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Related Concept Videos

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.
In this solution, the primary...
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Electrolytes: van't Hoff Factor03:08

Electrolytes: van't Hoff Factor

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Colligative Properties of Electrolytes
The colligative properties of a solution depend only on the number, not on the identity, of solute species dissolved. The concentration terms in the equations for various colligative properties (freezing point depression, boiling point elevation, osmotic pressure) pertain to all solute species present in the solution. Nonelectrolytes dissolve physically without dissociation or any other accompanying process. Each molecule that dissolves yields one...
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Solubility Equilibria: Overview01:09

Solubility Equilibria: Overview

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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.
Solubility is important in biological and environmental processes. A notable...
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Ionic Strength: Overview01:12

Ionic Strength: Overview

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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...
1.6K
Factors Affecting Activity Coefficient01:17

Factors Affecting Activity Coefficient

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The extended Debye-Hückel equation indicates that the activity coefficient of an ion in an aqueous solution at 25°C depends on three partially interdependent properties: the ionic strength of the solution, the charge of the ion, and the ion size. 
The activity coefficient value for an ion is close to one when the solution has almost zero ionic strength, i.e., when the solution shows close to ideal behavior. As the ionic strength of the solution increases from 0 to 0.1 mol/L, a...
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Enthalpy of Solution02:39

Enthalpy of Solution

25.1K
There are two criteria that favor, but do not guarantee, the spontaneous formation of a solution:
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Controlling the Size, Shape and Stability of Supramolecular Polymers in Water
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Overlapping hydration shells in salt solutions causing non-monotonic Soret coefficients with varying concentration.

Shilpa Mohanakumar1, Hartmut Kriegs1, W J Briels1,2

  • 1IBI-4:Biomacromolecular Systems and Processes, Forschungszentrum Jülich GmbH, D-52428 Jülich, Germany. s.wiegand@fz-juelich.de.

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Summary

The thermodiffusive properties of iodide salt solutions show a minimum Soret coefficient (ST) at 1 mol kg-1, suggesting similar hydration scales for sodium, potassium, and lithium iodide. This behavior is linked to fully hydrated salt molecules.

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Area of Science:

  • Physical Chemistry
  • Solution Thermodynamics
  • Transport Phenomena

Background:

  • Understanding thermodiffusive properties of electrolyte solutions is crucial for various chemical processes.
  • Previous studies often focused on dilute solutions, leaving behavior in more concentrated regimes less explored.

Purpose of the Study:

  • To investigate the thermodiffusive properties of aqueous sodium iodide, potassium iodide, and lithium iodide solutions.
  • To analyze the concentration and temperature dependence of the Soret coefficient (ST) in these salt systems.

Main Methods:

  • Utilized thermal diffusion forced Rayleigh scattering (TD-FRS) for precise measurements.
  • Studied solutions across a concentration range of 0.5-4 mol kg-1 and temperatures from 15 to 45 °C.

Main Results:

  • Observed non-monotonic variations in the Soret coefficient (ST) for all three iodide salts.
  • Identified a consistent minimum in ST around 1 mol kg-1 concentration for all systems.
  • Found that length and energy scales of hydrated ions are similar across the studied salts.

Conclusions:

  • The observed minimum in ST suggests a common behavior related to the packing of fully hydrated salt molecules.
  • Preliminary models indicate ST rises as hydrated particles approach random close packing.
  • The study provides insights into salt solution behavior at higher concentrations, highlighting limitations of current models.