The conjugate base of benzoic acid is used as a72preservative. Write the equilibrium reaction for thisweak acid in aqueous solution.ОНBenzoic acida. What substances are present at equilibrium?b. At equilibrium, are reactants or products favored,and why?c. Are the concentrations of benzoic acid andbenzoate constant or changing at equilibrium?d. What happens to the equilibrium if morehydronium ions are added to the reaction?e. Label the conjugate acid-base pairs.

Benzoic acid reacts with water to form benzoate ion and the hydronium ion. The equilibrium reaction…

Answered: The conjugate base of benzoic acid is…

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter15: Acid–base Equilibria

Section: Chapter Questions

Problem 21P

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Similar questions

Formic acid, HCOOH, is found in ants. Write a balanced chemical equation to represent why an aqueous solution of formic acid is acidic.
Which has the larger numerical value? (a) The pKa of a strong acid or the pKa of a weak acid (b) The Ka of a strong acid or the Ka of a weak acid
Salicylic acid, HOC6H4CO2H, and its derivatives have been used as pain relievers for a long time. Salicylic acid occurs in small amounts in the leaves, bark, and roots of some vegetation (most notably historically in the bark of the willow tree). Extracts of these plants have been used as medications for centuries. The acid was first isolated in the laboratory in 1838. (a) Bath functional groups of salicylic acid ionize in water, with Ka=1.0103 for the—CO2H group and 4.201013 for the -OH group. What is the pH of a saturated solution of the acid (solubility = 1.8 g/L).. (b) Aspirin was discovered as a result of efforts to produce a derivative of salicylic acid that would not be irritating to the stomach lining. Aspirin is acetylsalicylic acid, CH3CO2C6H4CO2H. The -CO2H functional group is still present, but its acidity is reduced, Ka=3.0104. What is the pH of a solution of aspirin with the same concentration as a saturated solution of salicylic acid (See Part a). (c) Under some conditions, aspirin reacts with water and forms a solution of salicylic acid and acetic acid: CH3CO2C6H4CO2H(aq)+H2O(l)HOC6H4CO2H(aq)+CH3CO2H(aq) i. Which of the acids, salicylic acid or acetic acid, produces more hydronium ions in such a solution? ii. What are the concentrations of molecules and ions in a solution produced by the hydrolysis of 0.50 g of aspirin dissolved in enough water to give 75 mL of solution?
. A strong acid has a weak conjugate base, whereas a weak acid has a relatively strong conjugate base. Explain.
Compare the percent dissociation of the acid in Exercise 21a with the percent dissociation of the acid in Exercise 21d. Explain the large difference in percent dissociation of the acid.
The butylammonium ion, C4H9NH3+, has a Ka of 2.3 1011. C4H9NH3+(aq) + H2O() H3O+(aq) + C4H9NH2(aq) a) Calculate Kb for the conjugate base, C4H9NH2 (butyl amine). b) Place the butylammonium ion and its conjugate base in Table 16.2. Name an acid weaker than C4H9NH3+ and a base stronger than C4H9NH3. c) What is the pH of a 0.015M solution of butylammonium chloride?
In terms of orbitals and electron arrangements, what must be present for a molecule or an ion to act as a Lewis acid? What must be present for a molecule or an ion to act as a Lewis base?

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