Simultaneous measurement of oxygen diffusion coefficients and solubilities in electrolyte solutions with a polarographic oxygen electrode

Ho, Chester S.; Ju, Lu‐Kwang; Baddour, R. F.; Wang, Daniel I.C.

doi:10.1016/0009-2509(88)80061-7

Cited by 33 publications

(21 citation statements)

References 40 publications

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“…As already mentioned, similar methods have been used numerous times to measure the diffusivities of gases in liquids. 9,10,13,16,23,32,33,37 The main complication in applying this approach to NO was that, to avoid artifacts due to chemical reactions, great care was needed to remove O 2 from the system. Simulations of O 2 removal during a preliminary purge period (Fig.…”

Section: Discussionmentioning

confidence: 99%

“…In a few instances, transient and steady state information have been combined to determine both the diffusivity and the solubility. 13,16 In the work reported here, we used a chemiluminescence detector to measure transient and steady fluxes of NO across aqueous films bounded by polydimethylsiloxane (Silastic) membranes. Oxygen was purged from the system to ensure that reactions would not influence the measured fluxes, and separate measurements of NO permeation through the Silastic membranes were made to account for their contributions to the overall resistance.…”

Section: Introductionmentioning

confidence: 99%

“…The advantage in using transient data, either by extracting the lag time before a flux is observed 13,16,37 or fitting the full set of time-dependent data, 9 is that the calculated diffusivity is independent of solubility. In a few instances, transient and steady state information have been combined to determine both the diffusivity and the solubility.…”

Section: Introductionmentioning

confidence: 99%

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Diffusivity and Solubility of Nitric Oxide in Water and Saline

2005

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Aqueous diffusivities and solubilities of NO were determined by using a chemiluminescence detector to measure time-dependent fluxes across stagnant liquid films confined between polydimethylsiloxane membranes. The NO diffusivities in pure water and PBS at 25 degrees C were found to be (2.21+/-0.02) x 10(-5) cm2 s(-1) and (2.21+/-0.04) x 10(-5) cm2 s(-1), respectively. Although lower than most previous values for NO at room temperature, these diffusivities are very similar to those for O2, as one would expect. Extrapolation to 37 degrees C yielded a value of 3.0 x 10(-5) cm2 s(-1). The solubility of NO in water at 25 degrees C was (1.94+/-0.03) x 10(-6) mol cm(-3) atm(-1), in agreement with the literature. This agreement, along with the excellent fits obtained to the transient flux data (<4% rms error in each experiment), supports the validity of the simultaneously measured diffusivity. The solubility of NO in PBS at 25 degrees C was (1.75+/-0.02) x 10(-6) mol cm(-3) atm(-1). The modest (10%) reduction in solubility relative to that in pure water is consistent with the usual effects of salts on gas solubilities.

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Section: Discussionmentioning

confidence: 99%

Section: Introductionmentioning

confidence: 99%

Section: Introductionmentioning

confidence: 99%

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Diffusivity and Solubility of Nitric Oxide in Water and Saline

2005

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“…16 D O2w may be calculated using the relation given by St-Denis and Fell. 18 The diffusion coefficient of oxygen in Fe II (EDTA) solutions (D O2 ) may be calculated from D O2w using a relation given by Ho et al 19 3.3 Determination of the Stoichiometric Coefficient. To obtain information of possible other oxygenconsuming reactions besides the main reaction, the stoichiometric coefficient of iron for the reaction has to be determined experimentally.…”

Section: Calculation Of the Kinetics Of The Oxidationmentioning

confidence: 99%

Kinetics of the Reaction of Fe^II(EDTA) with Oxygen in Aqueous Solutions

Gambardella¹,

Ganzeveld

Winkelman³

et al. 2005

Ind. Eng. Chem. Res.

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The kinetics of the reaction of oxygen with aqueous Fe II (EDTA) solutions has been determined in a range of process conditions (C Fe II (EDTA) ) 15-60 mol/m 3 , P O2 ) 5-20 kPa, pH ) 5-8, T ) 298-328 K, C NaCl ) 0-15 kg/m 3 ) using a gas-liquid stirred cell reactor. The oxygen absorption rates were modeled using an expression derived by De Coursey using the penetration theory of mass transfer. Within the range of process conditions applied, the reaction was shown to be first order in oxygen and second order in iron chelate. The temperature dependence of the kinetic constant may be expressed as (pH ) 7, no salt addition): k 12 ) 5.3 × 10 3 e -4098/T m 6 /(mol 2 ‚s). The kinetic constant is essentially independent of the pH in the range 5 < pH < 8. When applying a NaCl concentration of 15 kg/m 3 , the kinetic constant increases ∼35% (T ) 328 K). The oxidation of Fe II (EDTA) to Fe III (EDTA) is not the sole oxygen-consuming reaction. The extent of side reactions, possibly related to EDTA ligand degradation, is a function of the pH and the oxygen concentration. A remarkable, unprecedented step change in the selectivity of the reaction was observed when the reaction was performed at a higher oxygen concentration.

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“…The value of the diffusion coefficient of oxygen in Fe II (EDTA) 2− solutions was calculated using the diffusivity of oxygen in water (Janssen and Warmoeskerken, 1987) and applying a correction for the influence of viscosity in aqueous electrolyte solutions (Ho et al, 1990). The diffusion coefficients of the iron chelate, D B , was taken from O' Connor et al, 1971.…”

Section: Estimation Of Parametersmentioning

confidence: 99%