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Titration

Acids & Bases. Titration. Neutralization. Chemical reaction between an acid and a base. Products are a salt (ionic compound) and water. Neutralization. ACID + BASE  SALT + WATER. HCl + NaOH  NaCl + H 2 O. strong. strong. neutral. HC 2 H 3 O 2 + NaOH  NaC 2 H 3 O 2 + H 2 O. weak.

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Titration

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  1. Acids & Bases Titration

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

  3. 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.

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

  5. Titration • Equivalence point (endpoint) • Point at which equal amounts of H3O+ and OH- have been added. • Determined by… • indicator color change • dramatic change in pH

  6. Acid-Base Titrations • For the titration of a strong base and a strong acid, the equivalence point is reached when the pH of the solution is seven (7)

  7. Acid-Base Titrations • For the titration of a strong base with a weak acid, the equivalence point is reached when the pH is greater than seven (7).

  8. Titration moles H3O+ = moles OH- MAVA n = MBVB n M: Molarity V: volume n: # of H+ ions in the acid or OH- ions in the base

  9. Titration • 42.5 mL of 1.3M KOH are required to neutralize 50.0 mL of H2SO4. Find the molarity of H2SO4. H3O+ M = ? V = 50.0 mL n = 2 OH- M = 1.3M V = 42.5 mL n = 1 MV# = MV# M(50.0mL)(2) =(1.3M)(42.5mL)(1) M = 0.55M H2SO4

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