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  1. For a summary of the literature on this subject, see pp. 1018–1020 in J. N. Demas, G. A. Crosby, J. Chem. Phys. 75, 991 (1971).
  2. L. W. Tilton, J. K. Taylor, in Physical Methods in Chemical Analysis, Vol. 1 (Academic, New York, 1960), p. 455.
  3. R. C. Weast, Ed., Handbook of Chemistry and Physics (Chemical Rubber Company, Cleveland, Ohio, 1971/72).
  4. The two KNO3 solutions were prepared by R. W. Burke (Analytical Chemistry Division, NBS), and their indices were measured by M. J. Dodge (Optical Physics Division, NBS). The values for nH2O were computed from Eq. (3) of this paper.
  5. E. W. W Hashburn, Ed., International Critical Tables (McGraw-Hill, New York, 1930), Vol. 7, p. 13.
  6. J. Bartels et al., Eds., Landolt-Börnstein Zahlenwerte und Funktionen (Springer, Berlin, 1962), Vol. 2/8, p. 5–565.
  7. D. E. Gray, Ed., American Institute of Physics Handbook (McGraw-Hill, New York, 1972), p. 6–105.
  8. L. W. Tilton, J. K. Taylor, J. Res. NBS 20, 419 (1938).
  9. L. H. Dawson, E. Hulburt, J. Opt. Soc. Am. 24, 175 (1934).
    [CrossRef]
  10. R. A. Velapoldi, K. D. Mielenz, “A Fluorescence Standard Reference Material: Quinine Sulfate Dihydrate,” NBS Special Publication (1978), to be published.

1971 (1)

For a summary of the literature on this subject, see pp. 1018–1020 in J. N. Demas, G. A. Crosby, J. Chem. Phys. 75, 991 (1971).

1938 (1)

L. W. Tilton, J. K. Taylor, J. Res. NBS 20, 419 (1938).

1934 (1)

Crosby, G. A.

For a summary of the literature on this subject, see pp. 1018–1020 in J. N. Demas, G. A. Crosby, J. Chem. Phys. 75, 991 (1971).

Dawson, L. H.

Demas, J. N.

For a summary of the literature on this subject, see pp. 1018–1020 in J. N. Demas, G. A. Crosby, J. Chem. Phys. 75, 991 (1971).

Hulburt, E.

Mielenz, K. D.

R. A. Velapoldi, K. D. Mielenz, “A Fluorescence Standard Reference Material: Quinine Sulfate Dihydrate,” NBS Special Publication (1978), to be published.

Taylor, J. K.

L. W. Tilton, J. K. Taylor, J. Res. NBS 20, 419 (1938).

L. W. Tilton, J. K. Taylor, in Physical Methods in Chemical Analysis, Vol. 1 (Academic, New York, 1960), p. 455.

Tilton, L. W.

L. W. Tilton, J. K. Taylor, J. Res. NBS 20, 419 (1938).

L. W. Tilton, J. K. Taylor, in Physical Methods in Chemical Analysis, Vol. 1 (Academic, New York, 1960), p. 455.

Velapoldi, R. A.

R. A. Velapoldi, K. D. Mielenz, “A Fluorescence Standard Reference Material: Quinine Sulfate Dihydrate,” NBS Special Publication (1978), to be published.

J. Chem. Phys. (1)

For a summary of the literature on this subject, see pp. 1018–1020 in J. N. Demas, G. A. Crosby, J. Chem. Phys. 75, 991 (1971).

J. Opt. Soc. Am. (1)

J. Res. NBS (1)

L. W. Tilton, J. K. Taylor, J. Res. NBS 20, 419 (1938).

Other (7)

R. A. Velapoldi, K. D. Mielenz, “A Fluorescence Standard Reference Material: Quinine Sulfate Dihydrate,” NBS Special Publication (1978), to be published.

L. W. Tilton, J. K. Taylor, in Physical Methods in Chemical Analysis, Vol. 1 (Academic, New York, 1960), p. 455.

R. C. Weast, Ed., Handbook of Chemistry and Physics (Chemical Rubber Company, Cleveland, Ohio, 1971/72).

The two KNO3 solutions were prepared by R. W. Burke (Analytical Chemistry Division, NBS), and their indices were measured by M. J. Dodge (Optical Physics Division, NBS). The values for nH2O were computed from Eq. (3) of this paper.

E. W. W Hashburn, Ed., International Critical Tables (McGraw-Hill, New York, 1930), Vol. 7, p. 13.

J. Bartels et al., Eds., Landolt-Börnstein Zahlenwerte und Funktionen (Springer, Berlin, 1962), Vol. 2/8, p. 5–565.

D. E. Gray, Ed., American Institute of Physics Handbook (McGraw-Hill, New York, 1972), p. 6–105.

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Figures (1)

Fig. 1
Fig. 1

Residuals, nmeasuredncomputed, of the refractive indices of water calculated from the dispersion formula of Tilton and Taylor8 and from Eq. (3) of this paper. The sixty-six values of nmeasured plotted in this graph were taken from Refs. 57.

Tables (1)

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Table I Effect of Solute Concentration on the Refractive Index and Dispersion of Two Aqueous KNO3 Solutions

Equations (3)

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I ext = I int / n 2 ,
n n = k c ,
n H 2 O 2 ( 20 ° C ) = 1.7604457 + 4.03368 × 10 3 λ 1.54182 × 10 2 λ 2 + 6.44277 × 10 3 λ 2 1.49119 × 10 2 , 0.235 μ m < λ < 1.028 μ m ,

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