Which of the statements below best describes this equilibrium: HCIO4 + CH3CO2 CIO4 + CH3CO₂H Note: the Ka of CH3CO₂H is 1.8 x 10.5 This is a product-favored equilibrium and the final solution is acidic This is a product-favored equilibrium and the final solution is basic This is a reactant-favored equilibrium and the final solution is acidic O This is a reactant-favored equilibrium and the final solution is basic

Which of the statements below best describes this equilibrium: HCIO4 + CH3CO2 CIO4 + CH3CO₂H Note: the Ka of CH3CO₂H is 1.8 x 10.5 This is a product-favored equilibrium and the final solution is acidic This is a product-favored equilibrium and the final solution is basic This is a reactant-favored equilibrium and the final solution is acidic O This is a reactant-favored equilibrium and the final solution is basic

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter14: Acids And Bases

Section: Chapter Questions

Problem 181CP: Calculate the pH of a 0.200-M solution of C5H5NHF. Hint: C5H5NHF is a salt composed of C5H5NH+ and F...

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Most naturally occurring acids are weak acids. Lactic acid is one example. CH3CH(OH)CO2H(s)+H2O(l)H3O+(aq)+CH3CH(OH)CO2(aq) If you place some lactic acid in water, it will ionize to a small extent, and an equilibrium will be established. Suggest some experiments to prow that this is a weak acid and that the establishment of equilibrium is a reversible process.
Calculate the pH of a 0.200-M solution of C5H5NHF. Hint: C5H5NHF is a salt composed of C5H5NH+ and F ions. The principal equilibrium in this solution is the best acid reacting with the best base; the reaction for the principal equilibrium is C5H5NH+(aq)+F(aq)C5H5N(aq)+HF(aq)K=8.2103
Consider a 0.60-M solution of HC3H5O3, lactic acid (Ka = 1.4 104). a. Which of the following are major species in the solution? i. HC3H5O3 ii. C3H5O3 iii. H+ iv. H2O v. OH b. Complete the following ICE table in terms of x, the amount (mol/L) of lactic acid that dissociates to reach equilibrium. c. What is the equilibrium concentration for C3H3O3? d. Calculate the pH of the solution.
Characterize each of the following as product- or reactant-favored at equilibrium. (a) CO(g) + O2(g) CO2(g)Kp = 1.2 1045 (b) H2O(g) H2(g) + O2(g)Kp = 9.1 1041 (c) CO(g) + Cl2(g) COCl2(g)Kp = 9.1 1011
We have seen an introductory definition of an acid: An acid is a compound that reacts with water and increases the amount of hydronium ion present. In the Chapter on acids and bases, we saw two more definitions of acids: a compound that donates a proton (a hydrogen ion, H+) to another compound is called a Bronsted-Lowry acid, and a Lewis acid is any species that can accept a pair of electrons. Explain why the introductory definition is a macroscopic definition, while the Bronsted-Lomy definition and the Lewis definition are microscopic definitions.
What 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 + OH
What is the effect on the concentrations of NO2-, HNO2, and OH- when the following are added to a solution of KNO2 in water: (a) HCl. (b) HNO2. (c) NaOH. (d) NaCl. (e) KNO The equation for the equilibrium is: NO2(aq)+H2O(l)HNO2+OH(aq)
Consider the following aqueous chemical equilibrium of benzoic acid, a weak acid: C6H5COOH(aq) + H2O(l) is in equilibrium with H3O+(aq) + C6H5COO-(aq) a. The addition of H3O+(aq) to the chemical equilibrium will have what effect on the amount (moles) of C6H5COO-(aq) in the system? b. Addition of OH-(aq) to the chemical equilibrium will have what effect on the amount (moles) of C6H5COOH(aq) in the system? c. Removal of C6H5COO-(aq) from the chemical equilibrium will have what effect on the amount of (moles) H3O+(aq) in the system? d. Increasing the pH of the solution will have what effect on the amount (moles) of C6H5COOH(aq) in the system?