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Ionic Strength: Effects on Chemical Equilibria01:19

Ionic Strength: Effects on Chemical Equilibria

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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.
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The effect of an inert salt on the solubility of a sparingly soluble salt is known as the salt effect. The degree of the salt effect varies with the ionic strength of the solution, which in turn depends on the activity of the species in the solution. The activity is expressed as the product of concentration and the activity coefficient of the species.
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When a substance such as sodium chloride is added to water, it dissolves, forming an aqueous solution. The extent of dissolution is called solubility. The process of dissolution can exist in equilibrium, just like other chemical processes. Solubility equilibria are also called precipitation equilibria because the process of solubility can be reversible. The reverse of the solubility process is called precipitation.
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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.
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Ionic Strength: Overview01:12

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The ionic strength of a solution is a quantitative way of expressing the total electrolyte concentration of a solution. This concept was first introduced in 1921 by two American physical chemists, Gilbert N. Lewis and Merle Randall, while describing the activity coefficient of strong electrolytes. During the calculation of ionic strength (I or μ), all the cations and anions are considered. However, the concentration (c) of an ion with a greater charge number (z) has a greater contribution...
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Colligative Properties of Electrolytes
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Analyzing the concentration-dependent Soret coefficient minimum in salt solutions: an overview.

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Temperature gradients drive thermodiffusion, separating liquid mixture components. This study reveals Onsager coefficients, not thermodynamic factors, primarily cause non-monotonic Soret coefficients in aqueous salt solutions.

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Area of Science:

  • Physical Chemistry
  • Chemical Thermodynamics
  • Solution Chemistry

Background:

  • Temperature gradients induce thermodiffusion, a phenomenon quantified by the Soret coefficient.
  • Recent studies indicate non-monotonic behavior (minima) in the Soret coefficient versus concentration for aqueous salt solutions.

Purpose of the Study:

  • To analyze Soret coefficient data for ten 1:1 electrolytes in water and newly measured data for aqueous cesium iodide.
  • To investigate the factors contributing to the non-monotonic behavior of the Soret coefficient.

Main Methods:

  • Experimental measurement of Soret coefficients for aqueous cesium iodide using thermal diffusion forced Rayleigh scattering (TDFRS).
  • Analysis of existing and new Soret coefficient data by decomposing them into thermodynamic and Onsager coefficient factors.
  • Temperature range: 15-45 °C; Concentration range: 0.5-3 mol/kg.

Main Results:

  • The ratio of Onsager coefficients is identified as the primary driver of non-monotonic Soret coefficient behavior.
  • This finding contrasts with recent computer simulation results for binary Lennard-Jones mixtures.
  • For salts with identical anions, thermodynamic factors correlate with cation Pauling radii, while Onsager ratios correlate with hydrated cation radii.

Conclusions:

  • The non-monotonicity of Soret coefficients in aqueous salt solutions is mainly attributed to the behavior of Onsager coefficients.
  • The study provides insights into the interplay between ionic size, hydration, and thermodiffusive transport in electrolyte solutions.