Organic Chemistry
6th Edition
ISBN: 9781936221349
Author: Marc Loudon, Jim Parise
Publisher: W. H. Freeman
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Chapter 3, Problem 3.13P
Interpretation Introduction
(a)
Interpretation:
The value of
Concept introduction:
Dissociation constant
The formula used to calculate the value of
Interpretation Introduction
(b)
Interpretation:
The value of
Concept introduction:
Dissociation constant
The formula used to calculate the value of
Interpretation Introduction
(c)
Interpretation:
The value of
Concept introduction:
Dissociation constant
The formula used to calculate the value of
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Students have asked these similar questions
Write the formula for the K eq for the following reaction:
N 2(g) +3H 2(g) ->2NH3(g)
What is the correct equilibrium constant expression for the following reaction?
NH3(aq) + H₂O(1) ⇒NH4*(aq) + OH¯(aq)
O
O
(A) Ke
(B) Kc
(c) Ke
(D) Kc
(E) Kc
-
=
=
=
[NH3] [H₂O]
[NH4]+[OH]-
[NH4+][OH-]
[NH3]
[NH4+] [OH
[NH3] [H₂O]
[NH3]
[NH₂+] [OH-]
4
[NH₁+OH
[NH3]
COHSOH(ag) + H2On + CeHsO (aq) + H3O*(a9)
Ka= 1.12 x 10-10
(a) Phenol is a weak acid that partially dissociates in water according to the equation above.
Write the equilibrium-constant expression for the dissociation of the acid in water.
(b) What is the pH of a 0.75 M CaHsOH(ag) solution?
(C) For a certain reaction involving CaHsOH(ag) to proceed at a significant rate, the phenol must be
primarily in its deprotonated form, C3H5O (eg). In order to ensure that the CsHsOH(aq) is deprotonated,
the reaction must be conducted in a buffered solution. On the number scale below, circle each pH for
which more than 50 percent of the phenol molecules are in the deprotonated form (CoHsO (aq).
Justify your answer.
1 2 3 4 5 6 7 8 9 10 11 12 13 14
Justification:
(d) CeHsOH(ag) reacts with NaOH(ag). Write a net ionic equation representing this reaction (aka:
invasion equation).
(e) What is the pH of the resulting solution when 30 mL of 0.40 M CSH5OH(aq) is added to 25 mL of
0.60 M NAOH. Show all work…
Chapter 3 Solutions
Organic Chemistry
Ch. 3 - Prob. 3.1PCh. 3 - Prob. 3.2PCh. 3 - Prob. 3.3PCh. 3 - Prob. 3.4PCh. 3 - Prob. 3.5PCh. 3 - Prob. 3.6PCh. 3 - Prob. 3.7PCh. 3 - Prob. 3.8PCh. 3 - Prob. 3.9PCh. 3 - Prob. 3.10P
Ch. 3 - Prob. 3.11PCh. 3 - Prob. 3.12PCh. 3 - Prob. 3.13PCh. 3 - Prob. 3.14PCh. 3 - Prob. 3.15PCh. 3 - Prob. 3.16PCh. 3 - Prob. 3.17PCh. 3 - Prob. 3.18PCh. 3 - Prob. 3.19PCh. 3 - Prob. 3.20PCh. 3 - Prob. 3.21PCh. 3 - Prob. 3.22PCh. 3 - Prob. 3.24PCh. 3 - Prob. 3.25PCh. 3 - Prob. 3.26PCh. 3 - Prob. 3.27PCh. 3 - Prob. 3.28PCh. 3 - Prob. 3.29PCh. 3 - Prob. 3.30PCh. 3 - Prob. 3.31PCh. 3 - Prob. 3.32APCh. 3 - Prob. 3.33APCh. 3 - Prob. 3.34APCh. 3 - Prob. 3.35APCh. 3 - Prob. 3.36APCh. 3 - Prob. 3.37APCh. 3 - Prob. 3.38APCh. 3 - Prob. 3.39APCh. 3 - Prob. 3.40APCh. 3 - Prob. 3.41APCh. 3 - Prob. 3.42APCh. 3 - Prob. 3.43APCh. 3 - Prob. 3.44APCh. 3 - Prob. 3.45APCh. 3 - Prob. 3.46APCh. 3 - Prob. 3.47APCh. 3 - Prob. 3.48APCh. 3 - Prob. 3.49APCh. 3 - Prob. 3.50APCh. 3 - Prob. 3.51APCh. 3 - Prob. 3.52APCh. 3 - Prob. 3.53APCh. 3 - Prob. 3.54APCh. 3 - Prob. 3.55APCh. 3 - Prob. 3.56APCh. 3 - Prob. 3.57APCh. 3 - Prob. 3.58APCh. 3 - Prob. 3.59APCh. 3 - Prob. 3.60AP
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- For conjugate acidbase pairs, how are Ka and Kb related? Consider the reaction of acetic acid in water CH3CO2H(aq)+H2O(l)CH3CO2(aq)+H3O+(aq) where Ka = 1.8 105 a. Which two bases are competing for the proton? b. Which is the stronger base? c. In light of your answer to part b. why do we classify the acetate ion (CH3CO2) as a weak base? Use an appropriate reaction to justify your answer. In general, as base strength increases, conjugate acid strength decreases. Explain why the conjugate acid of the weak base NH3 is a weak acid. To summarize, the conjugate base of a weak acid is a weak base and the conjugate acid of a weak base is a weak acid (weak gives you weak). Assuming Ka for a monoprotic strong acid is 1 106, calculate Kb for the conjugate base of this strong acid. Why do conjugate bases of strong acids have no basic properties in water? List the conjugate bases of the six common strong acids. To tie it all together, some instructors have students think of Li+, K+, Rb+, Cs+, Ca2+, Sr2+, and Ba2+ as the conjugate acids of the strong bases LiOH, KOH. RbOH, CsOH, Ca(OH)2, Sr(OH)2, and Ba(OH)2. Although not technically correct, the conjugate acid strength of these cations is similar to the conjugate base strength of the strong acids. That is, these cations have no acidic properties in water; similarly, the conjugate bases of strong acids have no basic properties (strong gives you worthless). Fill in the blanks with the correct response. The conjugate base of a weak acid is a_____base. The conjugate acid of a weak base is a_____acid. The conjugate base of a strong acid is a_____base. The conjugate acid of a strong base is a_____ acid. (Hint: Weak gives you weak and strong gives you worthless.)arrow_forward8-87 The pKavalue of barbituric acid is 5.0. If the H3O+ and barbiturate ion concentrations are each 0.0030 M, what is the concentration of the undissociated barbituric acid?arrow_forwardWhat are the products of each of the following acid-base reactions? Indicate the acid and its conjugate base and the base and its conjugate acid. (a) HCIO4 + H2O (b) NH4 ++ H2O (c) HCO3 + OHarrow_forward
- The Kb values for ammonia and methylamine are 1.8 105 and 4.4 104, respectively. Which is the stronger acid, NH4+ or CH3NH3+?arrow_forwardWhat are the products of each of the following acid-base reactions? Indicate the acid and its conjugate base and the base and its conjugate acid. HC1O4+ H2O — NH/ + H2O -» HCOr + OH" —arrow_forward8-112 Consider an initial 0.040 M hypobromous acid (HOBr) solution at a certain temperature. At equilibrium after partial dissociation, its pH is found to be 5.05. What is the acid ionization constant, Ka, for hypobromous acid at this temperature?arrow_forward
- At 25 oC, Ammonia is a weak base that reacts with water according to this equation: NH3(aq) + H2O(aq) ⇌ NH4+(aq) + OH−(aq) Briefly explain how the equilibrium will shift (to get back to equilibrium) if the following perturbations are made to the system: (a) Addition of HCl (b) Addition of NaOH (c) Addition of NH4Clarrow_forwardA major component of coral is carbonate ions, which is created by the dissociation of bicarbonate ions as follows: HCO3-(aq) ⇌ CO32-(aq) + H+(aq) How will carbonate ion concentrations potentially be affected by an increase in the acidity of the ocean? Please explain the reasoning for your response in 1-2 sentences.arrow_forwardThe Keq for the reaction: A + B ↔ AB is 2.163 What is the Keq for 2 + AB ↔ 2 A + 2 Barrow_forward
- The ionization constant (Kb) of trimethylamine ((CH3);N) is 7.40 x 105. If 5.911 grams of trimethylamine is dissolved in 50.0 mL of water, what are the equilibrium concentration of all species present?arrow_forwardThe acid-dissociation constant for hypochlorous acid (HClO) is 3.0 × 10-8. Calculatethe concentrations of H3O+, ClO- and HClO at equilibrium if the initial concentration of HClO is 0.0075 Marrow_forward(a) Given that Ka for acetic acid is 1.8 x 10-5 and that hypochlorous acid is 3.0 x10-8 , which is a stronger acid? (b) Which is the stronger base, the acetate ion or the hypochlorite ion? (c) calculate the Kb values for the CHCOO- and ClO- .arrow_forward
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