5. A common buffer solution can be prepared by using ammonia and ammonium salts. The base equilibrium constant is 1.815×10¯5. A student is preparing a pH buffer solution with 2.561 M NH3 solution and (NH4)2SO4 solid. Please answer the following questions. A. B. What is the best pH buffer range of the buffer solution that can be prepared by NH3 solution and (NH4)2SO4 solid? Please put down "1″ if the answer is pH = 4.741 ± 1, please put down "2" if the answer is pH = 4.741 ± 10, please put down "3" if the answer is pH = 9.26 ± 1, please put down "4" if the answer is pH=9.26 ± 10. Your answer follows. Assume that the addition of the solid will NOT change the volume, how many grams of is needed to prepare a pH = 8.66 buffer solution? The volume of the buffer solution is 250.0 mL. grams

5. A common buffer solution can be prepared by using ammonia and ammonium salts. The base equilibrium constant is 1.815×10¯5. A student is preparing a pH buffer solution with 2.561 M NH3 solution and (NH4)2SO4 solid. Please answer the following questions. A. B. What is the best pH buffer range of the buffer solution that can be prepared by NH3 solution and (NH4)2SO4 solid? Please put down "1″ if the answer is pH = 4.741 ± 1, please put down "2" if the answer is pH = 4.741 ± 10, please put down "3" if the answer is pH = 9.26 ± 1, please put down "4" if the answer is pH=9.26 ± 10. Your answer follows. Assume that the addition of the solid will NOT change the volume, how many grams of is needed to prepare a pH = 8.66 buffer solution? The volume of the buffer solution is 250.0 mL. grams

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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Choose the letter of the correct answer: 1. Which of the following salts will produce a basic solution upon hydrolysis?a. NH4NO3b. K2SO4c. NaC6H5COOd. NH4ClO4 2. What buffer pH can be prepared from an arbitrary weak acid whose pKa is 7.20?a. pH 8.30b. pH 6.40c. pH 2.80d. pH 5.80 3. All salts are products of neutralization reactions between an acid and a base. Thus, all salts form a neutral solution when dissolved.a. Trueb. False 4. Which source of error will cause an increase in buffer capacity during determination?a. Higher volume of the buffer was usedb. pH meter was read prematurely, resulting to a larger pH changec. Large amounts of the NaOH was added to the buffer with minimal pH changed. Large amounts of water was accidentally spilled into the buffer 5. Ions that are derived from strong acids and bases, which neither has acid nor base propertiesa. Hydrolyzable ionsb. Acidic/Basic ionsc. Spectator ionsd. Neutralizer ions
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2. Determine the best answer on the follow:What buffer pH can be prepared from an arbitrary weak acid whose pKa is 7.20?a. pH 8.30b. pH 6.40c. pH 2.80d. pH 5.80 All salts are products of neutralization reactions between an acid and a base. Thus, all salts form a neutral solution when dissolved.a. Trueb. False
show calculations for how the pH of each of these solutions would be determined. a. Buffer solution prepared from 10.00 mL of 1.0 M HC2H3O2 and 10.00 mL of 1.0 M NaC2H3O2 b. 20.00 mL of buffer solution with 1.00 mL of 1.0 M NaOH. c. 20.00 mL of buffer solution with 1.00 mL of 1.0 M HCl. d. 20.00 mL of water with 1.00 mL of 1.0 M NaOH added e. 20.00 mL of water with 1.00 mL of 1.0 M HCl added
4) A buffer solution is made from 135 mL of 0.395 M in HC2H3O2 and 115 mL 0.345 M NaC2H3O2 (the Ka of acetic acid is 1.79 x 10-5). a. Determine the pH of the initial buffer solution. b. What is the buffering range of this solution? c. What is the buffering capacity of this solution? d. What is the maximum volume of 2.00 M HCl solution you can add this buffer before it is no longer effective?
Use the Henderson–Hasselbalch equation to calculate the pH of each solution.a. a solution that is 0.135 M in HClO and 0.155 M in KClOb. a solution that contains 1.05% C2H5NH2 by mass and 1.10% C2H5NH3Br by massc. a solution that contains 10.0 g of HC2H3O2 and 10.0 g of NaC2H3O2 in 150.0 mL of solution
A 200. mL sample of buffer contains 1.20 M CH3NH2 (methylamine) and 1.00 M CH3NH3Cl (methylammonium chloride). a. Write the net ionic equation that shows how the buffer will react with added generic acid H+. b. Write the net ionic equation that shows how the buffer will react with added generic base OH–. c. Determine the pH of this buffer solution. d. Determine the pH of this solution after the addition of 8.0 mL 5.0 M HBr. e. Phenol red is an organic compound that can be used as an acid/base indicator with pKa = 7.2. The two different forms and colors of phenol red are shown. At the pH you determined in part b, what color would you expect the phenol red indicator to be? (Circle one.) yellow, orange, pink, cannot predict
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30.00 mL of 0.200 M benzoic acid (K, = 6.3x105) is titrated with 0.100 M NaOH. Find the pH of the resulting solution after the following volumes of NaOH have been added. a. 0.00 mL b. 20.00 mL c. 60.00 mL d. 75.00 mL
A sample weighing 1.25 g of the diprotic acid potassium acid phthalate (KHP) is dissolved in 50.0 ml of water. Consider the titration of this solution with 0.100 M NaOH. The two Ka’s for KHP are 1.12 x 10-3 and 3.90 x 10-6. a. Calculate the pH of this solution before adding any NaOH. b. How many ml of NaOH must be added to reach the equivalence point? What is the pH at the equivalence point? c. Calculate the pH of the solution after 100. ml of NaOH have been added.
22. Which of the following mixture could be considered as a buffer? Hint: Try to react each mixture (if possible) and look for a pair that could be components for the buffer c. HC1 + CF d. CH3COO+ OH- a. NH4C1 + NAOH b. NH3 + NaOH 23. What is the pH of a buffer solution containing 0.25 M acetic acid and 0.030 M sodium acetate? The acid dissociation constant for acetic acid is equal to 1.8 x 10 Hint no dilution occurred a. 3.82 b. 5.67 C. 10.18 d. 8.34
7. A solution was made by mixing 50.0 mL of 0.750 M HCN with 25.0 mL of water. What is the pH of this solution? The pka of HCN = 9.31. 8. One of the compounds featured on the TV series "Breaking Bad" was hydrofluoric acid (HF), pKa = 3.14. a) A solution of HF has a pH = 1.77. What was the initial [HF] for this solution in mol L-1? b) What is the equilibrium concentration of F in this solution in mol L-1? c) What is the percent ionization of HF in this solution?