Which of the following aqueous solutions are good buffer systems?(Select all that apply.)0.25 M ammonium nitrate + 0.31 M ammonia0.39 M hydrofluoric acid + 0.23 M sodium fluoride0.21 M hydrocyanic acid + 0.14 M potassium cyanide200.12 M potassium hypochlorite + 0.20 M hypochlorous acid0.26 M hydroiodic acid + 0.18 M potassium iodideSubmit Answer$4000000 F4RShow Hint%[Review Topics)[References]Use the References to access important values if needed for this question.Retry Entire Group 9 more group attempts remainingTCengage Learning Cengage Technical SupportF5A6MacBook AirF6&F7U*8F81▶9F9F104)PAPreviF11

The given problem is based on the preparation of buffer solutions.

Use the References to access important values if 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 0.12 M potassium hypochlorite + 0.20 M hypochlorous acid 0.26 M hydroiodic acid + 0.18 M potassium iodide

Use the References to access important values if 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 0.12 M potassium hypochlorite + 0.20 M hypochlorous acid 0.26 M hydroiodic acid + 0.18 M potassium iodide

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter15: Acid–base Equilibria

Section: Chapter Questions

Problem 56P

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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?
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.
Consider the weak acids in Table 13.2. Which acid-base pair would be best for a buffer at a pH of (a) 3.0(b) 6.5 (c) 12.0
A student intends to titrate a solution of a weak monoprotic acid with a sodium hydroxide solution but reverses the two solutions and places the weak acid solution in the buret. After 23.75 mL of the weak acid solution has been added to 50.0 mL of the 0.100 M NaOH solution, the pH of the resulting solution is 10.50. Calculate the original concentration of the solution of weak acid.
Enough water is added to the buffer in Question 30 to make the total volume 5.00 L. (a) Calculate the pH of the buffer. (b) Calculate the pH of the buffer after adding 0.0250 mol of HCl to 0.376 L of the buffer. (c) Calculate the pH of the buffer after adding 0.0250 mol of KOH to 0.376 L of the buffer. (d) Compare your answers to Question 30 (a-c) with your answers to (a-c) of this problem. (e) Comment on the effect of dilution on the pH of a buffer and on its buffer capacity. Â
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?
A buffer solution that is 0.100 M acetate ion and 0.100 M acetic acid is prepared. (a) Calculate the initial pH, final pH, and change in pH when 1.00 mL of 1.00 M NaOH is added to 100.0 mL of the buffer. (b) Calculate the initial pH, final pH, and change in pH when 1.00 mL of 1.00 M NaOH is added to 100.0 mL pure (pH 7.00) water.
2. If an acetic acid/sodium acetate buffer solution is prepared from 100. mL of 0.10 M acetic acid what volume of 0.10 M sodium acetate must be added to have a pH of 4.00? 100. mL 50. mL 36 mL 18 mL
A solution of weak base is titrated to the equivalence point with a strong acid. Which one of the following statements is most likely to be correct? a The pH of the solution at the equivalence point is 7.0. b The pH of the solution is greater than 13.0. c The pH of the solution is less than 2.0. d The pH of the solution is between 2.0 and 7.0. e The pH of the solution is between 7.0 and 13.0. The reason that best supports my choosing the answer above is a Whenever a solution is titrated with a strong acid, the solution will be very acidic. b Because the solution contains a weak base and the acid (titrant) is used up at the equivalence point, the solution will be basic. c Because the solution contains the conjugate acid of the weak base at the equivalence point, the solution will be acidic.

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