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# Titration PowerPoint PPT Presentation

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

Titration

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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

• - It provides a means to determine the concentration of an unknown solution.

Titration

• End Point: Point in a titration at which an indicator changes color

• Equivalence Point: Point where the two solutions used in a titration are present in chemically equivalent amounts

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

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

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

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

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

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