Which of the following statements is true about a 1-L buffer solution prepared by mixing 1.13 mol propionic acid (C2H5COOH) and 2.03 mol sodium propionate (C2H5COONA)? Ka(C2H5COOH) = 1.34 x 10-5. The pH of the above buffer solution is less than the pka of C2H5COOH. b. By adding water to dilute the above buffer solution, the pH of the buffer solution will decrease. O. The pH of the above buffer solution is greater than the pKą of C2H5COOH. By readjusting the amount of propionic acid and sodium propionate, we can prepare a buffer solution ´at pH = 8.00. %3D e. By adding water to dilute the above buffer solution, the pH of the buffer solution will increase.

Which of the following statements is true about a 1-L buffer solution prepared by mixing 1.13 mol propionic acid (C2H5COOH) and 2.03 mol sodium propionate (C2H5COONA)? Ka(C2H5COOH) = 1.34 x 10-5. The pH of the above buffer solution is less than the pka of C2H5COOH. b. By adding water to dilute the above buffer solution, the pH of the buffer solution will decrease. O. The pH of the above buffer solution is greater than the pKą of C2H5COOH. By readjusting the amount of propionic acid and sodium propionate, we can prepare a buffer solution ´at pH = 8.00. %3D e. By adding water to dilute the above buffer solution, the pH of the buffer solution will increase.

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...

See similar textbooks

Similar questions

You have 0.100 M solutions of acetic acid ( p?a = 4.76 ) and sodium acetate. If you wanted to prepare 1.00 L of 0.100 M acetate buffer of pH 4.00 , how many milliliters of acetic acid and sodium acetate would you add?
Calculate the pH of solution after the addition of 0.010 mol NaOH to 1.00L of a 0.100 M acetic acid / 0.100 M sodium acetate buffer solution. (Ka = 1.8 x 10*) What is the neutralization reaction that happens? Is the system still a buffer after neutralization?
What is the pH of a solution that results when 3.00 mL of 0.034 M HCl is added to 0.200 L of a buffer solution is prepared from equal volumes of 0.200 M acetic acid and 0.600 M sodium acetate. (The Ka for acetic acid is 1.80 ×10-5.)
The pK, value for HCN is 9.40. Would a buffer prepared from HCN and KCN with a pH of 11.4 be considered to be an effective buffer? A buffer in which the mole ratio of KCN to HCN is 0.60 has a pH of 9.18. Would this buffer solution have a greater capacity for added acid (H30*) or added base (OH )?
Consider a buffer made by adding 132.8 g of NaC₇H₅O₂ to 300.0 mL of 2.35 M HC₇H₅O₂ (Ka = 6.3 x 10⁻⁵) a What is the pH of this buffer? b What is the pH of the buffer after 0.750 mol of H⁺ have been added? c What is the pH of the buffer after 0.250 mol of OH⁻ have been added?
Consider a buffer made by dissolving 0.140 mol cyanic acid, HCNO, and 0.11 mol potassium cyanate, KCNO, in enough water to make a 1-L solution. Assuming that the volume does not change, what is the pH of the buffer before any acid or base is added? Ka = 3.5 x 10-4 O 3.46 O 3.25 3.36 O None of the above
A buffer contains 0.175 moles C2H5NH3NO3 and 0.225 moles C2H5NH2 in 800.0 mL water. Kp (C2H5NH2) = 4.3 x 104 Express value to three decimal places. Determine the number of moles of base that can be added before the buffer capacity is exceeded. moles base F TOOLS x10
O ACIDS AND BASES Calculating the pH of a weak base titrated with a strong acid with a 0.3000 M solution of HNO,. The p K, of An analytical chemist is titrating 160.2 mL of a 0.5000 M solution of dimethylamine ((CH₂)2NH) w dimethylamine is 3.27. Calculate the pH of the base solution after the chemist has added 280.8 mL of the HNO, solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO, solution added. Round your answer to 2 decimal places... PH-0 X
Which is true about buffer solutions? -they hold the pH close to the pKa -they contain comparable moles of a weak acid and a strong base - they hold pH constant at pH=7 -they prevent acids and bases from reaching equilibrium -they hold the pH close to the equivalence point pH
To create a buffer solution, 40.00mL of a 0.100M benzoic acid (Bz) solution are mixed with 20.00mL of 0.100M sodium hydroxide solution. What is the pH of the resulting solution if the Ka of benzoic acid 6.5 x10 -5 and the pKa = 4.19? (Use the Henderson Hasselbach Equation with mmol). Reaction: HOBz + OH- ---> H2O + OBz- From the buffer solution above, youo take a 10.00mL portion of the buffer. Using all of the information provided, how much conjugate acid and conjugate base are in the 10.00mL portion that you took out? Group of answer choices 0.167mmol 0.500mmol 0.222mmol 0.333mmol