A student needs to prepare a buffer solution with a pH of 6.00. Assuming a pKą of 4.86, how many mL of 0.1 M B¯ would need to be added to 17.0 mL of 0.1 M HB prepare this buffer? Please include a proper (abbreviated) unit. HINT: Use pH = pKa + log ([B minus]/[HB]) or, if concentrations are the same, pH = pka + log (Volume of B minus/ Volume of HB) Your Answer: Answer units

A student needs to prepare a buffer solution with a pH of 6.00. Assuming a pKą of 4.86, how many mL of 0.1 M B¯ would need to be added to 17.0 mL of 0.1 M HB prepare this buffer? Please include a proper (abbreviated) unit. HINT: Use pH = pKa + log ([B minus]/[HB]) or, if concentrations are the same, pH = pka + log (Volume of B minus/ Volume of HB) Your Answer: Answer units

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...

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Dino needs to prepare 200.0 mLs of a 0.25M /0.20 M buffer solution that has pH of 4.7. To make this buffer solution, Dino has available 0.50 M solutions each of the following: Chemicals .. NH3/NH4CI •HCOOH/HCOOK HONH2/HONH3CI CH3COOH/NaCH3COO ● NH3/NH4CI HONH2/HONH3C HCOOH/HCOOK K₂ Which set of conjugate acid - base pairings should Dino select? CH3COOH/NaCH3COO 1.78 x 10-5 5.62 x 10-10 1.82 x 10-4 9.12 x 10-9
You are given a 1.00 L buffer solution that is 0.250 M in HF and 0.250 M in LiF. Find the pH of the solution after the addition of 0.150 moles of solid LiOH. Assume no volume change upon the addition of base. The Ka for HF is 3.5 × 10-4.
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The Ka of acetic acid is 1.76 ×10-5. Determine the pH of a buffer solution prepared by combining same volume of 1.00 M potassium acetate and 2.00 M acetic acid.
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A student needs to prepare a buffer solution with a pH of 4.18. Assuming a pKa of 4.69, how many mL of 0.1 M NaOH would need to be added to 15.0 mL of 0.1 M HB to prepare this buffer? Please include a proper (abbreviated) unit. HINT : Use pH = pKa + log ([B minus]/[HB]) or, if concentrations are the same, pH = pKa + log (Volume of OH minus/ (Volume of HB minus Volume of OH minus)
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A chemistry graduate student is given 125. mL of a 0.30M methylamine (CH, NH₂) solution. Methylamine is a weak base with K-44×10 what mass of CH, NH, Br should the student dissolve in the CH, NH, solution to turn it into a buffer with pH-10.377 You may assume that the volume of the solution doesn't change when the CH, NH, Br is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits.