Buffer solutions resist dramatic changes in pH due to the presence of a weak acid-conjugate base pair present in the solution. However, the combination of 20.0mL of 0.30M HC2H3O2 and 10.0mL of 0.30M NaOH also produces an excellent buffer solution. How? Provide a thorough explanation that explains the apparent discrepancy. (Using calculations and reactions to support your explanation is encouraged. Feel free to use another page if additional space in needed.) The Ka of HC2H3O2 is 1.8x 10-5.

Buffer solutions resist dramatic changes in pH due to the presence of a weak acid-conjugate base pair present in the solution. However, the combination of 20.0mL of 0.30M HC2H3O2 and 10.0mL of 0.30M NaOH also produces an excellent buffer solution. How? Provide a thorough explanation that explains the apparent discrepancy. (Using calculations and reactions to support your explanation is encouraged. Feel free to use another page if additional space in needed.) The Ka of HC2H3O2 is 1.8x 10-5.

Organic Chemistry: A Guided Inquiry

2nd Edition

ISBN:9780618974122

Author:Andrei Straumanis

Publisher:Andrei Straumanis

Chapter20: Acidity And Pka Of Phenols

Section: Chapter Questions

Problem 3CTQ

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The maximum buffering capacity is nearest to the pKa of the buffer. Explain why?
Please answer it ALL ASAP and CORRECTLY for an upvote. PROVIDE YOUR FULL SOLUTION. You prepared a buffer solution by mixing 68 ml of 0.17 M ammonia and 42 ml of 0.13 M ammonium chloride. The dissociation constant of ammonia is 1.8x10^-5 What is the total volume of the buffer? What is the final concentration of the base? What is the final concentration of the salt? What is the acid strength of the solution? What is the pH of the buffer solution?
Provide the chemical formulas and the names of the three predominant carbonic acid species indicated by arrows in the image below: Species 1 species 2 Species 3 Explain i) how you can determine the pH range at which a weak acid/conjugate base system will display buffering properties.ii) what is the reason/logic behind the rule applied in i)? and iii) indicate the pH ranges of the carbonic acid system based on the pka values provided above. Provide the chemical equilibrium that describes the carbonic acid buffer system that exists at pH 9.3. Clearly indicate the chemical formulas, identify the weak acid and it’s conjugate base, and the names of the chemical compounds.
The following text may be found at the ThermoFisher website: "PBS (phosphate buffered saline) is a pH-adjusted blend of ultrapure-grade phosphate buffers and saline solutions which, when diluted to a 1X working concentration, contains 137 mM NaCl, 2.7 mM KCl, 8 mM Na2HPO4, and 2 mM KH2PO4. Each 10X PBS solution is ready to use upon dilution to the desired concentration." This means that the product that you purchase has a concentration 10 times the concentration at which it is used. 1. Look up the pKa values for phosphoric acid and list them as a part of your response. 2. Based on the description of the contents of the PBS buffer, calculate the pH of the 1X solution. 3. Assume that you wish to use a pH = 7.00 buffer. If your answer to 2 was more acidic than pH 7.00, calculate how much 1.00 M NaOH you would need to add to get to pH = 7.00. If your answer to 2 was more basic than pH 7.00, calculate how much 1.00 M HCl you would need to add to get to pH = 7.00.
Your research advisor asks you to prepare a buffer solution at pH = 3.50 with capacity of about 0.100 M. Given the following solutions available (of any concentration), determine which species would give the best buffer, and give possible concentrations of the conjugate species. Dimethylamine pKb = 3.27; ethlyamine pKb = 3.35; aniline pKb =9.13; sodium nitrite pKb = 10.60.
Hello, can someone please help me with these chem questions and give me a clear step-by-step solution. Thank you very much for your help. (there is also a chart that is included in the question) Question: Determine the [H3O+] of the eight buffer solutions made by mixing 1.10 M acetic acid and 0.900 M sodium acetate solutions according to the following volumes. The pKa for acetic acid, CH3CO2H (HAc), is 4.745. You will also need this information in your post-lab. It is highly suggested you write these calculations down (both unrounded and rounded values) to use later. To enter exponential values, use the format 1.0e-5:
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)
Which is the correct order of steps in the preparation of a hydrochoric acid standard solution with sodium bicarbonate standard solution. I. Dissolved sodium carbonate (13.25 g) in about 150 mL of distilled water in a beaker II. Solution of sodium carbonate was transferred into a volumetric flask and diluted to mark before mixing. III. Weigh the appropriate amount of the primary standard. IV. Titrate with enough volume of the acid to completely neutralize the base. V. Transfer 10.00 ml primary standard into an erlenmeyer flask and add indicator III, I, II, V, IV III, II, I, V, IV V, III, I, II, IV V, IV, III, I, II
a). What are acids, bases and buffers?b) What are the different types of buffers? Describe the mechanism howbuffers resist pH change in a system.c) Elaborate all chemical reactions in the standardization of NaOH withKHP?d) Why do you need to use KHP in the standardization of NaOH?e) Why is phenolphthalein used as an indicator in this experiment?f) Compare and contrast: endpoint vs equivalence point.g) Discuss the role of acids, bases, buffers and pH in water qualitymonitoring and post-harvest fisheries.
H8. Describe the difference between a buffered and an unbuffered solution. Explain the significance of a buffer solution in a real-life application. Provide a unique example in your discussion
By reference to the reacting ratio of HCL and NaOH, deduce the number of moles of NaOH required to reach Equivalence. Btw I did the first part of the question so this is a follow up.
Is it possible, upon precipitation of the third class ions, to add H2S first, then NH4OH and NH4Cl? And why