Which of the following aqueous solutions are good buffer systems? (Select all that apply.) 0.18 M acetic acid + 0.17 M potassium acetate 0.23 M hydroiodic acid + 0.20 M potassium iodide 0.27 M ammonia + 0.34 M ammonium bromide 0.15 M potassium hydroxide + 0.27 M potassium chloride 0.32 M sodium perchlorate + 0.23 M sodium iodide

Which of the following aqueous solutions are good buffer systems? (Select all that apply.) 0.18 M acetic acid + 0.17 M potassium acetate 0.23 M hydroiodic acid + 0.20 M potassium iodide 0.27 M ammonia + 0.34 M ammonium bromide 0.15 M potassium hydroxide + 0.27 M potassium chloride 0.32 M sodium perchlorate + 0.23 M sodium iodide

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 0.175 M in a weak acid and 0.200 M in the acids conjugate base? The acids ionization constant is 5.7 104.
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?
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?
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
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?(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
Which of the following aqueous solutions are good buffer systems? O 0.33 M ammonia + 0.39 M sodium hydroxide 0 0.16 M potassium hydroxide + 0.29 M potassium bromide V 0.16 M acetic acid + 0.10 M sodium acetate O 0.31 M calcium chloride + 0.23 M sodium chloride O 0.28 M hydroiodic acid + 0.21 M sodium iodide please explain each than solve
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
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?. 0.12 M potassium acetate + 0.20 M acetic acid 0.18 M nitrous acid + 0.18 M potassium nitrite 0.31 M ammonium bromide + 0.35 M ammonia 0.38 M hydrocyanic acid + 0.21 M potassium cyanide 0.24 M hydroiodic acid + 0.23 M sodium iodide
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
Which of the following aqueous solutions are good buffer systems?. 0.34 M nitrous acid + 0.27 M potassium nitrite 0.30 M ammonium bromide + 0.31 M ammonia 0.15 M sodium hypochlorite + 0.22 M hypochlorous acid 0.28 M nitric acid + 0.23 M sodium nitrate 0.14 M hydrocyanic acid + 0.11 M potassium cyanide you can choose multiple choices if needed.