TXT 9.2 Rank the labeled H's in the following molecules in order of increasing acidity (1 = least acidic, 5 = most acidic). Provide a brief explanation for your ordering. 2. HO a e HO ОН Br H ci H 3. Rank the following primary amines (anilines in this case) in order of increasing ТXT 9.6 basicity (1 = least basic, 4 = most basic). Write the conjugate acid and provide a brief explanation for your ordering. %3D NH2 NH2 NH2 NH2 OCH3 NO2 CH3 А В C 0=

TXT 9.2 Rank the labeled H's in the following molecules in order of increasing acidity (1 = least acidic, 5 = most acidic). Provide a brief explanation for your ordering. 2. HO a e HO ОН Br H ci H 3. Rank the following primary amines (anilines in this case) in order of increasing ТXT 9.6 basicity (1 = least basic, 4 = most basic). Write the conjugate acid and provide a brief explanation for your ordering. %3D NH2 NH2 NH2 NH2 OCH3 NO2 CH3 А В C 0=

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 9E

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Answer questions a-c about the Bronsted acid-base reaction below using the identifying letters A-D below each structure. The pKa's for the acids of interest are: phenol (pKa = 9.9), and acetic acid (pKa = 4.8). 1.) - The stronger acid is - Its conjugate base is - The species that predominate at equilibrium are 2.) - The stronger base is - Its conjugate acid is - The species that predominate at equilibrium are
NH4+ + HAsO4- ⇆ H2AsO4 + NH3What is the Bronsted base in the reaction above? a. NH 4 + b. HAsO 4 - c. H2AsO4 d. more than one response is correct
The Ka of acetic acid (CH3CO2H) is 1.8x10-5 and the Kb of methylamine (CH3NH2) is 4.4x10-4. Complete the following equilibrium reaction (acid-base reaction) equation and predict the side of the equilibrium that is favored. Explain. Show all your work.
Given that Kb for dimethylamine, (CH3)2NH, is 5.90 x 10-4 and the Kb for methylamine, CH3NH2, is 4.40 x 10-4, a. which one is the stronger base? b. Calculate the Ka for CH3NH3+. c. Calculate the Ka for (CH3)2NH2+.
For each pair of compounds: [1] Which indicated H is more acidic? [2] Draw the conjugate base of each acid. [3] Which conjugate base is stronger?
What am I doing wrong? I think the proton on the amine is more acidic and the conjugate acid seems to be more acidic than the acid which doesn't make sense for the Keq value.
can you explain in detail how to do the first 3 problems? How would I know if the acid base pairs would react with each other?
Which of the following protons will be the most deshielded - Ha, Hb, or Hc? Explain your answer
3. Rank the following acids in order from strongest to weakest.HA (pKa = 2.55) H2Z (pKa1 = 4.35) H3X (pKa1 = 3.17) HY (pKa = 5.72) 4. Rank each base in order from strongest to weakest.B (pKb = 4.12) Y– (pKa = 5.72 for conjugate acid) A– (pKa = 2.55 for conjugate acid)E (pKb = 8.12)
In each pair of compounds below decide which one is more acidic.
Could you explain how to find the answer? Will leave good rating! Thank you!
Arrange the compounds in each set in order of increasing base strength. consult Table 4.1 for pKa values of the conjugate acid of each base.