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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Consider a 1.00 L solution which is 0.010 M CH3CO2H and 0.10 M NaCH3CO2. Ka = 1.8*10-5 a. What is the pH of the initial solution? b. Calculate the pH upon adding 0.004 mol of KOH to the solution. c. How many mL of 10. M HNO3 must be added to the buffer in part A to reduce the pH to 5.00?
2. A solution of pH 12 will contain a large concentration of (fill in) a. Cl- b. Na+ С. ОН- d. H+ ions. Buffers are substances that keep the pH of a solution stable. In blood, the main buffer system is carbonic acid-bicarbonate in which bicarbonate acts as the a. H+ suppressor b. H+ асceptor c. H+ donor d. H+ processor H,CO3 HCO,- + Looking at the above equation we can deduct that if an acidic solution is injected in the blood of a person, the above equilibrium will move to the a. right b. left The action of buffers in the blood is important to keep the pH stable around а. 7.4 b.7.0 с. 7.8 d. 6.8 In the human stomach, digestive enzymes require a high concentration of a. hydroxide ions b. protons c. cholesterol d.inositol for optimal function.
What is the conjugate base of H₂CO3? Select one: a. HCO3 b. H₂CO3 Clear my choice What is the pH of a solution? a. pH = -log[OH-] O b. pH = -log[H3O+] Clear my choice Which set is a buffer solution? a. H3PO4 and K₂HPO4 b. NaOH and H₂O c. d. KH₂PO4 and K₂HPO4 HCI and NaCl
Can you help me with #2
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
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
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?
1. calculate the pH of a solution obtained by mixing 30.4 mL of 0.03 M HCL with 31.4 mL of o.1 M HNO3 solution 2.A given weak acid has a pKa of 8.27. Calculate the percent ionized in 0.34 M of the weak acid. 3. Calculate the pH of 0.021 M Sr(OH )2 PLEASE DO ALL THREE
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.)
Which of the following, when mixed, would NOT result in a buffer solution? а. 10 mL of 0.1M HCI and 20 mL of 0.1 M NH3 O b. 10 mL of 0.1 M HCI and 20 mL of 0.1 M NaC2H3O2 C. 10 mL of 0.1 M NaOH and 20 mL of 0.1 M potassium cyanide, KCN d. 10 mL of 0.1 M NaOH and 20 mL 0.1 M HF e. 10 mL of 0.1 M acetic acid, HC2H3O2, and 10 mL of 0.1 M sodium acetate, NaC2H3O2
Hh.129.
I need help with 3. Determine the pH of the solution at the equivalence point