Ion exchange in micellar solutions. 2. Binding of hydroxide ion to positive micelles

1979 ◽  
Vol 83 (14) ◽  
pp. 1851-1854 ◽  
Author(s):  
H. Chaimovich ◽  
J. B. S. Bonilha ◽  
M. J. Politi ◽  
F. H. Quina
Keyword(s):  
Ion Exchange ◽  
Micellar Solutions ◽  
Hydroxide Ion

Counterion micellar effects upon the reaction of low-spin diimine iron(II) complexes

1989 ◽  
Vol 67 (2) ◽  
pp. 305-309 ◽  
Author(s):  
Francisco Ortega ◽  
Elvira Rodenas
Keyword(s):  
Ion Exchange ◽  
Exchange Model ◽  
Micellar Solutions ◽  
Micellar Effects ◽  
Hydroxide Ion ◽  
Cationic Micelles ◽  
Rate Effects ◽  
Rate Of Reaction

The rate of reaction of tris(1,10-phenanthroline)iron(II) ion (1a), tris(3,4,7,8-tetramethyl-1,10-phenanthroline)iron(II) ion (1b), and tris(4,7-diphenhyl-1, 10-phenanthroline)iron(II) ion (1c) with hydroxide ion, in cationic micelles, is strongly affected by the concentration of micellar counterion in solution. The reaction of la in CTACl is modestly speeded up by the addition of added KCl, while the reactions of 1b and 1c are strongly inhibited by the addition of large amounts of KCl and KBr to micellar solutions of CTACl and CTABr, respectively. These rate effects fit the pseudophase-ion exchange model, assuming the binding of the substrates to the micelles depends upon the counterion concentration. Keywords: counterion micellar effects, low-spin diimine iron(II) complexes.

Ion exchange in micellar solutions. 7. Effect of detergent structure on the binding and reactivity of hydroxide in cationic micellar solutions

1982 ◽  
Vol 86 (25) ◽  
pp. 4941-4947 ◽  
Author(s):  
Joao B. S. Bonilha ◽  
Glaico Chiericato ◽  
Sandra M. Martins-Franchetti ◽  
Edson J. Ribaldo ◽  
Frank H. Quina
Keyword(s):  
Ion Exchange ◽  
Micellar Solutions

The Origin of Reversible Hydroxide Uptake on Reservoir Rock

1985 ◽  
Vol 25 (05) ◽  
pp. 711-718 ◽  
Author(s):  
A.L. Bunge ◽  
C.J. Radke
Keyword(s):  
Ion Exchange ◽  
Oil Recovery ◽  
Hydrogen Exchange ◽  
Weak Acid ◽  
Ion Uptake ◽  
Mass Action ◽  
Hydroxide Ion ◽  
Sodium Hydrogen ◽  
Simple Mass ◽  
Sodium Exchange

Abstract When reservoir solids reversibly consume hydroxide, the impact on alkaline-waterflood performance can be significant. Only recently has this reaction been recognized as a principal factor influencing oil recovery rates and chemical-pulse depletion. This paper considers the origin of the reversible hydroxide uptake to be ion exchange of sodium for hydrogen ions. Using a simple, mass-action equilibrium model, we describe the alkali exchange isotherm. Because hydronium and hydroxide concentrations in water are never zero, hydroxide uptake must be reported relative to a reference pH and salinity. With the recognition of a reference state pH and salinity. With the recognition of a reference state and with the mass-action model, we predict qualitatively the effects of pH, salt concentration, and temperature on the measured hydroxide uptake isotherms for the Wilmington, Ranger-zone sand. Mineral sites that exchange ions of sodium for hydrogen may also exchange calcium for hydrogen or for sodium. Using simple mass-action equilibria again, we demonstrate that reversible hydroxide uptake depends on hardness concentration and that calcium/sodium exchange is pH dependent. Introduction Alkaline flooding is a technique in which chemical interactions with reservoir minerals are of paramount importance to success or failure. Hydroxide consumption falls into three broad categories:reversible rock adsorption or ion exchange,congruent and incongruent mineral dissolution, andprecipitation of insoluble hydroxides. All three loss mechanisms have been considered in various levels of detail. Reversible hydroxide ion uptake, which was overlooked in earlier work on alkali/rock interactions, is, perhaps, the least transparent consumption reaction. Its perhaps, the least transparent consumption reaction. Its existence and importance have come to light only recently. In modeling the alkaline oil recovery process, de Zabala et al. point out that equilibrium hydroxide ion uptake causes a chromographic lag in caustic and in the accompanying in-situ generated surfactants, which in turn slows oil-production rates. Likewise, Bunge and Radke demonstrate that hydroxide ion uptake alone can diminish an alkaline chemical pulse to ineffective concentration levels. Thus, even if caustic consumption by dissolution and precipitation could be eliminated, ion-exchange delay can precipitation could be eliminated, ion-exchange delay can limit the success of alkaline EOR. Therefore, when a reservoir is considered for possible alkaline flooding, understanding and quantifying any alkali/rock ion exchange is necessary. This paper presents a simple, mass-action treatment of reversible hydroxide ion uptake by sodium/hydrogen ion exchange followed by a reaction to form or dissociate water. We refer to this overall reaction scheme as hydroxide uptake, or reversible hydroxide consumption. By using the mass-action model and by paying careful attention to the measurement of alkali exchange isotherms, we show how the effects of pH, salt content, and temperature on the hydroxide uptake isotherms may be explained. The relationship between sodium/hydrogen exchange and calcium/sodium exchange is also explored. We demonstrate that calcium/sodium exchange is a combination of sodium/hydrogen and calcium/hydrogen exchange. Therefore, calcium/sodium exchange isotherms generally must be a function of pH, and hydroxide exchange isotherms must depend on calcium concentration. Finally, the connection between the hydrogen exchange capacity (HEC) and the calcium exchange capacity (CEC) is elucidated. Sodium/Hydrogen Exchange Fig. 1 gives the reversible hydroxide uptake on Wilmington, Ranger-zone sand as a function of hydroxide concentration at three temperatures with and without NaCl. Although there is considerable scatter in the data and few points at the lower pH values, the uptake isotherms appear Langmuir in shape. Also, alkali exchange increases with increasing temperature but decreases when salt is added. Reversible alkali exchange occurs not only with the unconsolidated reservoir materials shown here but also on consolidated Berea sandstone. To quantify the behavior of reversible surface uptake of hydroxide ions on reservoir minerals, we adopt our previous. ture of weak-acid sodium/hydrogen cation previous. ture of weak-acid sodium/hydrogen cation exchange: MOH+Na+ + MONa+H+................... (1) where M represents a mineral exchange site. For oxides (such as silica) MOH denotes a hydrolyzable acid site, while for clay minerals (such as kaolinite or montmorillonite MOH denotes a negative lattice exchange site occupied by a hydronium ion. SPEJ P. 711

scholarly journals Poly(bis-arylimidazoliums) possessing high hydroxide ion exchange capacity and high alkaline stability

2019 ◽  
Vol 10 (1) ◽  
Author(s):  
Jiantao Fan ◽  
Sapir Willdorf-Cohen ◽  
Eric M. Schibli ◽  
Zoe Paula ◽  
Wei Li ◽  
...  
Keyword(s):  
Ion Exchange ◽  
Exchange Capacity ◽  
Ion Exchange Capacity ◽  
Hydroxide Ion ◽  
Alkaline Stability

Ion exchange in micellar solutions. 4. "Buffered" systems

1980 ◽  
Vol 84 (4) ◽  
pp. 361-365 ◽  
Author(s):  
Frank H. Quina ◽  
Mario J. Politi ◽  
Iolanda M. Cuccovia ◽  
Elisa Baumgarten ◽  
Sandra M. Martins-Franchetti ◽  
...  
Keyword(s):  
Ion Exchange ◽  
Micellar Solutions
Sign in / Sign up

Export Citation Format

Share Document