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By G. Charlot

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199 (1931). 6. WALDEN and E. BIRR, Z. Physik. Chem. A163, 263, 321 (1932). 7. V . K . DOWNES, / . Am. Chem. Soc. 55, 1840 (1933). 8. HETZER, / . Res. Nat. Bur. Stand. 46, 496 (1951). 9. SINGLETERRY, / . Phys. Chem. 56, 604 (1952). 10. , / . Am. Chem. Soc. 74, 2691 (1952). 11. LEE, / . Am. Chem. Soc. 75, 1834 (1953). 12. HETZER, / . Am. Chem. Soc. 76, 4247 (1954). 13. A. YERGER, / . Am. Chem. Soc. 76, 5211, 5247, 5248 (1954). 14. C. R. HOLMES, / . Am. Chem. Soc. 11, Mil (1955). 15. A. BARROW, / .

Am. Chem. Soc. 7 1 , 1496 (1949). 18. A. LIFSON, / . Am. Chem. Soc. 73, 5889 (1951). 19. 20. 21. 22. 23. 24. 25. 26. 27. 28. 29. 30. R . M . ONSAGER, Proc. Nat. Acad. Sci. 4 1 , 274, 1010 (1955). Fuoss, J. Chim. Phys. 53, 493 (1956). ONSAGER, / . Phys. Chem. 6 1 , 668 (1957). Fuoss, / . Am. Chem. Soc. 79, 3301 (1957). ONSAGER, J. Phys. Chem. 62, 1339 (1958). Fuoss, / . Am. Chem. Soc. 80, 3163, 5059 (1958). H . S . H A R N E D and B . B . O W E N , The Physical Chemistry of Electrolytic Solutions, Reinhold, 3rd edition, 1958.

10)]. Further, it is possible to add a foreign salt BHA sufficiently concentrated and sufficiently dissociated so that the ion A~ concentration is constant. Then we have, even if the dissociation of IHA and H A is significant, A = constant — log c and, if the concentration of A~ is quite high, Kc and KA <^ [A~] where A x — pKi — log c For the indirect determination of pK of a base using an indicator I, the general formula is K 1 + —c^ ~ [A + l o g - ^ _ - Jog- A = pK-pKl C BHA ! , ] ^C 1 + [A-] where cB is the concentration of B, C BH A the concentration of its salt (BHA + BH+), and Kc and KQ are the ionic dissociation constants: v [IH+] [A-] [IHA] [BH+] [A~] [BHA] 2 CRS 34 CHEMICAL REACTIONS IN SOLVENTS AND MELTS It can be shown as before that [B] and [BHA] must be sufficiently concentrated to prevent appreciable dissociation of BHA and IHA.

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