1. Which of the following is/are true when NH4Br is dissolved in water? I. Both NH4* and Br" are hydrolysable ions resulting in a neutral solution. II. The salt will completely dissociate into NH4* and Br ions in the solution. III. The Brion is considered as the hydrolysable ion and thus an acidic solution will form. IV. The most probable pH of the solution is acidic due to the hydrolysis of the NH4* ion. OI and II OII and III O II and IV Land Y

1. Which of the following is/are true when NH4Br is dissolved in water? I. Both NH4* and Br" are hydrolysable ions resulting in a neutral solution. II. The salt will completely dissociate into NH4* and Br ions in the solution. III. The Brion is considered as the hydrolysable ion and thus an acidic solution will form. IV. The most probable pH of the solution is acidic due to the hydrolysis of the NH4* ion. OI and II OII and III O II and IV Land Y

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter15: Acid-base Equilibria

Section: Chapter Questions

Problem 8ALQ: You have a solution of the weak acid HA and add some of the salt NaA to it. What are the major...

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. The concepts of acid-base equilibria were developed in this chapter for aqueous solutions (in aqueous solutions, water is the solvent and is intimately involved in the equilibria). However, the Brønsted-Lowry acid-base theory can be extended easily to other solvents. One such solvent that has been investigated in depth is liquid ammonia. NH3. a. Write a chemical equation indicating how HCl behaves as an acid in liquid ammonia. b. Write a chemical equation indicating how OH- behaves as a base in liquid ammonia.
Use the data in Table 15.1 to select a conjugate acid-base pair you could use to make buffer solutions having each of these hydrogen ion concentrations. 3.2 × 10−4 M 5.0 × 10−5 M 7.0 × 10−8 M 6.0 × 10−11 M
2. Given the H3PO4 - NaH₂PO4 buffer system, which of the following is false when KOH is added into the said solution? O The concentration of the H3PO4 will decrease upon addition of KOH. O The concentration of the H₂PO4 will decrease upon addition of KOH. O The concentration of the H₂PO4 will increase upon addition of KOH. O The [H₂PO4 ]/[H3PO4] will decrease due to the neutralization of the added KOH.
1. Which of the following is/are true when Ca(CH3COO)2 is dissolved in water? 1. The salt will completely dissociate into Ca2+ and CH3COO ions in the solution. II. Both Ca²+ and CH3COO are hydrolysable ions resulting in a neutral solution. III. The Ca²+ ion is considered as the hydrolysable ion and thus a basic solution will form. IV. The most probable pH of the solution is basic due to the hydrolysis of the CH3COO ion. OI and II O II and III O II and IV O I and IV
Which of the following is/are true when NH Br is dissolved in water? 1. Both NH4 and Br are hydrolysable ions resulting in a neutral solution. II. The salt will completely dissociate into NH4+ and Br ions in the solution. III. The Br ion is considered as the hydrolysable ion and thus an acidic solution will form. IV. The most probable pH of the solution is acidic due to the hydrolysis of the NH4+ ion. A. I and II B. II and III C. II and IV D. I and IV
19. A student prepared a 250.0 mL solution by dissolving 4.559 g of (NH4)2SO4 in enough water. The temperature is 298 K. The base dissociation constant for NH3 is 1.796x10-5. Please answer the following questions. A. B. What is the equilibrium concentration of H3O+ in the solution? Please provider your answer below. 00 + → What is the equilibrium concentration of OH in the solution? Please provider your answer below. OO → $ → $ C. What is the pH of the solution? pH = Please provider your answer below. S M M
H8. Describe the difference between a buffered and an unbuffered solution. Explain the significance of a buffer solution in a real-life application. Provide a unique example in your discussion
1. Which of the following is/are true when Ca(CH3COO)2 is dissolved in water? 1. The salt will completely dissociate into Ca²+ and CH3COO ions in the solution. II. Both Ca2+ and CH3COO are hydrolysable ions resulting in a neutral solution. III. The Ca2+ ion is considered as the hydrolysable ion and thus a basic solution will form. IV. The most probable pH of the solution is basic due to the hydrolysis of the CH3COO ion. O I and II O II and III O II and IV I and IV
Let X represent a nonmetal. Which of the following buffer solutions functions at the lowest pH? More information is needed to make a determination. О.15 М НХО and O.10 M NaXO 0.15 М НХОЗ аnd O.10 M NaXОз О.15 М НХО2 and O.10 M NaXО2 О.15 М НХО4 and O.10 M NaXО4
Calculate the ratio [NH3]/[NH4+] in ammonia/ammonium chloride buffered solutions with the following pH values: (This problem requires values in your textbook's specific appendices, which you can access through the OWLV2 MindTap Reader. You should not use the OWLv2 References' Tables to answer this question as the values will not match. Simplify your answer completely.) a. pH = 9.00 [NH3] %3D [NH, *] b. pH = 8.10 [NH3] [NH,* c. pH = 10.60 [NH3] [NH, *] d. pH = 9.60 NH3] [NH, +] Submit Answer Try Another Version 6 item attempts remaining
B. Determination of the hydrolysis constant (or acid dissociation constant, Ka) of NH4+. 1. Consider a 0.01 M NH4CI solution. 2. Write the dissociation equation for NH4CI. 3. Identify the ion/s that can undergo hydrolysis. 4. It has been determined experimentally that the pH of 0.01 M NH4CI solution is 5.91. From the pH of the solution, solve for the concentration of all species present in the solution. Input all your answers in Tables 2 and 3. 5. Solve for the Ka of NH4+. 6. Compare your experimental value to the literature value for the Ka of NH4+. B. Determination of the hydrolysis constant (or acid dissociation constant, Ka) of NH4*. Table 2. Dissociation of NH,CI Dissociation equation of NH4CI pH of solution lon that undergoes hydrolysis: Hydrolysis reaction Table 3. ICE Table for the Hydrolysis of NH4* Parameter [NH,*] [H*] [NH3] Initial concentration Change in concentration Equilibrium Concentration Solving for the hydrolysis constant, Kn (or Ka) of NH4+ Theoretical Value for Ka…
Which of the following is true for a buffered solution? a. The solution resists change in its [H+]. b. The solution will not change its pH very much even if a concentrated acid is added. c. The solution will not change its pH very much even if a strong base is added. d. Any H+ ions will react with a conjugate base of a weak acid already in solution. e. All of these.