The molecular scene (see margin) shows a sample of an HB/B-buffer. (HB is blue and yellow, B- is yellow; other ions and water are not shown.)(a) Would you add a small amount of concentrated strong acid or strong base to increase the buffer capacity?(b) Assuming no volume change, draw a scene that represents the buffer with the highest possible capacity after the addition in part (a).

The molecular scene (see margin) shows a sample of an HB/B-buffer. (HB is blue and yellow, B- is yellow; other ions and water are not shown.)(a) Would you add a small amount of concentrated strong acid or strong base to increase the buffer capacity?(b) Assuming no volume change, draw a scene that represents the buffer with the highest possible capacity after the addition in part (a).

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter14: Equilibria In Acid-base Solutions

Section: Chapter Questions

Problem 12QAP: A buffer is prepared by dissolving 0.062 mol of sodium fluoride in 127 mL of 0.0399 M hydrofluoric...

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A buffer is prepared by dissolving 0.062 mol of sodium fluoride in 127 mL of 0.0399 M hydrofluoric acid. Assume no volume change after NaF is added. Calculate the pH of this buffer.
You want to prepare 1.00 L of a buffer solution with a pH of 3.5. You are given an 0.45 M solution of nitrous acid, HNO2, and an 0.68 M solution of NaOH. What volume of each of these solutions must be mixed in order to get the desired buffer solution? Use the simultaneous equations method to solve this problem. If the buffer solution prepared in a. also contained ~10-6M Ni2+ and ~10-6 M Pb2+ , could those metal ions be separated from each other by saturating the solution with H2S? Explain your answer by showing the necessary calculations.
What is the proper unit of molar ratio of weak acid and its conjugate base in a buffer solution? Is it mol to mol or part to part? Or is it unitless? I need to express the answer 1.45/1 = [A]/[HA] to the right unit. See image for more details. the buffer is acetic acid/sodium acetate buffer.
What is the effect of dilution on the pH of a buffer and the buffer’s capacity?
a. You want to prepare 1.00 L of a buffer solution with a pH of 3.5. You are given an 0.45 M solution of nitrous acid, HNO2, and an 0.68 M solution of NaOH. What volume of each of these solutions must be mixed in order to get the desired buffer solution? Use the simultaneous equations method to solve this problem. b. If the buffer solution prepared in a. also contained ~10–6M Ni2+ and ~10–6 M Pb2+ , could those metal ions be separated from each other by saturating the solution with H2S? Explain your answer by showing the necessary calculations.
What is the effect of dilution on the pH of a buffer and the buffer’s capacity? explain
a. You want to prepare 1.00 L of a buffer solution with a pH of 3.5. You are given an 0.45 M solution of nitrous acid, HNO2, and an 0.68 M solution of NaOH. What volume of each of these solutions must be mixed in order to get the desired buffer solution? Use the simultaneous equations method to solve this problem. b)If the acid used in a. was nitric acid, HNO3, could the same buffer solution be made? Briefly explain. c) If the buffer solution prepared in a. also contained ~10–6M Ni2+ and ~10–6 M Pb2+ , could those metal ions be separated from each other by saturating the solution with H2S? Explain your answer by showing the necessary calculations.
For a titration to be effective, the reaction must be rapid and the yield of the reaction must essentially be 100%. Is Kc > 1, < 1, or ≈ 1 for a titration reaction? Kc is the product of all reaction products (choose from: Multiplied by, added to, divided by, subtracted from) the product of the reactants, with all concentrations of reactants and products raised to their respective stoichiometric powers. As the titration proceeds, the amount of reactants (choose from: Increases, decreases, remains the same) and the amount of products (choose from: Increases, decreases, remains the same). Because the value of the numerator is (Choose from much greater than, much less than, approximately equal to) the value of the denominator, the value of Kc will be (Choose from much greater than, much less than, approximately equal to)1 for an effective titration reaction.
To fill a 500 mL volumetric flask, 40 g of ammonium chloride (NH4Cl) and 3.2 g of ammonia (NH3) are added along with water. Given the Kb of NH3 is 1.8 × 10−5, the pH of this buffer is...
What are buffers in terms of acid-base equilibria, give an example, and can abuffer capacity be overwhelmed?
At what point in the titration of a weak base with a strong acid is the maximum buffer capacity reached? This is the point at which a given small addition of acid causes the least pH change.
A buffer solution that is 0.473 M in HCN and 0.473 M in NaCN has a pH of 9.40. The addition of 0.01 mol of OH^- to 1.0 L of this buffer would cause the pH to _________ : increase slightly, increase by 2 units, decrease slightly, decrease by 2 units or not change. The capacity of this buffer for added H3O^+ could be increased by the addition of 0.175 mol _________of the: weak acid or of the salt.