Consider the titration of 100.0 mL of 0.250 M HA (Kα = 5.0 × 10-4, pKa = 3.30)with 0.250 M NaOH. Determine the pH at the equivalence point.a.7.00b. 5.80C.11.59d. 8.20e.9.86

To determine the pH at the equivalence point for the titration of a weak acid (HA) with a strong…

Answered: Consider the titration of 100.0 mL of…

Chemistry

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ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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A student added 501 mL of 0.35 M HCl to a buffer solution made up of 0.500 mol of citrate (A-), 0.500 mol of citric acid to 1.5 L of water (total volume = 1.5 L) (Ka = 7.41 x 10-4). A.) Calculate the pH of the initial buffer solution (before the addition of the acid). B.) Calculate the pH of the solution after the addition of HCl referenced above. C.) Did the buffer solution exceed its buffer capacity?
A. What is the pH of a buffer solution that is composed of 50.0 mL of a 0.25M weak base, Phyllis amine (Ph-NH2) combined with 75.0 mL of 0.23 its salt Phyllis chloride (PHCI)? pKb = 4.65 %3D B. Calculate the new pH of this buffer when 0.301 grams of solid sodium hydroxide is added to the solution. Assume there is no change in volume (MM sodium hydroxide 40.00 g/mol) Show all work on a separate sheet and upload your work. Write your answers in the spaces below: A. The pH of this buffer %3D B. The new pH %3D
12. A 1.00 L buffer solution is 0.150 M in weak organic acid HC₂H5O₂ and 0.250 M in LiC7H5O2. Calculate the pH of the solution after the addition of 0.01 mol HCI. The Ka for HC₂H5O2 is 6.5 x 10-5. (hint: the total volume after adding 100ml of HCl solution turn to 1.00L+100ml = 1.10 L, so molarity calculation should be based off the new volume)
Find the pH and the volume (mL) of 0.527 M HNO3 needed to reach the equivalence point in the titration of 2.65 L of 0.0750 M pyridine (C5H5N, Kb = 1.7 ×10−9)
With a.) 0 mL of NaOH added b.) 10 mL of NaOH added c.) 15 mL of NaOH added d.) 25 mL of NaOH added
12.A buffer was prepared by mixing 65.0 mL of 0.179 M NaHSO3 with 90.0 mL of 0.150 M NazSO3. Ka = 6.4 x 108 a. Determine the pH of this buffer. b. If 0.005 mol of NaOH was added to this buffer, indicate whether the following values would decrease, increase, or remain the same. %3D i. Moles of NaHSO3 ii. Moles of NazS03 pK, value pH value ii. iv.
100 mL of 0.05 M carbonic acid is titrated with 0.5 M NaOH. The first equivalence point is at 30 mL. What is the ph at the first equivalence point, the ph at 37 mL, and the pH at the second equivalence point. (Ka1= 0.0043, ka2= 0.000000000048)
Consider the titration of 20.00 mL of 0.1145 M sodium azide (NaN3) with 0.1250 M HCl. The Ka of HN3 is 2.2 x 10–5. What is the pH at the equivalence point?
A 20.0 mL sample of 0.115M H2SO3 is titrated with 0.1014 M KOH. At what volume (of added base) does each equivalence point occur? a. 25.0mL for the first equivalence point and 50.0mL for the second equivalence point. b. 33.2mL for the first equivalence point and 66.4mL for the second equivalence point. c. 22.7mL for the first equivalence point and 45.4mL for the second equivalence point. d. 20.0mL for the first equivalence point and 40.0mL for the second equivalence point.

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Consider the titration of 100.0 mL of 0.250 M HA (Kα = 5.0 × 10-4, pKa = 3.30) with 0.250 M NaOH. Determine the pH at the equivalence point. a. 7.00 b. 5.80 C. 11.59 d. 8.20 e. 9.86