A 25.0 mL sample of 0.100 M propanoic acid (HC3H5O2, Ka = 1.3 ✕ 10-5) is titrated with 0.100 M KOH solution. Calculate the pH after the addition of the following amounts of KOH. 0.0 mL 4.0 mL 8.0 mL 12.5 mL 20.0 mL 24.0 mL 24.5 mL 24.9 mL 25.0 mL 25.1 mL 26.0 mL 28.0 mL 30.0 mL
A 25.0 mL sample of 0.100 M propanoic acid (HC3H5O2, Ka = 1.3 ✕ 10-5) is...
3. A 30.0 mL sample of 0.165 M propanoic acid (HC3H5O2) is titrated with 0.300 M potassium hydroxide. Calculate the pH under the following conditions. Please write your final answers in the box. Show your work below and/or on scratch paper. (5 points) K CaH02 7.7 x 100 K, HCsHsO2 1.3 x 10 Answer Question What is the initial pH of propanoic acid before titrating with KOH? b a. 2.834 What is the pH after the addition of 10.0 mL...
Consider the titration of 50.0 mL of 0.100 M HC3H5O2 by 0.100 M KOH for the next five questions (Ka for HC3H5O2 = 1.3 x 10-5). Calculate all pH values to two decimal places. - Calculate the pH after 25.0 mL of KOH has been added?
4). A 25.0-mL sample of 0.265 M propanoic acid (Ka = 1.3x10-5) is titrated with 0.2500 M NaOH. What is the pH after 15mL of base was added?
A 50.0 mL solution of 0.156 M KOH is titrated with 0.312 M HCl. Calculate the pH of the solution after the addition of each of the given amounts of HCI. 0.00 mL pH = 13.2 6.00 mL pH = 13.1 12.5 mL pH = 12.84 20.0 mL pH = 13.35 24.0 mL pH = 13.32 25.0 mL pH = 13.32 26.0 mL 200 mL o pH = pH = 12:37 30.0 mt p# = 12.40 12.37 30.0 mL pH...
Acid/Base titrations 10. 25.0 mL of 0.100 M H2A (a weak diprotic acid) is titrated with 0.200 M NaOH. What is the pH of the solution when 0.00 mL, 10.0 mL, 12.5 mL, 20.0 mL, 25.0 mL, and 40.0 mL E.S RaWeMA 5.83 x 10 8) have been added? (Ka1= 2.46 x 10, Ka2 ANSWER: 0 mL = 2.315, 10.0 mL= 4.211 (or 4.213), 12.5 mL = 5.422, 20.0 mL 7.410, 25.0 mL = 9.966, 40.0 mL = 12.664 11....
A sample of 0.100 M acetic acid (Ka = 1.8 × 10−5) in 50.0 mL of solution is titrated with standard 0.100 M NaOH. What is the pH in the titration flask after addition of 15.0 mL of NaOH?
Nicole measured the pH of a 0.100 M solution of propanoic acid, CH3CH2COOH, a weak organic acid at equilibrium and found it to be 2.931 at 25C. Calculate the Ka of propanoic acid. Her lab instructor mentions that the half equivalence method is better for determining pKa. What is the half-equivalence point and why is this method better at determining pKa? What is the pH after 20.0 mL of 0.0750 M NaOH is added to 30.0 mL of the 0.100...
A 50.0 mL solution of 0.137 M KOH is titrated with 0.274 M HCl. Calculate the pH of the solution after the addition of each of the given amounts of HCI. 0.00 mL pH = 5.00 mL pH = 12.5 mL pH = 20.0 mL pH = 24.0 mL pH = 25.0 mL pH= 26.0 mL pH = 29.0 mL pH =
A 50.0 mL solution of 0.110 M KOH is titrated with 0.220 M HCl. Calculate the pH of the solution after the addition of each of the given amounts of HCl. 0.00 mL pH = 7.00 mL pH = | 12.5 mL pH = 20.0 mL pH = 24.0 mL pH = 25.0 mL pH = 26.0 mL pH = 29.0 mL pH =
A 50.0 mL solution of 0.146 M KOH is titrated with 0.292 M HCl. Calculate the pH of the solution after the addition of each of the given amounts of HCl. 0.00 mL pH = 6.00 mL pH = 12.5 mL pH = 1 20.0 mL pH = 24.0 mL pH = 25.0 mL pH= 26.0 mL pH = 29.0 mL pH =