Buffer B and Buffer C both contain 1.000 M HC,H3O2, yet adding 5.00 mL of 0.5000 M NaOH to 20.00 mL of Buffer B (same amounts as in Question 7) would cause Buffer B to have a ApH = 0.29. Select all of the possible .explanations for why Buffer C is a better buffer against a base, even though the two buffers contain the same amount of buffering conjugate acid. Having equal amounts of the two buffering conjugates (like in Buffer C) results in the largest buffering capacity in both directions Buffer C has more conjugate base, which minimizes the forward shift in the equilibrium reaction due to the common ion effect OIn Buffer C, the pH is closer to the pKa Don't pick this answer ;) In Buffer C the ratio of conjugate base to conjugate acid is closer to 1

Buffer B and Buffer C both contain 1.000 M HC,H3O2, yet adding 5.00 mL of 0.5000 M NaOH to 20.00 mL of Buffer B (same amounts as in Question 7) would cause Buffer B to have a ApH = 0.29. Select all of the possible .explanations for why Buffer C is a better buffer against a base, even though the two buffers contain the same amount of buffering conjugate acid. Having equal amounts of the two buffering conjugates (like in Buffer C) results in the largest buffering capacity in both directions Buffer C has more conjugate base, which minimizes the forward shift in the equilibrium reaction due to the common ion effect OIn Buffer C, the pH is closer to the pKa Don't pick this answer ;) In Buffer C the ratio of conjugate base to conjugate acid is closer to 1

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

The Ka of lactic acid is 1.38 x 10^-4
For each of the buffer systems below, determine the concentration of the acid and base components in the buffer: 1) An acetate buffer with a pH of 5.15 and a concentration of 3.5M. The (HC2H302] = Type your answer here M and the [NAC2H302] = Type your answer here M 2) A Carbonate buffer with a pH of 9.85 and a concentration of 0.50M. The [NAHCO3] = Type your answer here M and the Na2CO3] = Type your answer here M 3) A Phosphate buffer of pH 2.5 and a concentration of 1.0M. The [H3PO4] = Type your answer here Mand the [KH2PO4) Type your answer here
Determine the mass of solid NaCH,COO that must be dissolved in an existing 500.0 mL solution of 0.200 M CH;COOH to form a buffer with a pH equal to 5.00. The value of Ka for CH,COOH is 1.8 x 10. NEXT > Let x represent the original concentration of CH;COO in the water. Based on the given values, set up the ICE table in order to determine the unknown. CH;COOH(aq) + H2O(1) H,O (aq) CH;COO (aq) Initial (M) Change (M) Equilibrium (M)
What ratio of CH₃NH₂ to CH₃NH₃⁺ is needed to prepare a pH 10.10 buffer? (Kb for CH₃NH₂ is 4.4 × 10⁻⁴)
Question 4 a) Determine the pH of 0.10 M NAOH solution. b) Find out the pH of a 0.002 M acetic acid solution if it is 2.3% ionised at this dilution. c) A chemistry student desires to prepare one litre of a solution buffered at pH 9.00. How many grams of ammonium chloride haye to be added to one litre of 0.20 M NH3 to makesuch a buffer. pKb value of ammonia is 4.75 in the equation. NH3 + H20 = NH + OH
We have 500.0 mL of a buffer solution that is 0.697 M in NH3 and 0.380 M in NH4Cl. We add 500.0 mL of a solution 0.202 M in HCl. The final volume is 1.0000 L. The Kb value for NH3 is 1.8 x 10-5. What is the pH of the final solution?
P Please don't provide the handwriting solution
1. all the aqueous solutions that are good buffer systems 2. a buffer solution is 0.421 m in hcn and 0.281 m in kcn, if Ka for Hcn is 4.0 * 10^-10. what is the PH of this buffer solution. b. a buffer solution is 0.495 m in h2s and 0.354 m in khs, if Ka1 for H2s is 1.0 * 10^-7. what is the PH of this buffer solution. c. a buffer solution is 0.455 m in NaHSO and 0.299 m in Na2SO3, if Ka for HSO3 is 6.4 * 10^-8. what is the PH of this buffer solution. 3. A 28.9 ml sample of a 0.385 m aqueous hydrocyanic acid solution is titrated with a 0.372 m aqueous sodium hydroxide solution. what is the ph at the start of the titration, before any sodium hydroxide has been added. b. A 31.9 ml sample of a 0.599 m aqueous hydrofluoric acid solution is titrated with a 0.242 m aqueous barium hydroxide solution. what is the ph after 15.8ml of base has been added. c. when a 23.8 ml sample of a 0.357 m aqueous acetic acid solution is titrated with a 0.459 m aqueous barium hydroxide solution. what is the ph…
esti alist titrates 20.0 ml of 0.20 M HBIO with 0.10 M NaOH. Galculate the pH: 1. Before the titration. 2. When the concentration of HBro equal to the concentration of Bro. 3. When number of moles of HBrO are equal to number of moles of bane added Given an acid dissociation constant, K of HBrO=23 x 10.
We have 500.0 mL of a buffer solution that is 0.661 M in NH3 and 0.304 M in NH4Cl. We add 500.0 mL of a solution 0.245 M in HCl. The final volume is 1.0000 L. The Kb value for NH3 is 1.8 x 10-5. What is the pH of the final solution?
100. mL of 0.200 M HC1 is titrated with 0.250 M NaOH.
What is [OH – ] in a solution of 0.125 M CH 3 NH 2 and 0.130 M CH 3 NH 3 Cl? I do not understand how to solve for Kb. Can you please explain this problem step by step?