Abstract
The apparent molal volume φ v of boric acid has been determined in various sodium chloride solutions at 0 and 25°C from precise density measurements. Similar to its behavior in pure water, the φ v of boric acid in NaCl solutions is a linear function of the concentration. The infinite dilution φ v ° and the slope S v * of B(OH)3 are larger in NaCl solutions than in pure water. NaCl appears to be able to dehydrate B(OH)3 and cause an increase in B(OH)3-B(OH)3 interactions. The mean apparent molal volumes Φ v of the B(OH)3-NaCl solutions are predicted from pure water data using a modification of Young's rule for electrolyte-nonelectrolyte mixtures and are compared to the directly measured values. A similar treatment was carried out on the density data of acetic acid-sodium chloride solutions. The modified Young's rule was found to give a good first approximation of the mean apparent molal volumes of nonelectrolyte-electrolyte systems. The deviations from the Young's rule approximation are studied as excess volumes of mixing boric acid and NaCl solutions.
| Original language | English (US) |
|---|---|
| Pages (from-to) | 431-444 |
| Number of pages | 14 |
| Journal | Journal of Solution Chemistry |
| Volume | 3 |
| Issue number | 6 |
| DOIs | |
| State | Published - Jun 1974 |
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Keywords
- Boric acid
- molal volume
- nonelectrolyte-electrolyte mixture
- volumes of mixing
ASJC Scopus subject areas
- Physical and Theoretical Chemistry
Cite this
Molal volume of aqueous boric acid-sodium chloride solutions. / Ward, Gary K.; Millero, Frank J.
In: Journal of Solution Chemistry, Vol. 3, No. 6, 06.1974, p. 431-444.Research output: Contribution to journal › Article
}
TY - JOUR
T1 - Molal volume of aqueous boric acid-sodium chloride solutions
AU - Ward, Gary K.
AU - Millero, Frank J
PY - 1974/6
Y1 - 1974/6
N2 - The apparent molal volume φ v of boric acid has been determined in various sodium chloride solutions at 0 and 25°C from precise density measurements. Similar to its behavior in pure water, the φ v of boric acid in NaCl solutions is a linear function of the concentration. The infinite dilution φ v ° and the slope S v * of B(OH)3 are larger in NaCl solutions than in pure water. NaCl appears to be able to dehydrate B(OH)3 and cause an increase in B(OH)3-B(OH)3 interactions. The mean apparent molal volumes Φ v of the B(OH)3-NaCl solutions are predicted from pure water data using a modification of Young's rule for electrolyte-nonelectrolyte mixtures and are compared to the directly measured values. A similar treatment was carried out on the density data of acetic acid-sodium chloride solutions. The modified Young's rule was found to give a good first approximation of the mean apparent molal volumes of nonelectrolyte-electrolyte systems. The deviations from the Young's rule approximation are studied as excess volumes of mixing boric acid and NaCl solutions.
AB - The apparent molal volume φ v of boric acid has been determined in various sodium chloride solutions at 0 and 25°C from precise density measurements. Similar to its behavior in pure water, the φ v of boric acid in NaCl solutions is a linear function of the concentration. The infinite dilution φ v ° and the slope S v * of B(OH)3 are larger in NaCl solutions than in pure water. NaCl appears to be able to dehydrate B(OH)3 and cause an increase in B(OH)3-B(OH)3 interactions. The mean apparent molal volumes Φ v of the B(OH)3-NaCl solutions are predicted from pure water data using a modification of Young's rule for electrolyte-nonelectrolyte mixtures and are compared to the directly measured values. A similar treatment was carried out on the density data of acetic acid-sodium chloride solutions. The modified Young's rule was found to give a good first approximation of the mean apparent molal volumes of nonelectrolyte-electrolyte systems. The deviations from the Young's rule approximation are studied as excess volumes of mixing boric acid and NaCl solutions.
KW - Boric acid
KW - molal volume
KW - nonelectrolyte-electrolyte mixture
KW - volumes of mixing
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U2 - 10.1007/BF00651534
DO - 10.1007/BF00651534
M3 - Article
VL - 3
SP - 431
EP - 444
JO - Journal of Solution Chemistry
JF - Journal of Solution Chemistry
SN - 0095-9782
IS - 6
ER -