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Titration
• strong acids ionize almost completely
• weak acids don’t ionize very much• [H[H33OO+1+1] ] notnot same as acid same as acid
concentrationconcentration
[H3O+1]
• can’t be measured directly
• determined by comparison
Acid-Base Titration
• carefully controlled neutralization rxncarefully controlled neutralization rxn• requires:requires:
– standard solutionstandard solution & – acid-base indicatoracid-base indicator
• standard solution is: acid/base of knownknown concentration
TitrationTitration
• 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 pointequivalence point
Equivalence pointEquivalence point
total # moles H+1 ions donated by acid =
total # moles H+1 accepted by base
so: total moles H+1 = total moles OH-1
TitrationTitration
• end-pointend-point: point at which indicator changes color
– if indicator chosen correctly: • end-point very close to equivalence point
Titration: strong acid with strong base
volume of 0.100 M NaOH added (ml)
pH
0-
14-
7- equivalence pt
phenolphthalein phenolphthalein color change: color change: 8.28.2 to 10 to 10
0 ml
40ml
20 ml
MMH+1H+1VVH+1H+1 = M = MOH-1OH-1VVOH-1OH-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
MaVa = MbVb
• [true for:– monoprotic acids with monohydroxy bases
– diprotic acids with dihydroxy bases
– triprotic acids with trihydroxy bases]
IF:
# H’s in acid
(Ma)(Va) = (Mb)(Vb)
≠ # OH’s in base
need to modify equation:
(#H’s) (#OH’s)
Titration Problem #1
In a titration of 40.0 mL40.0 mL of a nitric acid solution, the end point was reached when 35.0mL35.0mL of 0.100M0.100M NaOHNaOH was added.
calculate the concentration of the calculate the concentration of the nitric acid solutionnitric acid solution
Neutralization Reaction
HNO3 + NaOH H2O + NaNO3
•HNO3 is a monoprotic acid
•NaOH is a monohydroxy base
Variables
• Ma = ?
• Va = 40.0 mL
• Mb = 0.100 M
• Vb = 35.0 mL
• #H’s = #OH’s = 1
Plug and Chug
(1)(x) (40.0 mL) = (0.100 M )(35.0mL)(1)
X = 0.875 M HNO3
Titration Problem #2
• What is theWhat is the concentration concentration of aof a hydrochloric acid solutionhydrochloric acid solution if 50.0 mL50.0 mL of a 0.250M KOH0.250M KOH solution is needed to neutralize 20.0mL 20.0mL of anof an HCl HCl solutionsolution of unknown concentration?
Neutralization Reaction
KOH + HCl H2O + KCl
•HNO3 is a monoprotic acid
•KOH is a monohydroxy base
Variables
• Ma = X
• Va = 20.0 mL
• Mb = 0.250 M
• Vb = 50.0 mL
• #H’s = #OH’s = 1
Plug and Chug
(1)(X)(20.0 mL) = (0.250 M) (50.0 mL)(1)
X = 0.625 M HCl
Titration Problem #3
• What is theWhat is the concentration concentration of aof a sulfuric acid solutionsulfuric acid solution if 50.0mL 50.0mL of aof a 0.25 M KOH0.25 M KOH solution is needed to neutralize 20.0mL 20.0mL of theof the H H22SOSO44 solutionsolution of unknown concentration?
Neutralization Reaction
• H2SO4 + 2 KOH 2 H2O + K2SO4
• H2SO4 is a diprotic acid
• KOH is a monohydroxy base
Variables
• Ma = X
• Va = 20.0mL
• Mb = 0.25M
• Vb = 50.0mL
• #H’s = 2
• #OH’s = 1
Plug and Chug
(2)(X)(20.0ml) = (0.25M)(50.0ml)(1)
X = 0.3125 M H2SO4(sulfuric acid)