Titration

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Titration

• Acids Bases

2
A. Neutralization

• Chemical reaction between an acid and a base
• Products are a salt (ionic compound) and water

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A. Neutralization

• ACID BASE ? SALT WATER

HCl NaOH ? NaCl H2O
strong
strong
neutral
HC2H3O2 NaOH ? NaC2H3O2 H2O
weak
strong
basic

• Salts can be neutral, acidic, or basic

• Neutralization does not mean pH 7

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A. Neutralization

• ACID BASE ? SALT WATER

• Double replacement reaction

• Can predict products ex. antacids in your
  stomach

CaCl2 H2O
2
HCl Ca(OH)2 ?
2
neutral
strong
strong
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B. Titration
standard solution

• Titration
• Analytical method in which a standard solution is
  used to determine the concentration of an unknown
  solution

unknown solution
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B. Titration

• Stoichiometry
• Provides basis for titration
• Examples
• 1 mol HCl will neutralize 1 mol NaOH
• 2 mol HCl will neutralize 1 mol Mg(OH)2

HCl NaOH ? NaCl H2O
2HCl Mg(OH)2 ? MgCl2 2H2O
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B. Titration

• Equivalence point
• Point at which equal number of moles of H3O and
  OH- are in solution
• Determined by
• indicator color change

• dramatic change in pH

8
B. Titration
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B. Titration

• Endpoint
• Point at which indicator color changes
• Should be close to equivalence point if correct
  indicator is chosen

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B. Titration
moles H3O moles OH- MA?VA? nA MB?VB? nB
M Molarity V volume n of H ions in the
acid or OH- ions in the base
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B. Titration

1. 50.0 mL of an unknown solution of NaOH are
   titrated with 0.100 M HCl. Find the molarity of
   the NaOH solution if 52.5 mL of acid are required
   to reach the equivalence point.

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B. Titration

1. 42.5 mL of 1.3M KOH are required to neutralize
   50.0 mL of H2SO4. Find the molarity of H2SO4.