Concept explainers
(a)
Interpretation:
The equation for the equilibria is to be predicted. The
Concept introduction:
Dissociation constant
Where,
•
•
Answer to Problem 3.19P
The equation for the equilibria is
Explanation of Solution
The relation between
Where,
•
•
The base and acid is given as
The corresponding reaction is shown below.
The equation (1) for the reaction is written as shown below.
Where,
•
•
The
Substitute the value of
Therefore, the equilibrium constant for the reaction is
The equation for the equilibria is
(b)
Interpretation:
The equation for the equilibria is to be predicted. The
Concept introduction:
Dissociation constant
Where,
•
•
Answer to Problem 3.19P
The equation for the equilibria is
The equilibrium constant for the reaction is
Explanation of Solution
The relation between
Where,
•
•
The acid and base is given as
The corresponding reaction is shown below.
The equation (1) for the reaction is written as shown below.
Where,
•
•
The
Substitute the value of
Therefore, the equilibrium constant for the reaction is
The reaction in part (a) has the larger value of
The equation for the equilibria is
The reaction in part (a) has the larger value of
Want to see more full solutions like this?
Chapter 3 Solutions
Loose-leaf Version For Organic Chemistry
- Acid-Base Equilibria Many factors contribute to the acidity of organic compounds. Electronegativity, resonance, induction, hybridization, aromaticity, and atomic size, all play a role. In the following comparisons, you are asked to identify the factor(s) that would be most important to analyze when predicting relative acidity, and then to predict the trend in acidity and pKa values. For each of the following pairs of compounds answer the following two multiple-choice questions. 1. What factor(s) are the most important to consider when predicting the relative acidity of the two compounds? a. Electronegativity of the atom possessing the hydrogen. b. Resonance stabilization of the anionic conjugate base. c. Inductive stabilization of the anionic conjugate base. d. Hybridization of the atom possessing the hydrogen. e. The atomic size of the atom possessing the hydrogen.arrow_forwardWrite the equilibrium-constant expressions and obtain numerical values for each constant in(a) The basic dissociation of aniline, C6H5NH2.(b) The acidic dissociation of methyl ammonium hydrochloride, CH3NH3Cl.(c) The dissociation of H3AsO3 to H3O+ and AsO3^3-.arrow_forwardIf the acetate to acetic acid ratio of a solution is five, what is its pH? The pKa of acetic acid is 4.75.arrow_forward
- Estimate the Keq for the acid/base equilibria below using pKa Values. (Not provided so I have been looking in my text book and online and not getting anywhere..)arrow_forwardCalculate the pH for a mixture of one mole of benzoic acid and one mole of sodium benzoate. The pKa of benzoic acid is 4.2. 0 2 8 8 2 8 2 5 6arrow_forwardUsing pKa Values to Determine Relative Acidity and Basicity Rank the following compounds in order of increasing acidity, and then rank their conjugate bases in order of increasing basicity.arrow_forward
- Chemical Equilibrium Write the equilibrium-constant expressions and obtain numerical values for each constant in (a) the basic dissociation of aniline, C6H5NH2. (b) the acidic dissociation of hypochlorous acid, HClO. (c) the acidic dissociation of methyl ammonium hydrochloride, CH3NH3Cl. (d) the basic dissociation of NaNO2. (e) the dissociation of H3AsO3 to H3O+ and AsO33- Using step-by-step processarrow_forwardWhat is the acid dissociation constant Ka for its conjugate acid? If the base dissociation constant Kb for hypochlorite ion is 3.3x10-7arrow_forwardConsider the acid HXOy where X is a halogen that is less electronegative than oxygen. Which of the following gives the relationship between Ka of the acid and the value of y and gives the correct reasoning? As y increases the value of Ka increases because the conjugate base of the acid becomes less stable. As y increases the value of Ka increases because the conjugate base of the acid becomes more stable. As y increases the value of Ka decreases because the conjugate base of the acid becomes less stable. As y increases the value of Ka decreases because the conjugate base of the acid becomes more stable.arrow_forward
- Part 1. Choose the stronger acid in each pair of compounds. Part 2. Arrange the following compounds in order of increasing basicity. Part 3. Determine if the oxide is acidic or basearrow_forwardExplain why-(i) Anhydrous calcium chloride is used in desiccators(ii) If bottle full of concentrated H 2SO4 is left open in the atmosphere by accident, the acid starts flowing out the bottle of its own.arrow_forwardIdentify the base and conjugate acid in each of the equilibria and predict which side is favored.arrow_forward
- Principles of Modern ChemistryChemistryISBN:9781305079113Author:David W. Oxtoby, H. Pat Gillis, Laurie J. ButlerPublisher:Cengage LearningOrganic ChemistryChemistryISBN:9781305580350Author:William H. Brown, Brent L. Iverson, Eric Anslyn, Christopher S. FootePublisher:Cengage Learning