titrations - titration known concentration of base is added...

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titration  - known concentration of base is added to acid (or acid to base)   equivalence point - where amount of acid/base are stoichiometrically equivalent pH titration curve - graph of pH as a function of volume of added titrant strong acid-strong base titration - characterized by sudden, very steep change in pH o initial pH based on initial concentration of acid o pH increases slowly when base first added o pH increases dramatically near equivalence point o only the salt exists at the equivalence point, pH = 7 o pH after equivalence point determined by amount of base in solution weak acid-strong base titration - less change at equivalence point than strong acid-strong base o higher initial pH than strong acid-strong base o equivalence point always > 7 due to strong base Find the pH of solution formed when 45.0 mL of 0.100 M NaOH is added to 50.0 mL of 0.100 M acetic acid.   Given: o Ka = 1.8 x 10-5 mol of NaOH = 0.045 L (0.100 mol / 1 L) = 4.5 x 10-3 mol mol of acetic acid = 0.050 L (0.100 mol / 1 L) = 5 x 10-3 mol
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