pH values of certain phosphate-chloride mixtures, and the second dissociation constant of phosphoric acid from 0 degrees to 60 degrees C

Heat capacities and volumes of dissociation of phosphoric acid (1st, 2nd, and 3rd), bicarbonate ion, and bisulfate ion in aqueous solution

“…We suggest that our ACpO = -220 J K-' mol-I is the best available value. Although we are generally skeptical of ACpO values based on double differentiation of log K = f(T), we note that the equilibrium constants of Bates and Acree (26) and Grzybowski (28) appear to have been determined with considerable skill and accuracy; it is therefore gratifying to note that their (26,28) ACpO values are in good agreement with our value.…”

Heat capacities and volumes of dissociation of phosphoric acid (1st, 2nd, and 3rd), bicarbonate ion, and bisulfate ion in aqueous solution

“…We suggest that our ACpO = -220 J K-' mol-I is the best available value. Although we are generally skeptical of ACpO values based on double differentiation of log K = f(T), we note that the equilibrium constants of Bates and Acree (26) and Grzybowski (28) appear to have been determined with considerable skill and accuracy; it is therefore gratifying to note that their (26,28) ACpO values are in good agreement with our value.…”

Comparative liquid-junction potentials of some pH buffer standards and the calibration of pH meters

“…All values were corrected to I-atmosphere pressure of hydrogen gas. The values for (El + E2) reported here for hydrochloric acid, hydrochloric acid-sodium chloride, phthalate, phenolsulfonate, and borax agreed withi.n 0.05 mv with data published previously for these buffers; the emf for the phosphate buffer was 0.11 mv (0.0018 pH unit) higher than that subsequently found by Bates in an extension of his work [3], but is within I;he precision claimed for these measmements. The pH value for the phenolsulfonate buffer was recalculated by a somewhat more detailed method and is 0.006 unit higher thm that previously reporl;ed [4a] .…”

Investigation of α-deuterium kinetic isotope effects on the purine nucleoside phosphorylase reaction by the equilibrium-perturbation technique

“…2 shows that in fact the equilibrium constant varies with pH in the way expected from the differing pK2 values of phosphoric acid and ribose 1phosphate. The infinite-dilution pK2 of phosphoric acid (7.2) decreases with ionic strength and at an ionic strength of 0.1 is around 6.8 (Bates & Acree, 1943). We find the pK2 of ribose 1-phosphate, whose infinite-dilution pK2 is probably close to that of glucose 1-phosphate (6.5;Ashby et al, 1955), to be 6.2 in 0.1 M-NaCl.…”

Heat capacities and volumes of dissociation of phosphoric acid (1st, 2nd, and 3rd), bicarbonate ion, and bisulfate ion in aqueous solution

“…We suggest that our ACpO = -220 J K-' mol-I is the best available value. Although we are generally skeptical of ACpO values based on double differentiation of log K = f(T), we note that the equilibrium constants of Bates and Acree (26) and Grzybowski (28) appear to have been determined with considerable skill and accuracy; it is therefore gratifying to note that their (26,28) ACpO values are in good agreement with our value.…”

Comparative liquid-junction potentials of some pH buffer standards and the calibration of pH meters

“…All values were corrected to I-atmosphere pressure of hydrogen gas. The values for (El + E2) reported here for hydrochloric acid, hydrochloric acid-sodium chloride, phthalate, phenolsulfonate, and borax agreed withi.n 0.05 mv with data published previously for these buffers; the emf for the phosphate buffer was 0.11 mv (0.0018 pH unit) higher than that subsequently found by Bates in an extension of his work [3], but is within I;he precision claimed for these measmements. The pH value for the phenolsulfonate buffer was recalculated by a somewhat more detailed method and is 0.006 unit higher thm that previously reporl;ed [4a] .…”

Investigation of α-deuterium kinetic isotope effects on the purine nucleoside phosphorylase reaction by the equilibrium-perturbation technique

“…2 shows that in fact the equilibrium constant varies with pH in the way expected from the differing pK2 values of phosphoric acid and ribose 1phosphate. The infinite-dilution pK2 of phosphoric acid (7.2) decreases with ionic strength and at an ionic strength of 0.1 is around 6.8 (Bates & Acree, 1943). We find the pK2 of ribose 1-phosphate, whose infinite-dilution pK2 is probably close to that of glucose 1-phosphate (6.5;Ashby et al, 1955), to be 6.2 in 0.1 M-NaCl.…”

Heat capacities and volumes of dissociation of phosphoric acid (1st, 2nd, and 3rd), bicarbonate ion, and bisulfate ion in aqueous solution

“…We suggest that our ACpO = -220 J K-' mol-I is the best available value. Although we are generally skeptical of ACpO values based on double differentiation of log K = f(T), we note that the equilibrium constants of Bates and Acree (26) and Grzybowski (28) appear to have been determined with considerable skill and accuracy; it is therefore gratifying to note that their (26,28) ACpO values are in good agreement with our value.…”

Comparative liquid-junction potentials of some pH buffer standards and the calibration of pH meters

“…All values were corrected to I-atmosphere pressure of hydrogen gas. The values for (El + E2) reported here for hydrochloric acid, hydrochloric acid-sodium chloride, phthalate, phenolsulfonate, and borax agreed withi.n 0.05 mv with data published previously for these buffers; the emf for the phosphate buffer was 0.11 mv (0.0018 pH unit) higher than that subsequently found by Bates in an extension of his work [3], but is within I;he precision claimed for these measmements. The pH value for the phenolsulfonate buffer was recalculated by a somewhat more detailed method and is 0.006 unit higher thm that previously reporl;ed [4a] .…”

Investigation of α-deuterium kinetic isotope effects on the purine nucleoside phosphorylase reaction by the equilibrium-perturbation technique

“…2 shows that in fact the equilibrium constant varies with pH in the way expected from the differing pK2 values of phosphoric acid and ribose 1phosphate. The infinite-dilution pK2 of phosphoric acid (7.2) decreases with ionic strength and at an ionic strength of 0.1 is around 6.8 (Bates & Acree, 1943). We find the pK2 of ribose 1-phosphate, whose infinite-dilution pK2 is probably close to that of glucose 1-phosphate (6.5;Ashby et al, 1955), to be 6.2 in 0.1 M-NaCl.…”