2) a.Calculate the pH of a 100.0 mL buffer made by combining 0.24 M acetic acid (CH3COOH,K₂ = 1.8x10¹) and 0.15 M cesium acetate (CsCH₂COO).b. Calculate the pH of the above solution after 3.59 mL of 1.0 M CSOH is added. Include abalanced chemical equation and change table (or equivalent work) below.

Answered: Image /qna-images/answer/1e89a71e-31ef-4312-a7b2-2ccbead4108e.jpg

2) a. Calculate the pH of a 100.0 mL buffer made by combining 0.24 M acetic acid (CH₂COOH, K₂= 1.8x10-5) and 0.15 M cesium acetate (CsCH3COO). b. Calculate the pH of the above solution after 3.59 mL of 1.0 M CSOH is added. Include a balanced chemical equation and change table (or equivalent work) below.

2) a. Calculate the pH of a 100.0 mL buffer made by combining 0.24 M acetic acid (CH₂COOH, K₂= 1.8x10-5) and 0.15 M cesium acetate (CsCH3COO). b. Calculate the pH of the above solution after 3.59 mL of 1.0 M CSOH is added. Include a balanced chemical equation and change table (or equivalent work) below.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter15: Additional Aqueous Equilibria

Section: Chapter Questions

Problem 90QRT: Which of these buffers involving a weak acid HA has the greater resistance to change in pH? Explain...

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Which of these buffers involving a weak acid HA has the greater resistance to change in pH? Explain your answer. (i) [HA] =0.100 M = [A] (ii) [HA] = 0.300 M = [A]
Can someone please explain why and how the step 1 was done? What was its purpose? Why was only the pKa2 value was used in the second step 2? I don't understand shortcuts and I would appreciate it if it's explained step by step. This was the solution to my previous question in which I asked: What is the pH of a buffer prepared by mixing 100 mL 0.050 mM NaH2PO4 and 25 mL 0.075 mM Na2HPO4? (pKa1=2.2; pKa2= 7.21; pKa3=12.7)
At 25oC, a 1-L buffer solution is prepared by mixing acetic acid and sodium acetate.A) If the solution is to be buffered at pH = 5, what should be the molar ratio of sodium acetate to acetic acid?B) If the buffer is found to be 1.50M in acetic acid and 1.75M in sodium acetate, what will be the pH of the solution?C) If 0.05 mol of NaOH was added to the solution in B, what will be the pH of the solution?D) If the pH of the solution in B is 4.55, how many moles of HCl was added to the solution?
You are tasked with making a buffer solution containing equal amounts of propionic acid from a 99.5 wt% solution (d = 0.993 g/mL, FW = 74.08 g/mol) and sodium propionate (solid, FW = 96.06 g/mol). What concentration of the buffer must be prepared to prevent a change in the pH by more than 0.5 pH units after the addition of 10.00 mL of 3.00 M HCl to 100.0 mL of the buffer solution? The Ka for propionic acid is 1.76 x 10-5.
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Consider a buffer made by adding 32.7 g of (CH₃)₂NH₂I to 250.0 mL of 1.42 M (CH₃)₂NH (Kb = 5.4 x 10⁻⁴) a) What is the pH of this buffer? b) What is the pH of buffer after 0.300 mol of H+ have been added? c) What is the pH of buffer after 0.120 mol of OH- have been added?
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