Consider the following equilibrium between ethanoic acid (K, = 1.8×10 ) and its conjugate base: H2O + H;O* CH3C-OH (1) Will lowering the pH shift the equilibrium to the right or to the left? (2) Calculate the ratio of the concentration of acetate ion to the concentration of acetic acid at a pH of 3.07. ratio [conjugate base] / [acid] =

Consider the following equilibrium between ethanoic acid (K, = 1.8×10 ) and its conjugate base: H2O + H;O* CH3C-OH (1) Will lowering the pH shift the equilibrium to the right or to the left? (2) Calculate the ratio of the concentration of acetate ion to the concentration of acetic acid at a pH of 3.07. ratio [conjugate base] / [acid] =

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Concept explainers

Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

Question

Consider the following equilibrium between ethanoic acid (K, = 1.8×10 ) and its conjugate base:
H2O
+ H;O*
CH3C-OH
(1) Will lowering the pH shift the equilibrium to the right or to the left?
(2) Calculate the ratio of the concentration of acetate ion to the concentration of acetic acid at a pH of 3.07.
ratio [conjugate base] / [acid] =

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