Which of the following solutions is a good buffer system? A. A solution that is 0.10 M HC2H3O2 and 0.10 M LİC2H3O2 B. A solution that is 0.10 M HF and 0.10M NaC2H3O2 C. A solution that is 0.10 M HCI and 0.10 M NH4* D.A solution that is 0.10 M NaOH and 0.10 M KOH E. None of the above are buffer systems.

Which of the following solutions is a good buffer system? A. A solution that is 0.10 M HC2H3O2 and 0.10 M LİC2H3O2 B. A solution that is 0.10 M HF and 0.10M NaC2H3O2 C. A solution that is 0.10 M HCI and 0.10 M NH4* D.A solution that is 0.10 M NaOH and 0.10 M KOH E. None of the above are buffer systems.

Chemistry & Chemical Reactivity

9th Edition

ISBN:9781133949640

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter17: Principles Of Chemical Reactivity: Other Aspects Of Aqueous Equilibria

Section17.2: Controlling Ph: Buffer Solutions

Problem 1RC: 1. Which choice would be a good buffer solution? 0.20 M KCH3CO2 and 0.20 M CH3CO2H 0.20 M HCl and...

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Similar questions

a Draw a pH titration curve that represents the titration of 50.0 mL of 0.10 M NH3 by the addition of 0.10 M HCl from a buret. Label the axes and put a scale on each axis. Show where the equivalence point and the buffer region are on the titration curve. You should do calculations for the 0%, 30%, 50%, and 100% titration points. b Is the solution neutral, acidic, or basic at the equivalence point? Why?
A 30.0-mL sample of 0.05 M HClO is titrated by a 0.0250 M KOH solution Ka for HClO is 3.5 108. Calculate a the pH when no base has been added; b the pH when 30.00 mL of the base has been added; c the pH at the equivalence point; d the pH when an additional 4.00 mL of the KOH solution has been added beyond the equivalence point.
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.
1. Which choice would be a good buffer solution? 0.20 M KCH3CO2 and 0.20 M CH3CO2H 0.20 M HCl and 0.10 M KOH 0.20 M CH3CO2H and 0.10 M HCO2H 0.10 HCl and 0.010 M KCl
What is meant by the capacity of a buffer? Describe a buffer with low capacity and the same buffer with greater capacity.
A buffer solution is prepared by adding 0.125 mol ammonium chloride to 500. mL of 0.500-M aqueous ammonia. Calculate the pH of the buffer. If 0.0100 mol HCl gas is bubbled into 500. mL buffer and all of the gas dissolves, calculate the new pH of the solution.
Mixing together solutions of acetic acid and sodium hydroxide can make a buffered solution. Explain. How does the amount of each solution added change the effectiveness of the buffer?
You want to make a buffer with a pH of 10.00 from NH4+/NH3. (a) What must the [ NH4+ ]/[ NH3 ]ratio be? (b) How many moles of NH4Cl must be added to 465 mL of an aqueous solution of 1.24 M NH3 to give this pH? (c) How many milliliters of 0.236 M NH3 must be added to 2.08 g of NH4Cl to give this pH? (d) What volume of 0.499 M NH3 must be added to 395 mL, of 0.109 M NH4Cl to give this pH?
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.
A 0.239-g sample of unknown organic base is dissolved in water and titrated with a 0.135 M hydrochloric acid solution. After the addition of 18.35 mL of acid, a pH of 10.73 is recorded. The equivalence point is reached when a total of 39.24 mL of HCl is added. The base and acid combine in a 1:1 ratio. a What is the molar mass of the organic base? b What is the Kb value for the base? The Kb value could have been determined very easily if a pH measurement had been made after the addition of 19.62 mL of HCl. Why?

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