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Chapter 17 Aqueous Ionic Equilibrium 389 (c) + + (e) 6.00 = 6.40 + log -0.40 = log = = 0.398107 In order for a buffer to be effective, the relative concentration of the acid and conjugate base should be within a factor of 10 of magnitude of each other. In order to neutralize 0.010 M acid, the concentration of the acid in the buffer should be at least 0.100 M. If the initial buffer concentrations are = 0.100 M and [C₆H₅O₇³⁻] = 0.040 M, after neutralizing 0.010 M acid these concentrations would change to = 0.110 M and [C₆H₅O₇³⁻] = 0.030 M. These are still within the guidelines for a buffer solution. Using the potassium salts, the buffer solution would be = 0.100 M and [K₃C₆H₅O₇] = 0.040 M. Copyright © 2017 Pearson Education, Inc.