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11 Nov 2019
Question 3 (5 poitts) A 25.0 mL solution of 0.10 M acetic acid (K 1.8 x 10-5) is titrated with a 0.1 M NaOH solution. The pH at equivalence is: srthe ) O a) pH = 8.72 O b) pH 5.60 O c) pH- 9.13 O d) pH 5.29 Save Question 4 (5 points) A 25.0 mL of a weak acid is titrated with a strong base (0.1 M). Calculate the pH of the solution during the titration if the weak acid concentration is 0.10 M and its K 1.8 x 10 and 10.0 mL of base has been added. (Hint: use Henderson-Hasselbach equation). O a) pH = 4.56 b) pH- 5.28 O c) pH= 7.00 O d) pH= 4.74
Question 3 (5 poitts) A 25.0 mL solution of 0.10 M acetic acid (K 1.8 x 10-5) is titrated with a 0.1 M NaOH solution. The pH at equivalence is: srthe ) O a) pH = 8.72 O b) pH 5.60 O c) pH- 9.13 O d) pH 5.29 Save Question 4 (5 points) A 25.0 mL of a weak acid is titrated with a strong base (0.1 M). Calculate the pH of the solution during the titration if the weak acid concentration is 0.10 M and its K 1.8 x 10 and 10.0 mL of base has been added. (Hint: use Henderson-Hasselbach equation). O a) pH = 4.56 b) pH- 5.28 O c) pH= 7.00 O d) pH= 4.74
Jarrod RobelLv2
17 Apr 2019