Carboxylic acids are weak acids and dissociate in an aqueous solution to the carboxylate anion. RCOOH(aq)↽−−⇀RCOO−(aq)+H+(aq) (Arrow is Reversible) The extent of dissociation is given by the equilibrium dissociation constant, Ka, which is often expressed in its logarithmic form as pKa. (The cation is written simply as H+ and is understood to be solvated with one or more water molecules in solution.) ?a=[H+][RCOO−]/[RCOOH] pKa=−log(Ka) If a formic acid in formate buffer is 0.022 M in formic acid and has a pH of 3.85, what is the molar concentration of the formate ion? The pKa of formic acid is 3.75.
Carboxylic acids are weak acids and dissociate in an aqueous solution to the carboxylate anion. RCOOH(aq)↽−−⇀RCOO−(aq)+H+(aq) (Arrow is Reversible) The extent of dissociation is given by the equilibrium dissociation constant, Ka, which is often expressed in its logarithmic form as pKa. (The cation is written simply as H+ and is understood to be solvated with one or more water molecules in solution.) ?a=[H+][RCOO−]/[RCOOH] pKa=−log(Ka) If a formic acid in formate buffer is 0.022 M in formic acid and has a pH of 3.85, what is the molar concentration of the formate ion? The pKa of formic acid is 3.75.
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter16: Reactions Between Acids And Bases
Section: Chapter Questions
Problem 16.83QE
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RCOOH(aq)↽−−⇀RCOO−(aq)+H+(aq) (Arrow is Reversible)
The extent of dissociation is given by the equilibrium dissociation constant, Ka, which is often expressed in its logarithmic form as pKa. (The cation is written simply as H+ and is understood to be solvated with one or more water molecules in solution.)
?a=[H+][RCOO−]/[RCOOH]
pKa=−log(Ka)
If a formic acid in formate buffer is 0.022 M in formic acid and has a pH of 3.85, what is the molar concentration of the formate ion? The pKa of formic acid is 3.75.
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