5. Prepare a buffer with a pH of 5.3 by selecting the correct weak acid and its conjugatebase:a. H2SO3/HSO3pKa =1.77b. HNO2/NO2pKa = 3.34C. NH3 /N3pKa = 4.72d. HCIO/CIOpKa = 7.54e. HIO/IOpka10.64

The best way to choose a buffer combination from pKa is by choosing from close proximity to the…

Answered: 5. Prepare a buffer with a pH of 5.3 by…

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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Acetic acid has a Ka of 1.8 x 10¬º. Three acetic acid/acetate buffer solutions, A, B, and C, were made using varying concentrations: A. [acetic acid] ten times greater than [acetate], B. [acetate] ten times greater than [acetic acid], and C. [acetate] = [acetic acid]. Match each buffer to the expected pH. Drag the appropriate items to their respective bins. • View Available Hint(s) Reset Help [acetate] ten times greater than [acetic acid] [acetate] = [acetic acid] [acetic acid] ten times greater than [acetate] pH = 3.74 pH = 4.74 pH = 5.74
A buffered solution containing dissolved aniline, C6H5NH2, and aniline hydrochloride, C6H5NH3Cl, has a pH of 5.39. A. Determine the concentration of C6H5NH3+ in the solution if the concentration of C6H5NH2 is 0.215 M. The p?b of aniline is 9.13. [C6H5NH3+]= B. Calculate the change in pH of the solution, ΔpH, if 0.371 g NaOH is added to the buffer for a final volume of 1.55 L. Assume that any contribution of NaOH to the volume is negligible. ΔpH=
a) A solution consists of 0.15 M NH4Br and 0.18 M NH3. Calculate the pH of 1.00 L of the solution AFTER the addition of 150 mL of 0.080 M HNO3. The pKa of NH4+ is 9.26. b) By how much did the pH of the solution change after the addition of the HNO3?
Calculate the pH of each of the following solutions a. 0.10 M propanoic acid, CH3CH2COOH, Ka = 1.3 x 10-5 b. 0.10 M sodium propanoate, NaCH3CH2COO. c. A mixture containing 0.10 M propanoic acid and 0.10 M sodium propanoate d. Calculate the pH after 0.020 mole of HCl is added to 1.00 L of a solution that contains 0.10 M propanoic acid and 0.10 M sodium propanoate e. Calculate the pH after 0.020 mole of NaOH is added to 1.00 L of a solution that contains 0.10 M propanoic acid and 0.10 M sodium propanoate
Which acid would be best to use when preparing a buffer with a pH of 4.76? A list of Ka values can be found in this table. Ohypoiodous acid O hydrazoic acid Ochloroacetic acid O formic acid
Draw the step-by-step procedure of linear form (Fischer Projection) of α- D Glucose and β- D Glucose to Haworth.
What mass of NaOH would be added to a one liter 0.200 M solution of acetic acid (pKa = 4.76) to adjust the final pH to 4.76? Assume the NaOH won't significantly change the volume. NaOH has a molar mass of 40.0 g.
A buffer is prepared from acetic acid and acetate ions, so that [CH3COOH] = [CH3COO-]. Ka of acetic acid equals 1.8 x 10-5. What is the pH of the buffer? A. More information is needed to answer this question. B. 7.00 C. 4.74 D. 1.8 x 10-
The acid HX has a pKa of 5.76. What volume, in mL, of a 0.100 M solution of sodium hydroxide needs to be added to 25.00 mL of a 0.100 M solution of the acid solution to make a buffer with a pH of 5.44?
Which is true about buffer solutions? -they hold the pH close to the pKa -they contain comparable moles of a weak acid and a strong base - they hold pH constant at pH=7 -they prevent acids and bases from reaching equilibrium -they hold the pH close to the equivalence point pH
O ACIDS AND BASES 451 Calculating the pH of a weak base titrated with a strong acid An analytical chemist is titrating 177.2 ml. of a 0.6100M solution of piperidine (C,H1,NH) with a 0.09700M solution of HIO, The pKy of piperidine is 2.09. Calculate the pH of the base solution after the chemist has added 1317.5 ml of the HIO, solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HIO, solution added. Round your answer to 2 decimal places. -0- ? pH- II
Which weak acid would be best to use when preparing a buffer solution with a pH of 8.50? an acid with K₁ = 2.0 × 10-10 an acid with Ka = 4.0 x 10-5 an acid with Ka 3.3 x 10-⁹ an acid with Ka an acid with Ka an acid with Ka = 0.00050 6.3 x 10-6 5.0 x 10-7

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5. Prepare a buffer with a pH of 5.3 by selecting the correct weak acid and its conjugate base: a. H2SO3/HSO3 pKa =1.77 b. HNO2/NO2 pKa = 3.34 C. NH3 /N3 pKa = 4.72 d. HCIO/CIO pKa = 7.54 e. HIO/IO pka 10.64