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© University of South Carolina Board of Trustees Determine the number of moles of Na(CH 3 COO) that must be added to 250 mL of 0.16 M CH 3 COOH to prepare a pH 4.70 solution. K a = 1.8x10 −5 pH Buffer composition

© University of South Carolina Board of Trustees Determine the number of moles of Na(CH 3 COO) that must be added to 250 mL of 0.16 M CH 3 COOH to prepare

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Page 1: © University of South Carolina Board of Trustees Determine the number of moles of Na(CH 3 COO) that must be added to 250 mL of 0.16 M CH 3 COOH to prepare

© University of South Carolina Board of Trustees

Determine the number of moles of Na(CH3COO) that must be added to 250 mL of 0.16 M CH3COOH to prepare a pH 4.70 solution. Ka = 1.8x10−5

pH Buffer composition

Page 2: © University of South Carolina Board of Trustees Determine the number of moles of Na(CH 3 COO) that must be added to 250 mL of 0.16 M CH 3 COOH to prepare

© University of South Carolina Board of Trustees

Does a Buffer Stabilize pH?Calculate the initial and final pH when10.0 mL of 0.100 M HCl is added to:

(a) 100 mL of water

(b) 100 mL of a buffer which is 1.50 M in CH3COOH (pKa = 4.74) and 1.25 M in Na(CH3COO)

pH 7.00

pH 4.66 4.65

2.04

Page 3: © University of South Carolina Board of Trustees Determine the number of moles of Na(CH 3 COO) that must be added to 250 mL of 0.16 M CH 3 COOH to prepare

© University of South Carolina Board of Trustees

Chapt. 16More Acids and Bases

Sec. 1Titration: Chemistry Unplugged

Page 4: © University of South Carolina Board of Trustees Determine the number of moles of Na(CH 3 COO) that must be added to 250 mL of 0.16 M CH 3 COOH to prepare

© University of South Carolina Board of Trustees

Titration Experiment

acid solutionunknown concentration

strong base solution known concentration

indicator dye changes color

record volume of base

Page 5: © University of South Carolina Board of Trustees Determine the number of moles of Na(CH 3 COO) that must be added to 250 mL of 0.16 M CH 3 COOH to prepare

© University of South Carolina Board of Trustees

Titration Overview (Strong Acid + Strong Base example)

Titration Curve: a graph of pH of the solution in the flask as titrant (base) is added.

Page 6: © University of South Carolina Board of Trustees Determine the number of moles of Na(CH 3 COO) that must be added to 250 mL of 0.16 M CH 3 COOH to prepare

© University of South Carolina Board of Trustees

Titration Overview (Strong Acid + Strong Base example)

Equivalence Point: (known) moles of base added equals (unknown) moles of acid in sample.

Page 7: © University of South Carolina Board of Trustees Determine the number of moles of Na(CH 3 COO) that must be added to 250 mL of 0.16 M CH 3 COOH to prepare

© University of South Carolina Board of Trustees

Titration Overview (Strong Acid + Strong Base example)

Indicator: Added dye that changes color at the equivalence point.

color change

Page 8: © University of South Carolina Board of Trustees Determine the number of moles of Na(CH 3 COO) that must be added to 250 mL of 0.16 M CH 3 COOH to prepare

© University of South Carolina Board of Trustees

Classroom Titration Problem

The equivalence point in the titration of 20.00 mL of ??? M HCl with 0.1008 M NaOH is at 24.84 mL. What is the concentration of the HCl?

What is the pH of the equivalence point?

Page 9: © University of South Carolina Board of Trustees Determine the number of moles of Na(CH 3 COO) that must be added to 250 mL of 0.16 M CH 3 COOH to prepare

© University of South Carolina Board of Trustees

Real Titration Problem

A solution of ascorbic acid has an unknown concentration. A small amount of phenolphthalein (indicator) is added to 25.00 mL of the solution, and it is titrated with 0.100 M NaOH. The first pink color is seen when 18.12 mL of NaOH solution has been added. What is the concentration of ascorbic acid in the original sample?