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Solubility of Ionic Compounds02:55

Solubility of Ionic Compounds

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Solubility is the measure of the maximum amount of solute that can be dissolved in a given quantity of solvent at a given temperature and pressure. Solubility is usually measured in molarity (M) or moles per liter (mol/L). A compound is termed soluble if it dissolves in water.
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Solubility Equilibria: Ionic Product of Water01:16

Solubility Equilibria: Ionic Product of Water

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Pure water is a weak electrolyte; only a small amount ionizes into hydrogen and hydroxide ions. At any given temperature, the concentration of undissociated water is almost constant, so the ionic product of water is the product of the hydrogen and hydroxide ion concentrations, denoted as Kw. The square root of Kw gives the individual ion concentrations.
The ionic product of water varies with temperature, and its value is 1.0 x 10−14 at standard experimental conditions. Per Le...
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Solvents01:12

Solvents

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A solvent is a substance, most often a liquid, that can dissolve other substances. Here, the substance being dissolved is called a solute. When a solvent and a solute combine, they form a solution - a homogenous mixture of both the solvent and the solute. Water is a universal biological solvent. Its polar structure allows it to dissolve many other polar compounds. The ability of water to dissolve is governed by a balance between water molecules binding to each other and binding to the solute.
A...
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Intermolecular Forces03:13

Intermolecular Forces

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Atoms and molecules interact through bonds (or forces): intramolecular and intermolecular. The forces are electrostatic as they arise from interactions (attractive or repulsive) between charged species (permanent, partial, or temporary charges) and exist with varying strengths between ions, polar, nonpolar, and neutral molecules. The different types of intermolecular forces are ion–dipole, dipole–dipole, hydrogen bonds, and dispersion; among these, dipole–dipole, hydrogen...
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Aqueous Solutions and Heats of Hydration02:42

Aqueous Solutions and Heats of Hydration

19.1K
Water and other polar molecules are attracted to ions. The electrostatic attraction between an ion and a molecule with a dipole is called an ion-dipole attraction. These attractions play an important role in the dissolution of ionic compounds in water.
When ionic compounds dissolve in water, the ions in the solid separate and disperse uniformly throughout the solution because water molecules surround and solvate the ions, reducing the strong electrostatic forces between them. This process...
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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.
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Synthesis of Ionic Liquid Based Electrolytes, Assembly of Li-ion Batteries, and Measurements of Performance at High Temperature
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Water in Solvate Ionic Liquids: Preserving Lithium Coordination While Enhancing Ionic Conductivity.

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Summary
This summary is machine-generated.

Hybrid electrolytes combine solvate ionic liquids (SILs) and water-in-salt (WIS) concepts. Adding water to SILs significantly improves conductivity and reduces viscosity, creating water-in-solvate-ionic-liquid (WISIL) systems with stable electrochemical windows.

Keywords:
cluster formationmolecular dynamics simulationssolvate ionic liquidstructurewater‐in‐salt electrolyte

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Area of Science:

  • Electrochemistry
  • Materials Science
  • Computational Chemistry

Background:

  • Solvate ionic liquids (SILs) offer unique properties but often suffer from high viscosity.
  • Water-in-salt (WIS) electrolytes demonstrate enhanced ionic conductivity.
  • Combining SILs and WIS concepts could lead to advanced electrolyte materials.

Purpose of the Study:

  • To investigate the creation of hybrid electrolyte systems by merging SILs and WIS electrolytes.
  • To explore the effects of water addition on the properties of a specific SIL, [Li(G3)][NTf2].
  • To characterize the structure and electrochemical performance of the resulting hybrid systems.

Main Methods:

  • Molecular dynamics simulations were employed to model electrolyte behavior.
  • Experimental techniques were used to validate simulation findings.
  • Electrochemical measurements assessed conductivity and stability.

Main Results:

  • The addition of equimolar water to the neat SIL [Li(G3)][NTf2] significantly reduced viscosity and increased ionic conductivity.
  • Water molecules were found to be individually incorporated into cationic complexes, preventing water network formation.
  • The resulting water-in-solvate-ionic-liquid (WISIL) electrolytes maintained a wide electrochemical stability window (4.9 V).

Conclusions:

  • Hybrid WISIL electrolytes offer a promising route to overcome the limitations of neat SILs.
  • These electrolytes exhibit improved transport properties and maintain excellent electrochemical stability.
  • WISIL electrolytes represent a new class of advanced materials for electrochemical applications.