Question
6. You have 40.00 mL of a 0.250 M aqueous solution of the weak base (CH3)3N (Kb = 7.40 x 10-5). This solution will be
6. You have 40.00 mL of a 0.250 M aqueous solution of the weak base (CH3)3N (Kb = 7.40 x 10-5). This solution will be titrated with 0.250 M HCl. (a) How many mL of acid must be added to reach the equivalence point? (b) What is the pH of the solution before any acid is added? (c) What is the pH of the solution after 10.00 mL of acid has been added? (d) What is the pH of the solution at the equivalence point of the titration? (e) What is the pH of the solution when 45.00 mL of acid has been added?
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Chemical Principles
Authors: Steven S. Zumdahl, Donald J. DeCoste
7th edition
9781133109235, 1111580650, 978-1111580650
