Titration Curves. Problem   50.0 mL of 0.10 M acetic acid (K a = 1.8 x 10 -5 ) are titrated with 0.10 M NaOH. Calculate the pH after the additions of.

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Titration Curves

Problem   50.0 mL of 0.10 M acetic acid (K a = 1.8 x ) are titrated with 0.10 M NaOH. Calculate the pH after the additions of 0, 10, 25, 40, 50, 60, and 75 mL samples of NaOH.   Then, construct a titration curve and label it properly.

Problem   50.0 mL of 0.20 M carbonic acid (K a = 4.4 x ) are titrated with 0.20 M NaOH. Calculate the pH after the additions of 0, 10, 25, 40, 50, 60, and 75 mL samples of NaOH.   Then, construct a titration curve and label it properly.

Weak Base-Strong Acid Titration Curves   Before the addition.   Construct an “equilibrium” reaction table ONLY!   K b = [OH - ] [BH + ] and obtain [OH - ].   [B]   Calculate the pOH, then the pH.

Additions before the equivalence point.   Construct a “stoichiometry” reaction table.   Determine MOLES of base in excess (not neutralized) and MOLES of conjugate acid formed.   Divide MOLES by the TOTAL VOLUME to obtain [BH + ] and [B].   Construct an “equilibrium” reaction table.   K b = [OH - ] [BH + ] and obtain [OH - ].   [B]   Calculate the pOH, then the pH.

Additions at the equivalence point   Construct a “stoichiometry” reaction table.   Determine MOLES of conjugate acid formed.   Divide MOLES by the TOTAL VOLUME to obtain [BH + ].   Calculate K a (K a x K b = K w ).   Construct an “equilibrium” reaction table, reacting the conjugate base with water.   K a = [A - ] [H 3 O + ] and obtain [H 3 O + ].   [HA]   Calculate the pH.

Additions beyond the equivalence point   Construct a “stoichiometry” reaction table.   Determine MOLES of acid in excess (not neutralized) and the MOLES of conjugate acid.   Divide MOLES by the TOTAL VOLUME,   Because [H 3 O + ] excess >> [H 3 O + ] conj. acid, use [OH - ] excess to calculate the pH.

Problem   20.0 mL of 0.10 M triethylamine, (CH 3 CH 2 ) 3 N, (K b = 5.2 x ) are titrated with M HCl. Calculate the pH after the additions of 0.0, 10, 15, 19, 19.95, 20, 20.05, and 25 mL samples of HCl.   Then, construct a titration curve and label it properly.