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Ionic conductance of HMIM-Br

  • Rudolf Holze
Chapter
Part of the Physical Chemistry book series (volume 9B2)

Abstract

This chapter contains a tabular compilation of ionic conductance of HMIM-Br at various temperatures.

Table 1.7.2

Ionic conductances of aqueous solutions

Electrolyte

k or Λ or Λ01

−1cm−1 or Ω−1mol−1cm2]

T

[K or °C]

c 2

[mol · dm−3]

k or Λ or Λ01

−1cm−1 or Ω−1mol−1cm2]

T

[K or °C]

c 2

[mol · dm−3]

Ref.

HMIM-Br

128.73

298.15

0.9205·10−3

127.34

298.15

0.0027486

[11She2]

124.74

298.15

4.5962·10−3

121.64

298.15

0.0074616

[11She2]

118.71

298.15

10.3712·10−3

115.26

298.15

0.0143768

[11She2]

112.12

298.15

18.3849·10−3

107.95

298.15

0.0234673

[11She2]

104.81

298.15

28.6145·10−3

101.49

298.15

0.0345851

[11She2]

98.41

298.15

40.7307·10−3

95.14

298.15

0.0479006

[11She2]

1Conductances at infinite dilution Λ0 are printed in italics without mentioning a concentration, units are Ω−1 mol−1cm2. Molar conductances are given in italics with a concentration value, units are Ω−1 mol−1cm2. Simple conductivities are given stating the concentration, units are Ω−1 cm−1

2Concentrations are molar (units: mol · dm−3), molal concentrations are given in italics (units: mol · kg−1), other concentrations as specified

Symbols and Abbreviations

Short form

Full form

κ, Λ

ionic conductivity

T

temperature

Λ 0

ionic conductance at infinite dilution

c

molar concentration

References

  1. [11She2]
    Shekaari, H., Jebali, F.: Phys. Chem. Liqu. 49 (2011) 572.CrossRefGoogle Scholar

Copyright information

© Springer-Verlag Berlin Heidelberg 2016

Authors and Affiliations

  • Rudolf Holze
    • 1
  1. 1.Technische Universität ChemnitzInstitut für ChemieChemnitzGermany

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