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

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

Calculate the pH of the solution after the addition of each of the given amounts of 0.0691 M HNO, to a 50.0 mL solution of 0.0750 M aziridine. The pKa of aziridinium is 8.04. What is the pH of the solution after the addition of 0.00 mL HNO3? pH 10.457 What is the pH of the solution after the addition of 6.19 mL HNO,? 9.32 pH = Incorrect What is the pH of the solution after the addition of a volume of HNO, equal to half the equivalence point volume? 8.04 pH What is the pH of the solution after the addition of 51.1 mL HNO,? 6.58 pH = Incorrect What is the pH of the solution after the addition of a volume of HNO, equal to the equivalence point? pH = 4.76 What is the pH of the solution after the addition of 57.7 mL HNO,? 2.87
Please help in solving e-f of question. Thanks
An analytical chemist is titrating 221.9 mL of a 0.8100M Solution of diethylamine ((C,H3),NH) with a 0.7200M Solution of The pK, of diethylamine is 2.89. Calculate the pH of the base solution after the chemist has added 131.7 mL of the HNO, solution to it. HNO3. 2 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 = U
5. Determine the pH of the resulting solutions when the following reagents are mixed. a. 20.00mL of 0.2500M HCI mixed with 35.00mL of 0.2250M NaOH b. 18.00mL of 0.3500M HC₂H3O2 mixed with 15.00mL of 0.3000M NaOH c. 22.50mL of 0.2000M NH3 mixed with 25.00mL of 0.1000M HCI d. 25.00mL of 0.1000M HClO₂ mixed with 25.00mL of 0.1000M KOH e. 15.00mL of 0.1000M CH3NH₂ mixed with 25.00mL of 0.1500M HCI
An analytical chemist is titrating 71.3 mL of a 1.000M solution of formic acid (H,CO,) with a 0.6600M solution of KOH. The pK, of formic acid is 3.74. Calculate the pH of the acid solution after the chemist has added 119. mL of the KOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of KOH Solution added. Round your answer to 2 decimal places. pH =
8) Determine the pH of the following solutions: a) 0.20 M CH3COOH b) 0.025 moles of CH3NH3CI dissolved in 1.50A102 mL of water c) 0.15 M solution of Cr(NO3)3 d) 0.25 M NazCO3 pKa of Cr+ is 3.89
17. Determine the pH of the resulting solutions when the following reagents are mixed. a. 20.00mL of 0.2500M HCI mixed with 35.00mL of 0.2250M NaOH b. 18.00mL of 0.3500M HC2H;O2 mixed with 15.00mL of 0.3000M NaOH 22.50mL of 0.2000M NH, mixed with 25.00mL of 0.1000M HCI d. 25.00mL of 0.1000M HCIO, mixed with 25.00mL of 0.1000M KOH e. 15.00mL of 0.1000M CH3NH2 mixed with 25.00mL of 0.1500M HCI
I love you, Bartleby. Thank you for saving my life and career. I've learned so much!
C. increases by one A. decreases by one B. decreases by one tenth In a solution, when the concentrations of a weak acid and its conjugate base are equal, A. the system is not at equilibrium. D. increases ten fold B. the buffering capacity is significantly decreased. C. the -log of the [H*] and the -log of the K, are equal. D. all of the above are true. p. Consider a solution which is 0.10M in CH3COOH and 0.20 M in NaCH;COO. Which of the following statements is TRUE?
1. Create a set of rules for determining which anions and cations will react with water (Hydrolyze) and which won't. Then write another set of rules to describe what happens when a cation reacts with water, and what happens when an anion reacts with water. 2. What is the pH of a solution made by dissolving 8.50 g of potassium formate, KCHO2, in 500.0 mž of 0.100M formic acid, HCHO2. State any assumptions you need to make to answer this question.
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…
Consider a solution of Hydrofluoric acid at equilibrium as follows:HF (aq)+H2O (l) F ̄ (aq)+H3O+ (aq) a.Suppose a strong base (OH-) is added to the buffer system above. Which two species could react and why? b.Write the chemical reaction for the reaction of hydroxide ion (OH-) being neutralized by reacting with the hydrofluoric acid. c.Explain why the addition of a small amount of strong base will not cause a significant change in the pH of the solution as long as the HF is not used up. d. Suppose a strong acid (H3O+) is added to the buffer system above. Which species could react and why? e.Write the chemical reaction for the reaction of hydronium ion (H3O+) being neutralized by reacting with the fluoride ion. f.Explain why the addition of a small amount of strong acid will not cause a significant change in the pH of the solution as long as the fluoride ion (F ̄) is not used up.