Which of the following aqueous solutions are good buffer systems? (Select all that apply.) 0.12 M sodium fluoride + 0.21 M hydrofluoric acid 0.25 M nitric acid + 0.23 M potassium nitrate 0.30 M ammonium nitrate + 0.39 M ammonia 0.16 M nitrous acid + 0.20 M sodium nitrite 0.39 M hydrocyanic acid + 0.29 M potassium cyanide

Which of the following aqueous solutions are good buffer systems? (Select all that apply.) 0.12 M sodium fluoride + 0.21 M hydrofluoric acid 0.25 M nitric acid + 0.23 M potassium nitrate 0.30 M ammonium nitrate + 0.39 M ammonia 0.16 M nitrous acid + 0.20 M sodium nitrite 0.39 M hydrocyanic acid + 0.29 M potassium cyanide

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter16: Reactions Between Acids And Bases

Section: Chapter Questions

Problem 16.5QE

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What is the pH of a buffer that is 0.150 M in a weak acid and 0.150 M in the acids conjugate base? The acids ionization constant is 6.8 106.
Each symbol in the box below represents a mole of a component in one liter of a buffer solution; represents the anion (X-), = the weak acid (HX), = H+, and =OH. Water molecules and the few H+ and OH- ions from the dissociation of HX and X- are not shown. The box contains 10 mol of a weak acid, , in a liter of solution. Show what happens upon (a) the addition of 2 mol of OH- (2 ). (b) the addition of 5 mol of OH- (5 ). (c) the addition of 10 mol of OH- (10 ). (d) the addition of 12 mol of OH- (12 ). Which addition (a)-(d) represents neutralization halfway to the equivalence point?
Draw the general titration curve for a strong acid titrated by a strong base. At the various points in the titration, list the major species present before any reaction takes place and the major species present after any reaction takes place. What reaction takes place in a strong acidstrong base titration? How do you calculate the pH at the various points along the curve? What is the pH at the equivalence point for a strong acidstrong base titration? Why?
Which of the following aqueous solutions are good buffer systems?(more than one answer maybe required) a) 0.40 M sodium bromide + 0.30 M calcium bromide b) 0.25 M ammonia + 0.31 M barium hydroxide c) 0.14 M hypochlorous acid + 0.17 M sodium hypochlorite d) 0.25 M hydrochloric acid + 0.23 M potassium chloride e) 0.14 M potassium hydroxide + 0.24 M potassium chloride
Use the References to access important values if needed for this question. Which of the following aqueous solutions are good buffer systems? (Select all that apply.) 0.17 M hydrocyanic acid + 0.19 M sodium cyanide 0.21 M perchloric acid + 0.18 M potassium perchlorate 0.28 M ammonia + 0.33 M ammonium bromide 0.18 M barium hydroxide + 0.22 M barium bromide 0.35 M calcium nitrate + 0.22 M calcium chloride
Use the References to access important values if needed for this question. Which of the following aqueous solutions are good buffer systems? (Select all that apply.) 0.12 M hypochlorous acid + 0.21 M sodium hypochlorite 0.23 M perchloric acid + 0.25 M potassium perchlorate 0.29 M ammonium nitrate + 0.37 M ammonia 0.17 M barium hydroxide + 0.25 M barium bromide 0.31 M hydrofluoric acid + 0.23 M potassium fluoride
Which of the following aqueous solutions are good buffer systems? (more than one answer maybe needed) a) 0.31 M potassium iodide + 0.26 M barium iodide. b) 0.13 M nitrous acid + 0.12 M hydrobromic acid. c) 0.26 M ammonia + 0.33 M ammonium bromide. d) 0.11 M sodium hydroxide + 0.25 M sodium chloride. e) 0.28 M perchloric acid + 0.19 M potassium perchlorate.
Which of the following aqueous solutions are good buffer systems? (Select all that apply.) 0.22 M nitrous acid + 0.11 M potassium nitrite 0.29 M hydroiodic acid + 0.25 M potassium iodide 0.13 M potassium fluoride + 0.23 M hydrofluoric acid 0.33 M ammonium bromide + 0.38 M ammonia 0.33 M hypochlorous acid + 0.25 M potassium hypochlorite
ess impor Which of the following aqueous solutions are good buffer systems? (Select all that apply.) 0.18 M acetic acid + 0.17 M sodium acetate 0.27 M hydroiodic acid + 0.24 M potassium iodide 0.32 M ammonium nitrate + 0.31 M ammonia Use the References to 0.12 M calcium hydroxide + 0.22 M calcium chloride 0.37 M hypochlorous acid + 0.25 M potassium hypochlorite Submit Answer Retry Entire Group 7 more group attempts remaining ues ir needed tо
Which of the following aqueous solutions are good buffer systems? O0.19 M hydrocyanic acid + 0.16 M potassium cyanide 0.23 M hydrochloric acid + 0.15 M sodium chloride 0.37 M calcium bromide + 0.24 M potassium bromide 0.35 M ammonia + 0.30M barium hydroxide O 0.13 M calcium hydroxide + 0.22 M calcium chloride Submit Answer Retry Entire Group 9 more group attempts remaining
Which of the following aqueous solutions are good buffer systems? (Select all that apply.) 0.25 M ammonium nitrate + 0.31 M ammonia 0.39 M hydrofluoric acid + 0.23 M sodium fluoride 0.21 M hydrocyanic acid + 0.14 M potassium cyanide 20 0.12 M potassium hypochlorite + 0.20 M hypochlorous acid 0.26 M hydroiodic acid + 0.18 M potassium iodide Submit Answer $ 4 000 000 F4 R Show Hint % [Review Topics) [References] Use the References to access important values if needed for this question. Retry Entire Group 9 more group attempts remaining T Cengage Learning Cengage Technical Support F5 A 6 MacBook Air F6 & F7 U * 8 F8 1 ▶ 9 F9 F10 4) P A Previ F11
Which of the following aqueous solutions are good buffer systems? (Select all that apply.) 0.30 M hydroiodic acid + 0.17 M sodium iodide O 0.30 M ammonia + 0.39 M ammonium bromide 0.36 M barium bromide + 0.22 M potassium bromide O 0.14 M hypochlorous acid + 0.20 M perchloric acid O 0.18 M potassium hydroxide + 0.23 M potassium chloride