Apparent molal volumes of aqueous NaF, Na2SO4, KCl, K2SO4, MgCl2, and MgSO4 solutions at 0° and 50°C

Frank J Millero, Jonathan H. Knox

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Abstract

The apparent molal volumes, ΦV's, of dilute (0.002-1m) aqueous solutions of NaF, Na2SO4, KCl, K2SO4, MgCl2, and MgSO4 are determined at 0° and 500C from precision density measurements made with a magnetic float densitometer. The infinite dilution apparent molal volumes, ΦV°'s, are determined by using the Redlich equation, ΦV = ΦV° + SVc1/2 + bVc, where SV is the Debye-Hückel limiting law slope, and bV is a deviation constant. At 0°C the deviations are positive for all the salts except MgCl2. The temperature dependence of the bV for all the salts is similar to other common electrolytes (∂bV/∂T is negative). The effect of temperature on the ΦV°'s of all the electrolytes is similar in that ∂2ΦV°/∂T2 is negative. The ion-ion and ion-water interactions responsible for the observed behavior of the ΦV's are briefly discussed.

Original languageEnglish (US)
Pages (from-to)407-411
Number of pages5
JournalJournal of Chemical and Engineering Data
Volume18
Issue number4
StatePublished - 1973

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Magnesium Chloride
Ions
Electrolytes
Salts
Densitometers
Dilution
Temperature
Water

ASJC Scopus subject areas

  • Chemistry(all)
  • Chemical Engineering(all)

Cite this

Apparent molal volumes of aqueous NaF, Na2SO4, KCl, K2SO4, MgCl2, and MgSO4 solutions at 0° and 50°C. / Millero, Frank J; Knox, Jonathan H.

In: Journal of Chemical and Engineering Data, Vol. 18, No. 4, 1973, p. 407-411.

Research output: Contribution to journalArticle

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abstract = "The apparent molal volumes, ΦV's, of dilute (0.002-1m) aqueous solutions of NaF, Na2SO4, KCl, K2SO4, MgCl2, and MgSO4 are determined at 0° and 500C from precision density measurements made with a magnetic float densitometer. The infinite dilution apparent molal volumes, ΦV°'s, are determined by using the Redlich equation, ΦV = ΦV° + SVc1/2 + bVc, where SV is the Debye-H{\"u}ckel limiting law slope, and bV is a deviation constant. At 0°C the deviations are positive for all the salts except MgCl2. The temperature dependence of the bV for all the salts is similar to other common electrolytes (∂bV/∂T is negative). The effect of temperature on the ΦV°'s of all the electrolytes is similar in that ∂2ΦV°/∂T2 is negative. The ion-ion and ion-water interactions responsible for the observed behavior of the ΦV's are briefly discussed.",
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N2 - The apparent molal volumes, ΦV's, of dilute (0.002-1m) aqueous solutions of NaF, Na2SO4, KCl, K2SO4, MgCl2, and MgSO4 are determined at 0° and 500C from precision density measurements made with a magnetic float densitometer. The infinite dilution apparent molal volumes, ΦV°'s, are determined by using the Redlich equation, ΦV = ΦV° + SVc1/2 + bVc, where SV is the Debye-Hückel limiting law slope, and bV is a deviation constant. At 0°C the deviations are positive for all the salts except MgCl2. The temperature dependence of the bV for all the salts is similar to other common electrolytes (∂bV/∂T is negative). The effect of temperature on the ΦV°'s of all the electrolytes is similar in that ∂2ΦV°/∂T2 is negative. The ion-ion and ion-water interactions responsible for the observed behavior of the ΦV's are briefly discussed.

AB - The apparent molal volumes, ΦV's, of dilute (0.002-1m) aqueous solutions of NaF, Na2SO4, KCl, K2SO4, MgCl2, and MgSO4 are determined at 0° and 500C from precision density measurements made with a magnetic float densitometer. The infinite dilution apparent molal volumes, ΦV°'s, are determined by using the Redlich equation, ΦV = ΦV° + SVc1/2 + bVc, where SV is the Debye-Hückel limiting law slope, and bV is a deviation constant. At 0°C the deviations are positive for all the salts except MgCl2. The temperature dependence of the bV for all the salts is similar to other common electrolytes (∂bV/∂T is negative). The effect of temperature on the ΦV°'s of all the electrolytes is similar in that ∂2ΦV°/∂T2 is negative. The ion-ion and ion-water interactions responsible for the observed behavior of the ΦV's are briefly discussed.

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