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© 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
© 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
© University of South Carolina Board of Trustees
Chapt. 16More Acids and Bases
Sec. 1Titration: Chemistry Unplugged
© 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
© 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.
© 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.
© 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
© 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?
© 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?