Interpretation:
The validation corresponding to the fact that
Concept introduction:
The
This scale is defined from
Answer to Problem 20.35AP
The value of
Explanation of Solution
The given
So, the value of
The ionization table for acetic acid for initial and final concentration is given below.
The expression to calculate the value of
Substitute the values of respective concentrations and
The value of
Substitute the value of
Therefore, the value of
The given
So, the value of
The ionization table for phenol for initial and final concentration is given below.
The expression to calculate the value of
Substitute the values of respective concentrations and
Substitute the value of
Therefore, the value of
The
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Chapter 20 Solutions
EBK ORGANIC CHEMISTRY
- Find the value of Kb for the conjugate base of the following organic acids. (a) picric acid used in the manufacture of explosives; Ka = 0.16 (b) trichloroacetic acid used in the treatment of warts; Ka = 0.20arrow_forwardFor each equation, label the Lewis acid and the Lewis base. In addition, show all unshared pairs of electrons on the reacting atoms and use curved arrows to show the flow of electrons in each reaction. (a) F + BF3 BF4arrow_forwardFor the following reaction, K> 1. Classify each of the reactants and products based on their strength as Bronsted-Lowry acids or bases. CH3COOH + C18H2103NC18H2103NH+ + CH3COO- C18H2103NH+ CH3COO C18H2103N CH3COOH 1) Stronger Bronsted-Lowry acid 2) Weaker Bronsted-Lowry acid 3) Stronger Bronsted-Lowry base 4) Weaker Bronsted-Lowry basearrow_forward
- in e 10 C N g For the following reaction, draw the Lewis Dot structure for each reactant and product including any formal charges. Also identify the Lewis Acid and the Lewis Base for this reaction. CH3CH2CCH+ NH2 -> CH3CH₂CC + NH3 On the product side of the equation, one of the C atoms has 1 unshared pair of electrons and is (-) charged.arrow_forwardRank the acids below in order of decreasing acidity. HO SH HN SH H,N db (Choose one) (Choose one) (Choose one) (Choose one)arrow_forwardCalculate the pH of an acetic acid solution, originally 0.25 M, in water. The pKa for acetic acid = 4.76.arrow_forward
- 2,4-Pentanedione is a considerably stronger acid than is acetone (Chapter 19). Write a structural formula for the conjugate base of each acid and account for the greater stability of the conjugate base from 2,4-pentanedione.arrow_forwardWhich is the conjugate base in this reaction? acetic acid Pyridine Pyridinium H ion Lot -oH pka =4.76 pKa= 5,25 A acetic acid B) acetate ion pyridine D pyridinium ionarrow_forward1) When starting with completely un-dissociated acetic acid, is it accurate to assume that [HOAc]0 = [HOAc]eq? Why or why not? 2) A highly concentrated acetic acid solution contains 15.0 M acetic acid at equilibrium. What are the equilibrium concentrations of the hydronium and acetate ions in this solution?arrow_forward
- Identify the acid and base in each reaction. Additionally, predict the product of the reaction. 1. Arrhenius reaction between KOH and HCIO2 2. Bronsted-Lowry acid-base reaction between HCIO4 and Br 3. Lewis reaction between Ag* and 2 cyanide ions (CN')arrow_forwardWhat is the percent dissociation of acetic acid if the solution has a pH = 4.74 and a pK a = 4.74? What is the percent dissociation of acetic acid if the solution has a pH = 4.74 and a pK a = 4.74? 100% 10% 1% 50%arrow_forwardGive the major product of the following reaction. HBr Ph-C C-Ph НООН There is no reaction under these conditions or the correct product is not listed here. Br Ph Ph Br Br Ph Ph Br Br Ph Ph Br Br Ph Ph Br Br J Ph Ph Br Br Ph Ph Brarrow_forward
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