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Related Concept Videos

Ionic Strength: Effects on Chemical Equilibria01:19

Ionic Strength: Effects on Chemical Equilibria

1.6K
The addition of an inert ionic compound increases the solubility of a sparingly soluble salt. For example, adding potassium nitrate to a saturated solution of calcium sulfate significantly enhances the solubility of calcium sulfate. Le Châtelier's principle cannot predict this shift in the equilibrium. Instead, this could be explained in terms of changes in the effective concentration of the ions in solution in the presence of added inert salt.
In this solution, the primary...
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Preparation and Reactions of Sulfides02:26

Preparation and Reactions of Sulfides

5.0K
Sulfides are the sulfur analog of ethers, just as thiols are the sulfur analog of alcohol. Like ethers, sulfides also consist of two hydrocarbon groups bonded to the central sulfur atom. Depending upon the type of groups present, sulfides can be symmetrical or asymmetrical. Symmetrical sulfides can be prepared via an SN2 reaction between 2 equivalents of an alkyl halide and one equivalent of sodium sulfide.
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Common Ion Effect03:24

Common Ion Effect

41.9K
Compared with pure water, the solubility of an ionic compound is less in aqueous solutions containing a common ion (one also produced by dissolution of the ionic compound). This is an example of a phenomenon known as the common ion effect, which is a consequence of the law of mass action that may be explained using Le Châtelier’s principle. Consider the dissolution of silver iodide:
41.9K
Electrolyte and Nonelectrolyte Solutions02:21

Electrolyte and Nonelectrolyte Solutions

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Substances that undergo either a physical or a chemical change in solution to yield ions that can conduct electricity are called electrolytes. If a substance yields ions in solution, that is, if the compound undergoes 100% dissociation, then the substance is a strong electrolyte. Complete dissociation is indicated by a single forward arrow. For example, water-soluble ionic compounds like sodium chloride dissociate into sodium cations and chloride anions in aqueous solution.
63.4K
Electrolysis03:00

Electrolysis

27.0K
In a galvanic cell, the electrical work is done by a redox system on its surroundings as electrons produced by the spontaneous redox reactions are transferred through an external circuit. Alternatively, an external circuit does work on a redox system by imposing a voltage sufficient to drive an otherwise nonspontaneous reaction in a process known as electrolysis. For instance, recharging a battery involves the use of an external power source to drive the spontaneous (discharge) cell reaction in...
27.0K
Factors Affecting Solubility04:01

Factors Affecting Solubility

33.6K
Compared with pure water, the solubility of an ionic compound is less in aqueous solutions containing a common ion (one also produced by dissolution of the ionic compound). This is an example of a phenomenon known as the common ion effect, which is a consequence of the law of mass action that may be explained using Le Chȃtelier’s principle. Consider the dissolution of silver iodide:
33.6K

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Dimethyl sulfoxide as a function additive on halogen-free electrolyte for magnesium battery application.

R Gamal1, E Sheha2, M M El Kholy3,4

  • 1Physics Department, Belbeis High Institute of Engineering (BHIE) Belbeis Sharqia.

RSC Advances
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Summary

This study introduces a new halogen-free electrolyte for magnesium batteries, using dimethyl sulfoxide to improve magnesium anode performance and stability for better energy storage solutions.

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Area of Science:

  • Electrochemistry
  • Materials Science
  • Energy Storage

Background:

  • Practical magnesium (Mg) batteries face challenges including incompatible electrolytes, self-discharge, Mg anode passivation, and slow reaction kinetics.
  • Developing stable and efficient electrolytes is crucial for advancing Mg battery technology.
  • Current electrolytes often struggle with Mg anode stability and ion transport.

Purpose of the Study:

  • To develop a simple, halogen-free electrolyte (HFE) for magnesium batteries.
  • To investigate the effect of dimethyl sulfoxide (DMSO) as an additive on electrolyte properties and Mg anode behavior.
  • To enhance the performance and stability of Mg batteries.

Main Methods:

  • Formulation of a new halogen-free electrolyte (HFE) using magnesium nitrate, magnesium triflate, succinonitrile, and acetonitrile/tetraethylene glycol dimethyl ether cosolvents.
  • Inclusion of dimethyl sulfoxide (DMSO) as a functional additive.
  • Electrochemical characterization including conductivity, ionic transference number, oxidation stability, and Mg stripping/plating tests; postmortem analysis of Mg anodes.

Main Results:

  • The HFE with 0.75 ml DMSO exhibited high ionic conductivity (up to 9.41 × 10-5 S cm-1) and a high Mg ion transference number (0.91/0.94).
  • The electrolyte demonstrated high oxidation stability, low overpotential, and stable Mg stripping/plating for 100 hours.
  • DMSO addition modified the Mg anode/electrolyte interface, facilitating Mg ion transport and improving anode surface characteristics.

Conclusions:

  • The developed halogen-free electrolyte with DMSO additive significantly improves Mg anode interfacial properties and ion transport.
  • This electrolyte formulation shows promising potential for high-performance and stable magnesium battery applications.
  • Further optimization is expected to yield excellent cycle stability for future magnesium battery development.