Electronic Conductivity of NaCl-KCl Equimolar Melt Containing Eu(III) and Eu(II) Complexes by Electrochemical Impedance Spectroscopy
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The electronic conductivity of molten equimolar NaCl-KCl containing Eu(III) and Eu(II) complexes was studied by electrochemical impedance spectroscopy. The ratio between electronic and electrolyte resistance as a function of the electrode potential was determined. The electronic conductivity was found to be maximal when the amounts of Eu(III) and Eu(II) are about equal. The electronic conductivity of this melt does not exceed 2.3% of the ionic conductivity. Deviation from the molar ratio Eu(III)/Eu(II) = 1 led to a considerable diminution of the electronic conductivity.Keywords:
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A novel kind of polymer electrolyte based on hyperbranched polyether was prepared,and its ionic conductivity was studied by electrochemical impedance spectroscopy(EIS).The results show that adding amount of lithium salt and testing temperature both have effect on ionic conductivities of the polymer electrolytes.When the content of LiCF3SO3 is 30%,the electrolyte possesses the highest ionic conductivity,which is 5.45×10-4 S/cm at 80 ℃,1.2×10-5 S/cm and room temperature.
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The study of the conductivity of electrolyte solutions is important for practical applications and for the understanding of ion mobility. Because of that, undergraduate experiments on ionic conductivity are common practice in first year general chemistry or more advanced physical chemisdegreetry laboratories. Often, the conductivities are measured for solutions prepared for various salts, in a range of concentrations, and the relationship between solution conductivity and concentration is interpreted in terms of the Kohlrausch law. Extrapolation of the molar conductivities to infinite dilution allows the study of the individual ionic conductivities. In practice, the preparation of dilute solutions for these experiments can be cumbersome, because small electrolyte contaminations can dominate the conductivity of the solutions. Additionally, significant amounts of reactants, particularly deionized water, must be used. Here, a simple experimental procedure is proposed to obtain the concentration dependence of ionic conductivities for very dilute (sub-millimolar) electrolyte solutions. The experiment consists in measuring the conductivity of solutions of increasing concentration prepared by dropping the electrolyte solution into a single initial vessel of deionized water. The range of concentrations achieved is one in which the conductivities vary linearly with the concentrations, such that the molar conductivities can be obtained directly without the use of the Kohlrausch equation. The simplicity of the experimental procedure leads the students to obtain very good quality results using minimal amounts of materials. Examples are presented for the conductivities of various strong electrolytes, and for weak acetic acid electrolyte, for which the conductivity is dependent on the degree of dissociation even at very low concentrations
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Li₂SO₄–polyacryalamide (PAM) neutral pH polymer electrolytes with different salt:polymer molar ratios (5000:1 and 10000:1) were characterized for their ionic conductivity and material properties. Their ionic conductivity over time showed different trends: Li₂SO₄–PAM(5000:1) increased while Li₂SO₄–PAM(10000:1) decreased. Materials characterizations of the freestanding films were conducted to identify the cause of the difference in conductivity trends. X-ray diffraction and IR spectroscopy suggested slight differences in film crystallinity and sulfate ion bonding structure, but they were not conclusive. Raman spectroscopy proved to be a better tool as it revealed distinct characteristic peaks for different sulfate ion and water interactions. To correlate the film properties with electrolyte performance, a real-time tracking technique to correlate ionic conductivity and the vibrational spectroscopic responses was developed. Leveraging this approach, the level of hydration surrounding the salt molecule was identified as the determining factor of ionic conductivity in this polymer system. This approach can be extended to predict the shelf and service life of this Li₂SO₄–PAM system and to optimize the next generations of electrolytes.
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The purpose of this study is to predict the electrical conductivity of an electrolyte solution containing several simple ionic species. Explicit equations of the MSA-transport theory for the electrical conductivity in this complex solution are given. The theoretical conductivity of simple salts is first compared to experimental results of the literature to deduce the sizes of the ions. These sizes allow us to calculate the conductivity for a mixture of several ionic species without any additional parameter. We have also measured the electrical conductivity of solutions of LiCl, NaCl, and KCl and of KBr and MgCl(2) at 25 degrees C. A very good agreement between theoretical calculations and experimental values is obtained for each studied system.
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The study conductivity of electrolyte solutions is important for practical applications and for the understanding of ion mobility. Because of that, undergraduate experiments on ionic conductivity are common practice in first year general chemistry or more advanced physical chemistry laboratories.Often, the conductivities are measured for solutions prepared for various salts, in a range of concentrations, and the relationship between solution conductivity and concentration is interpreted in terms of the Kohlrausch law. Extrapolation of the molar conductivities to infinite dilution allows the study of the individual ionic conductivities. In practice, the preparation of dilute solutions for theseexperiments can be cumbersome, because small electrolyte contaminations can dominate the conductivity of the solutions. Additionally, significant amounts of reactants, particularly deionized water, must be used. Here, a simple experimental procedure is proposed to obtain the concentration dependence of ionic conductivities for very dilute (sub-millimolar) electrolyte solutions. The experimentconsists in measuring the conductivity of solutions of increasing concentration prepared by dropping the electrolyte solution into a single initial vessel of deionized water. The range of concentrations achieved is one in which the conductivities vary linearly with the concentrations, such that the molar conductivities can be obtained directly without the use of the Kohlrausch equation. The simplicity of the experimental procedure leads the students to obtain very good quality results using minimal amounts of materials. Examples are presented for the conductivities of various strong electrolytes, and for the weak acetic acid electrolyte, for which the conductivity is dependent on the dissociation rate even at very low concentrations.
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This chapter contains sections titled: Dissociation of Electrolytes and Electrolytic Conductivity Molar Conductivity of Dilute Solutions of Symmetrical Strong Electrolytes Molar Conductivity and Association Constants of Symmetrical Weak Electrolytes Molar Conductivity and the Formation of Triple Ions Conductivity of Solutions of Symmetrical Strong Electrolytes at Moderate to High Concentrations Molar Conductivity and Ion Association of Asymmetric Electrolytes Ionic Conductivities and Solvents Stokes' Law and Walden's Rule – Role of Ultrafast Solvent Dynamics Method for the Determination of Limiting Molar Conductivities of Ions Applications of Conductimetry in Non-Aqueous Solutions Study of the Behavior of Electrolytes (Ionophores) Conductimetric Studies of Acid-Base Equilibria
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In an attempt to be developed as a electrolyte material for solid oxide fuel cells,AC impedance spectroscopy was employed to study the bulk conductivity of(Gd2O3)x(ZrO2)1-x(x=0.05-0.15) electrolytes.The ionic dynamic behaviors of Gd2O3 doped ZrO2 solid electrolytes were also investigated by molecular dynamics simulation.The effect of temperature and Gd2O3 dopant content on the conductivity of materials were simulated and calculated.The results from both experiments and simulations showed that the ionic conductivity was enhanced by ramping temperature,while 8 mol% of Gd2O3 doping concentration tends to have the optimal ionic conductivity.
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This study was aimed at providing information on the effects brought on by hypotonicity and supporting electrolytes on ionic strength and conductivity of physiological solutions. Isotonic and 50% hypotonic solutions of chloride and chloride+sulphate salts were prepared, taking into account their molecular weight and osmotic concentration. Their specific conductivity and molar conductivity were measured at 25°C using a pH/conductivity meter. There was a decrease in specific and molar conductivity of all the electrolyte studied as a result of 50% hypotonicity except for CaCl 2+CaSO4 solution. Tonicity had more effect on the molar conductivity of week electrolytes. The addition of supporting electrolyte resulted in an increase in the calculated ionic strength and molar conductivity. It also resulted in an increase in the specific conductivity of the resultant supported solutions except CaCl2+CaSO4 and MgCl2+MgSO4 solutions. The relative ionic strengths of the electrolytes could not be determined from their specific conductivity because the contribution of multivalent supporting electrolyte ions to ionic concentration is not evident in the specific conductivity of the resultant solutions.
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