nuclear magnetic resonance studies of hydrogen bonding. i

Jeff C. Davis, Jr., and Kenneth S. Pitzer. Vol. 64. NS 6. —*•% METHANOL. Fig. 5. method applied intheir derivation, it is interesting to notice th...
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JEFFC. D A ~ I JR.. H . ASD KEXNETH S.PITZEI~

7-01, 64

case, although the similarities of the respective [TIS add weight to the assumption that one deals here indeed with B solvents, the difficulties of application of a 0 solvent concept to solutionr of blockpolymers shoidd he clearly recognized. TARLE IV 5%

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Type of Methanol [vlgIsodctane blockin " R 3101. u-t. 3101. wt. in "e 3101 a t . w l y m e r solvent" 158,000 15,800 solvent" 1 j8,OOO S p

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O.fi5 .OO .63 .. The calculated 6ar drop\ rapidly with increasing temperature and approacheq the region in which :dcohol monomers also are found This behavior of the monomer -hift\ i b itrongly suggestive of nn interaction of the moiionier with the benzene wlvent. It is recognized that molecules with acidic protons a+ociate TTith benzene. and n.m.r. ctudies indicate in swli an association the proton i i drawn into the face of the benzene molecule rather than around the edge.15 I t habeen show1 that the benzene molecule exhibits an anisotropic diamagnetic s eptibility 11-hich can tie xrielved a s arising from a culation of the mobile x electrons around the ring induced by the external magnetic field.Ifi Thege circulating electrons give rise to a qecondary magnetic field around the benzene molecule 'The rnagnitude of this field averaged over all orientationq of the benzene molecule n-ith timr hn- it~eiicalculaterl hy 1-nrioiis means."

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(17) .I. S. Wailah and R T?i Fessenden J . 4m Chem SOC.,7 9 , 84h C. E. J o h n w n Jr., and P A . Bovey, J . Chem Phiis., 29, 1012 (1958). 11957);

(18) See T. Miyazana a n d IC. S. Pltzer, ibzd information on the trann isomer of formic acid.

30. 1076 (1059), for

July, 1960

K T C L E iR 31-4GNETIC

RESONANCE STCDIES O F HYDROGEN RONDISG

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TABLEVI association in the aqueous phase, and possible DIMER SHIFTS O F BENZOIC higher polymers. The equilibrium constants obtained by Davies were used to calculate the monoACID IS BEXZENE AFTERADJTSTMENT OF EQUILIBRII-M mer and dimer shifts for acetic acid in benzene at COSSTASTS qeveral temperatures. Daries' values of AH = ( A H = -5.62 kcnl. mole I )

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-8.89 kcal. mole-' and A S = 19.82 cal. deg.-' inole-' were used t o cdculate KSat higher temperatures. The resulting constants and shifts are listed i n Table YII. TABLEVI1 DIVERSHIFTSFOR IN BENZENE ( A H = -8.2 kcal. mole-')

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