A buffer which contains 0.50 mol pyruvic acid and0.45 mol sodium pyruvate dissolved in 1.0 L of water has a pHof 2.34. Assuming no significant changes to volume, calculatethe pH when 0.10 mol of NaOH is added to the buffer. (Thepk of pyruvic acid is 2.39)A. 2.34B. 13.00C. 2.15D. 2.52E. How do I do this?[base]pH=pKa + log.[acid]

To solve the problem, we'll use the Henderson-Hasselbalch equation to calculate the pH of the buffer…

Answered: A buffer which contains 0.50 mol…

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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1. A buffer is prepared using 0.522 mol of NH4CI and 0.812 mol of NH3 to make 1.00 L of solution. What is the pH of the solution after adding 0.153 mol of NaOH. Assume that the volume change is negligible. The pKa of NH4Cl is 9.26. 2. A buffer is prepared using 0.636 mol of HO2C2H3 and 0.848 mol of NaO2C2H3 to make 1.00 L of solution. What is the pH of the solution after adding 0.137 mol of HCI. Assume that the volume change is negligible. The pKa of HO2C2H3 is 4.74.
5 a. What is the pH of a buffer made by mixing 0.30M CH3NH2 and 0.36M CH3NH3Br? b. What is the pH of this buffer solution after the addition of 20.0mL of 0.050M NaOH to 80.0mL of the buffer solution? c. What is the pH of the original buffer solution after the addition of 10.0mL of 0.025M HCl to 100.0mL of the buffer solution? Im ready to give up on this problem all help is appreciated.
Did either buffer F or G reach buffer capacity? How do you know? Explain your reasoning.
Given 100.0 mL of a buffer that is 0.50 M in HOCI and 0.60 M in NaOC1, what is the pH after 20.0 mL of 1.0 M NaOH has been added? (K ₂ for HOCI=3.5 × 10-8) a a. 7.55 O b.7.46 O c. 7.70 O d. 7.88 e. 7.63
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.
25). One of your classmates, Chem 109 student said, “I can make a perchlorate buffer using equal amount of 0.1 M HCIO4 and 0.1 M NaCIO4." Will the solution prepared properly by this student functions as a buffer? Another word, can this solution be a buffer? а. yes d. need only ClIO, to make the buffer. c. need only HCIO, to make a perchlorate buffer. e. none of the above b. no
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
.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.
2. Which one of the following is a buffer solution? a. 0.40 M HCN and 0.10 KCN b. 0.20 M СH;COОН c. 1.0 M HNO3 and 1.0 M NANO3 d. 0.10 M KCN с. e. 0.50 M HCl and 0.10 NaCl Why? (Be specific! Also explain why the other 4 choices are NOT buffer solutions.)
5
Determine the volumes of 0.12 M CH3COOH and 0.15 M CH3COONa required to prepare 10 mL of the following pH buffers. (Note: the pKa of CH3COOH =4.7) a. pH 3.8 b. pH 5.0
16. Calculate the pH at the equivalence point in the titration of 25 mL of 0.10 M formic acid with a 0.1 M NaOH solution (given that pka of formic acid = 3.74). A. 4.74 B. 8.74 C. 8.37 D. 6.06 17. When a 0.20 M solution of acetic acid is neutralized with 0.20 M NaOH in 0.50 L of water, the pH of the. resulting solution will be (given that pKa for CH3COOH = 4.74) A. 12.67 B. 7.87 C. 8.87 D. 7.00 18. Calculate the equivalent weight of Na2CO3 when it is titrated against HCI in the presence of phenolphthalein. A. 106 B. 53 C. 26.5 D. 212

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