The thermodynamic dissociation constant of the phenol group of p-phenolsulfonic acid was calculated from electromotive-force measurements of hydrogensilver-chloride cells without liquid junction. Thirty-nine buffer mixtures of potassium p-phenolsulfonate, sodium hydroxide, and sodium chloride were studied in five series of experiment s from 0° to 60° C at intervals of 5 degrees. In three series, t he molal ratio of phenolsulfonate ion to phenolate-sulfonate ion was unity, and in two series the buffer ratio was 2 :3. For two series of experiments, one at each buffer ratio, the molality of sodium chloride was m aintained constant near 0.05 for all dilutions of t he buffer. In the other experiments, the molality of each component of t he solut ion varied bet ween 0.0037 and 0.1.The values of pK2' the negative of the common logarithm of the second dissociat ion constant, between 0° and 60° C are given by the equation012139T, where T is in degrees Kelvin.Equations were formulated to give the changes of free energy, heat content, entropy, and heat capacity that accompany t he dissociation, at infinite dilution, of a mole of phenolsulfonate ion at any temperature between 0° and 60° C. For the dissociation of the phenol group at 25° C, ~F o is 12,351 cal, ~Ho is 4,036 cal, ~So is -27.9 cal deg-1, and ~c o p is -33 cal deg-1•The pH value of each buffer-chloride mixture was calculated from the experimental data and the activity coefficients that were found to characterize each series of solutions. The pH values of other phenolsulfonate buffers which have m olal ratios, mdm2, of phenolsulfonate ion to bivalent phenolate-sulfonate ion between 2/3 and 1 can be computed for temperatures between 0° and 60° C with an accuracy of ± 0.002 unit from their compositions and from the dissociation constants and ionic parameters given in this paper. The equation used is pH =pK2 -log (mt/m2) -3A.JJ;f(1 +8B-V JL), where JL is the ionic strength . Buffer solutions of this type are suitable pH standards in the range 8.6 to 9.0.
CONTENTS