11.The pKa of a weak acid was determined by measuring the pH of a solutioncontaining the weak acid at 0.40 M and its conjugate base at 0.60 M. Themeasured pH was 7.8. What is the pKa of the weak acid?a. 8.0b. 7.8c. 7.6d. 7.0e. 7.4

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Answered: 11.The pKa of a weak acid was…

Chemistry

10th Edition

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

Section: Chapter Questions

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

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Which of the following is true about the titration curves of solutions of weak acids? A. The pH for optimal buffering power of a weak acid is 7.00. B. You can calculate the pKa of an acid, given the pH and the molar ratio of the acid and its conjugate base. C. The pKa of a weak acid is the pH at which the acid is completely dissociated. D. At a pH below the pKa of a weak acid, its conjugate base will predominate.
A 0.150 M 1-naphthoic acid solution was titrated with 0.500 M NaOH. The equivalence point was reached after the addition of 0.30 mL of NaOH, as indicated by the data in the graph below. What is the estimated pK₁ of 1-naphthoic acid? (You may need to scroll down to see the entire image.) A. 4.4 ✓B. 3.7 C. 4.0 D. 3.4 12.00 11.80 11.60 11.40 11.20 11.00 10.80 10.60 10.40 10.20 10.00 9.80 9.60 9.40 9.20 9.00 8.80 8.60 8.40 8.20 8.00 7.80 160 7.60 7-40 7.20 7.00 6.80 6.60 6.40 6.20 6.00 5.80 5.60 5-40 5.20 5.00 4.80 4.60 4-40 4-20 Va 4.00 3.80 3.60 3-40 3.20 3.00 2.80 2.60 2-40 2.20 0.00 0.05 0.10 0.15 0.20 mL added NaOH 0.25 0.30 0.35
.H. Park 19. A buffer solution is made from 0.100 M HC3H5O2 and 0.100 M NaC3H5O2. The pKa of HC3H5O2 is 4.88. a. Calculate the pH of the solution. b. Calculate the pH after 0.0250 mol of HCl(g) is added to 500.0 mL of the buffer.
a. Give the chemical equation for the dissociation of PbCl2. b. What is the molar solubility of PbCl2? c. What are the equilibrium concentration of the ions?
A 40.00 solution of 0.1430 M chloroacetic acid (pK a = 2.865) is titrated with a 0.1500 M solution of NaOH. a. Find the initial pH of the solution. b. Find the pH of the resulting solution at the half-equivalence point. c. Find the pH of the resulting solution at the equivalence point. d. Find the pH of the resulting solution at 0.50 mL past the equivalence point.
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Chemistry a malate buffer solution.

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11.The pKa of a weak acid was determined by measuring the pH of a solution containing the weak acid at 0.40 M and its conjugate base at 0.60 M. The measured pH was 7.8. What is the pKa of the weak acid? a. 8.0 b. 7.8 c. 7.6 d. 7.0 e. 7.4