You are asked to make a buffer of pH 3.4 and given the above acids. Of these acids, which would create a buffer with the best capacity against acids? Which would have the best buffering capacity against bases? Which could not be used at all for this project? Best against acids Best against bases Acid #1 has a pka of 3.15 Acid #2 has a pKa of 3.65 Acid #3 has a pKa of 4.23 Acid #4 has a pKa of 4.79 Cannot be used Acid #2 Acid #1 Acid #4

You are asked to make a buffer of pH 3.4 and given the above acids. Of these acids, which would create a buffer with the best capacity against acids? Which would have the best buffering capacity against bases? Which could not be used at all for this project? Best against acids Best against bases Acid #1 has a pka of 3.15 Acid #2 has a pKa of 3.65 Acid #3 has a pKa of 4.23 Acid #4 has a pKa of 4.79 Cannot be used Acid #2 Acid #1 Acid #4

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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Choose the compound (or compounds) that best match the descriptions. 1. NaCIO, Superacid 2. H2SO4 and H3PO4 Lewis acid, not a Bronsted- 3. BeF2 Lowry acid 4. CH3NH3CI Makes a buffer with HCIO, 5. CIO4 Makes a buffer with CH3NH3Br 6. CH3NH2 Lewis base, not a Bronsted- Lowry base 7. HCIO4 8. B(OH)3 and HCIO4
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Again consider the same buffer solution from the previous question, where [H2CO3] = [HCO3–] = 0.100 M. What will be the pH after 0.005 mol of NaOH has been added to 1.00 L of this solution? (Ka1 for H2CO3 = 4.2 x 10–7) Group of answer choices
What is the pH at which a buffer composed of NH3 and NH4+ would be most effective at resisting pH change? Round your answer to 2 decimal places. Remember you can find KA and/or KB values
You are in charge of making a Tris buffer at pH 7.5. You could start with solid Tris base as you did in lab, but you found stock solutions of 1.0M Tris base and 1.0M Tris Hydrochloride (the conjugate acid form) in the lab and decided to make the buffer with those. How much of each of the stock solutions would you mix together to make 200.0 mL of 1.0M Tris buffer at pH 7.5?
Moving to another question will save this response. Question 10 A esc A Moving to another question will save this response. P buffer is frequently used in biochemical experiments 0 F1 Q 2 0: F2 W 20 #3 F3 E 000 000 $ 4 F4 1: % R 5
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Biology Match each weak acid with the pH value at which it would buffer. You are currently in a sorting module. Turn off browse mode or quick nav, Tab to items, Space or Enter to pick up, Tab to move, Space or Enter to drop. pH 33 pH 55 pH 99 Answer Bank hydrazoic acid (pKapKa of 4.64.6) formic acid (pKapKa of 3.83.8) acetic acid (pKapKa of 4.764.76) boric acid (pKapKa of 9.249.24) chloroacetic acid (pKapka of 2.872.87) ammonium (pKapKa of 9.259.25)
Which of the following acid/base pairs would not make a good buffer system? H2PO4-/ HPO42- HSO3-/Na2SO3 H2CO3/H2CO2- NH4+/NH3 HNO2/NO2-
Design a buffer that has a pH of 10.20 using one of the weak base/conjugate acid systems shown below. Weak Base Kb Conjugate Acid Ka pKa CH3NH2 4.2×10-4 CH3NH3+ 2.4×10-11 10.62 C6H15O3N 5.9×10-7 C6H15O3NH+ 1.7×10-8 7.77 C5H5N 1.5×10-9 C5H5NH+ 6.7×10-6 5.17 How many grams of the chloride salt of the conjugate acid must be combined with how many grams of the weak base, to produce 1.00 L of a buffer that is 1.00 M in the weak base? grams chloride salt of conjugate acid = grams weak base =
Ka reaction: C₂H₂N₂H+ + H₂O=C3H₂N₂ + H₂0+ Calculate the pH of a solution prepared by mixing 1.90 g of imidazole with 1.90 g of imidazole hydrochloride and diluting to 100.0 mL. The pKa of imidazole hydrochloride is 6.993. pH = Calculate the pH of the solution if 2.40 mL of 1.07 M HClO are added. 4 pH = 7.18 volume: 7.08 How many milliliters of 1.07 M HClO4 should be added to 1.90 g of imidazole to give a pH of 6.993? mL