1 edition of Thermodynamics of strong electrolytes in protium-deuterium oxide mixtures found in the catalog.
Thermodynamics of strong electrolytes in protium-deuterium oxide mixtures
Evan Carter Noonan
in New York city
Written in English
|Statement||by Evan Carter Noonan and Victor K. La Mer ...|
|Contributions||La Mer, Victor K. (Victor Kuhn), 1895-1966, joint author|
|LC Classifications||QD561 .N68 1939|
|The Physical Object|
|Pagination||1 p. l., p. 247-258 1 l. incl. 1 illus., tables, 2 diagr.|
|Number of Pages||258|
|LC Control Number||40009493|
In book: Thermodynamics in Earth and Planetary Sciences, pp deals with thermodynamics of electrolyte solutions with applications to low temperature geochemical problems, such as Author: Jibamitra Ganguly. Chemical Thermodynamics - Electrolyte Activity TMP Chem. The activity coefficient of electrolytes deviates from 1 at very low concentrations due to the strong interactions of charged ions.
The full text of this article hosted at is unavailable due to technical difficulties. Evan Carter Noonan has written: 'Thermodynamics of strong electrolytes in protium-deuterium oxide mixtures' -- subject(s): Hydrochloric acid, Protium oxide, Deuterium oxide, Electrolytes .
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Thermodynamics of Strong Electrolytes in Protium--Deuterium Oxide Mixtures II. Potassium Chloride. Protonation of nitroalkane anions by acetic acid in mixed water-deuterium oxide solvents. Journal of the American Chemical Society90 (2), DOI: /jaaCited by: 7.
Application of A Short-Range Ordered Model to Strong Electrolytes. , DOI: /ch Mustafa Sabri Kilic, Martin Z. Bazant, Armand Ajdari. Steric effects in the dynamics of electrolytes at large applied voltages.
Double-layer charging. Thermodynamics of Strong Electrolytes in Protium--Deuterium Oxide Mixtures II. Potassium Chloride The Properties of Electrolytes in Mixtures of Water and Organic Solvents. Hydrochloric Acid in Ethanol-- and Isopropanol--Water Mixtures of High Dielectric Constant. Herbert S.
Harned; Calvin. Calmon; Journal of the American Chemical. Comparison among Pitzer-type Models for the Osmotic and Activity Coefficients of Strong Electrolyte Solutions at K. Industrial & Engineering Chemistry Research50 (18), DOI: / by: The standard change of free energy; the equilibrium constant.
Solutions of electrolytes. The activity of strong electrolytes. The activity of electrolytes from freezing point data, and tables of activity coefficients. Activity coefficient in mixed electrolytes; the principle of the ionic strength; the activity of individual ions.
The galvanic cell. The temperature dependence of the parameters for symmetrical mixing of ions of the same sign in the virial-coefficient (Pitzer) system are evaluated from literature data on heats of mixing in the presence of a common ion for 20 systems.
The higher-order limiting law for symmetrical mixing is used in the form of an expression for the ionic strength dependence Thermodynamics of strong electrolytes in protium-deuterium oxide mixtures book Cited by: Mineral solubilities in binary and ternary electrolyte mixtures in the system Na-K-Mg-Cl-SO 4-OH-H 2 O are calculated to high temperatures using available thermodynamic data for solids and for aqueous electrolyte solutions.
Activity and osmotic coefficients are derived from the ion-interaction model of Pitzer (, ) and co-workers, the parameters of which are Cited by: Molar excess volumes, VEijk and molar excess enthalpies, HEijk data have been measured at K for benzene (i) + toluene, o-xylene or p-xylene (j) Cited by: 6.
Thermochimica Acta, 87 () 59 Elsevier Science Publishers B.V., Amsterdam -Printed in The Netherlands THERMODYNAMICS OF TERNARY MIXTURES OF NON ELECTROLYTES: MOLAR EXCESS ENTHALPIES R.K. NIGAM, SADHNA AGGARWAL and S.P.
SHARMA Department of Chemistry, Maharshi Dayanand University, Rohtak (India) (Received 2 Cited by: 2. Solution phase thermodynamics of strong electrolytes based on ionic concentrations, hydration numbers and volumes of dissolved entities Solution thermodynamics Aqueous electrolytes Notes on hydration theory in book.
In: Butler JN (ed) Ionic equilibrium. Wiley, New York, pp – Google Scholar. by: 5. The MSA was first introduced by Percus and Yevick  as an approximate way of introducing hard-core effects on the distribution of chargedWaisman and Lebowitz applied this approximation to electrolytes .They obtained the solution to the Ornstein-Zernike equation  in the case of ions having the same diameter, in the primitive model of solutions in.
Heavy water is also known as deuterium oxide. It is a form of water that contains a larger than normal amount of the hydrogen isotope deuterium. Heavy water contains elements such as hydrogen, oxygen, as well as uranium.
The enthalpies of mixing of a variety of aqueous electrolytes at an ionic strength of molkg −1 have been measured at K. The mixtures studied were LiBr + KBr, NaBr + KBr, KBr + (C 4 H 9) 4 NBr, NaCl + Na 2 SO 4, NaCl + MgCl 2, MgSO 4 + Na 2 SO 4, MgCl 2 + MgSO 4, NaCl + MgSO 4, and MgCl 2 + Na 2 SO contrast to most previous enthalpies of mixing of Cited by: 9.
Thermodynamic Properties of Strong Electrolytes in Aqueous Solutions A generalized analytic correlation is presented for activity coefficient. osmotic coefficient, enthalpy, and heat capacity of single and multicom- ponent strong aqueous solutions.
A good correlation for each salt to an. However, combined with CP and a measurements it gives - (aVE/aP)T which is predicted by the Prigogine-Flory Theory. The Prigogine-Flory theory Background The interplay between experiment and simple theory is probably the most attractive feature of the thermodynamics of non-electrolyte by: Handbook of aqueous electrolyte thermodynamics: theory & application.
Expertise in electrolyte systems has become increasingly important in traditional chemical process industry operations, as well as in oil/gas exploration and production.
In particular, electrolyte systems come into play in many important applications involving the environment. Electrolyte Solutions In the last few chapters of this book, we will deal with several speci c types of chemical systems. The rst one is solutions and equilibria involving electrolytes, which we will take up in this chapter.
The thermodynamics of electrolyte so-lutions is important for a large number of chemical systems, such as acid-baseFile Size: KB. Classical Thermodynamics of Non-Electrolyte Solutions covers the historical development of classical thermodynamics that concerns the properties of vapor and liquid solutions of non-electrolytes.
Classical thermodynamics is a network of equations, developed through the formal logic of mathematics from a very few fundamental postulates and Book Edition: 1. Protium, deuterium, and tritium are all isotopes of hydrogen (H). As far as their masses: Tritium>Deuterium>Protium In their nuclei: Protium has 1 proton and 0 neutrons Deuterium has 1 proton and 1 neutron Tritium has 1 proton and 2 neutrons So yes, Deuterium is heavier than tritium.
Thermodynamics of Electrolyte Mixtures: HCl + NdCl3 + H2O from 5 to 55 ∘C Thermodynamics of electrolytes. II. Activity and osmotic coefficients for strong electrolytes with one or both ions. The contribution of higher-order electrostatic terms (beyond the Debye-Hückel approximation) to the thermodynamic properties of mixed and pure electrolytes is investigated.
It is found that these effects are important for cases of unsymmetrical mixing, especially when one ion has a charge of three units or more.
The appropriate correction can be made by a purely Cited by: Deuterium is the isotope of hydrogen with a nucleus of one proton and one neutron.
It occurs naturally in water to a small concentration. The main use at present is as heavy water, which is deuterium oxide (equivalent to H2O), which is used as a moderator in heavy water reactors, like the CANDU type.