b) We have assumed [CO;²] << [HCO;] in our precedent calculation and accordingly ignored the [CO;²] contribution. Explain why it is a good assumption to make for most natural waters. Note: the common pH range in natural waters is 5.5 to 8.5. (Hint: either use the second acid dissociation constant expression, or a quick sketch of the carbonate system Bierrum plot to demonstrate vour point)

b) We have assumed [CO;²] << [HCO;] in our precedent calculation and accordingly ignored the [CO;²] contribution. Explain why it is a good assumption to make for most natural waters. Note: the common pH range in natural waters is 5.5 to 8.5. (Hint: either use the second acid dissociation constant expression, or a quick sketch of the carbonate system Bierrum plot to demonstrate vour point)

Organic Chemistry

8th Edition

ISBN:9781305580350

Author:William H. Brown, Brent L. Iverson, Eric Anslyn, Christopher S. Foote

Publisher:William H. Brown, Brent L. Iverson, Eric Anslyn, Christopher S. Foote

Chapter4: Acids And Bases

Section: Chapter Questions

Problem 4.35AP: The sec-butyl cation can react as both a Brnsted-Lowry acid (a proton donor) and a Lewis acid (an...

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The sec-butyl cation can react as both a Brnsted-Lowry acid (a proton donor) and a Lewis acid (an electron pair acceptor) in the presence of a watersulfuric acid mixture. In each case, however, the product is different. The two reactions are as follows: (a) In which reaction(s) does this cation react as a Lewis acid? In which reaction(s) does it react as a Brnsted-Lowry acid? (b) Write Lewis structures for reactants and products and show by the use of curved arrows how each reaction occurs.
Give detailed Solution with explanation needed...don't give Handwritten answer
m/alekscgi/x/Isl.exe/10_u-IgNslkr7j8P3jH-IQUHIQg6bJxmeSyVpHOEB1plef9xyC5Ca9Q13FtjF-pE0ofvdFNRgOhdfPxWKytqn8 ||| O ACIDS AND BASES Interconverting pH and hydronium ion concentration Each row of the table below describes an aqueous solution at about 25 °C. Complete the table. That is, fill in any missing entries in the second and third columns. Round your entries for for pH to 2 decimal places. solution A B C [H₂O*] 6.3 × 10 -8 mol/L mol/L 0.0069 mol/L PH 8 9.13 X [H₂O*] to JMXRyqqz8W0qjsQSpv/Aqw 0/5 to 2 significant digits, and your entries
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