A 100.0 mL buffer solution is constructed using 0.035 M HX, a weak acid, and 0.045 M NaX. Ka, HX = 4.7 x 106 a) Based on the K,, what is the pH range where the buffer should be effective. b) From the given concentrations, what is the actual pH of the constructed buffer. c) What would the pH of the buffer if 0.0020 mol of HCl is added to the buffer solution.

A 100.0 mL buffer solution is constructed using 0.035 M HX, a weak acid, and 0.045 M NaX. Ka, HX = 4.7 x 106 a) Based on the K,, what is the pH range where the buffer should be effective. b) From the given concentrations, what is the actual pH of the constructed buffer. c) What would the pH of the buffer if 0.0020 mol of HCl is added to the buffer solution.

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

why is the pH of a buffer solution relatively unchanged upon dilution? (Hint: Show a calculation that illustrates why diluting a buffer does not change its pH)
Please don't provide hand written solution.....
A chemistry graduate student is given 100. mlL of a 0.10 M chlorous acid (HCIO,) solution. Chlorous acid is a weak acid with K,-1.1x 10. what mass of KCIO, should the student dissolve in the HCIO, solution to turn it into a buffer with pH = 1.96? You may assume that the volume of the solution doesn't change when the KCIO, is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. ?
Please don't provide handwritten solution .... What is the pH after 0.150 mol of HCl is added to the buffer from Part A? Assume no volume change on the addition of the acid. Express the pH numerically to three decimal places.
A 28.3 ml sample of 0.375 M diethylamine, (C,Hs),NH, is titrated with 0.270 M nitric acid. After adding 14.5 mL of nitric acid, the pH is Use the Tables link in the References for any equilibrium constants that are required.
A buffer solution contains 0.471 M KHC0; and 0.349 M Na,CO3. Determine the pH change when 0.106 mol KOH is added to 1.00 L of the buffer. pH after addition – pH before addition = pH change =|
Give detailed Solution...
Please don't provide handwritten solution...
18) What is the pH of a 100ml solution formed by adding 0.1mole NaOH to a buffer solution that contains 0.25 mole HF and 0.15 mole NaF? (K, = 6.8 x 10* for HF)
A 27.4 mL sample of 0.356 M ammonia, NH3, is titrated with 0.279 M hydrobromic acid. At the titration midpoint, the pH is Use the Tables link in the References for any equilibrium constants that are required.
An aqueous solution contains 0.26 M ammonium iodide. One liter of this solution could be converted into a buffer by the addition of: (Assume that the volume remains constant as each substance is added.) (Select all that apply.) 0.25 mol NH3 0.26 mol HNO3 0.12 mol HNO3 0.25 mol Nal 0.06 mol Ca(OH)2
How many mol of HCI would have to be added to 0.692 L of a 4.813 M B: in order to obtain a buffer with a pH of 8.79? (The Kb for B: is 6.05 10-2). Assume there is no volume change. mol HCI