0 mLHCl 1000 mL 1 L 4.22 x 10-2 m HCl

  10. Titration Sample Problem # 2 In a titration 20.0 mL of 5.0 x 10-3 M NaOH is added to a 10.0 mL sample of HCl until equivalence point is reached. What is the molarity of the acid solution? NaOH + HCL  NaCl + H2O

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