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Related Concept Videos

Solubility of Ionic Compounds02:55

Solubility of Ionic Compounds

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.
Solubility Equilibria: Ionic Product of Water01:16

Solubility Equilibria: Ionic Product of Water

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 Chatelier's...
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Solution, Solubility, and Solubility Equilibrium
A solution is a homogeneous mixture composed of a solvent, the major component, and a solute, the minor component. The physical state of a solution—solid, liquid, or gas—is typically the same as that of the solvent. Solute concentrations are often described with qualitative terms such as dilute (of relatively low concentration) and concentrated (of relatively high concentration).
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Crystalline solids are divided into four types: molecular, ionic, metallic, and covalent network based on the type of constituent units and their interparticle interactions.
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Molecular crystalline solids, such as ice, sucrose (table sugar), and iodine, are solids that are composed of neutral molecules as their constituent units. These molecules are held together by weak intermolecular forces such as London dispersion forces, dipole-dipole interactions, or hydrogen bonds, which...
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Recrystallization: Solid–Solution Equilibria

Recrystallization is a purification technique used to separate impurities from solid compounds. In this technique, no chemical reactions occur. Instead, it exploits physical properties only, specifically, the solubility differences between the desired compound and impurities, either at a single temperature or at different temperatures, and under other selected conditions. The solid-solution equilibrium (solubility equilibrium) of each component in the solution represents a binary phase...
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Aqueous Solutions and Heats of Hydration

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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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Published on: December 20, 2016

Temperature-dependent solvatochromic probe behavior within ionic liquids and (ionic liquid + water) mixtures.

Shruti Trivedi1, Naved I Malek, Kamalakanta Behera

  • 1Department of Chemistry, Indian Institute of Technology, Delhi, Hauz Khas, New Delhi 110016, India.

The Journal of Physical Chemistry. B
|June 4, 2010
PubMed
Summary

Spectroscopic probes reveal how temperature affects physicochemical properties in ionic liquids. Key parameters like dipolarity and acidity decrease with rising temperatures, while basicity remains stable, depending on the specific probe used.

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Area of Science:

  • Physical Chemistry
  • Materials Science
  • Spectroscopy

Background:

  • Ionic liquids (ILs) are tunable solvents with unique physicochemical properties.
  • Understanding temperature-dependent solvent properties is crucial for IL applications.
  • Solvatochromic probes offer a sensitive method to probe solvent environments.

Purpose of the Study:

  • To investigate the temperature dependence of physicochemical properties in ILs and their aqueous mixtures.
  • To evaluate the behavior of various solvatochromic probes (betaine dye 33, N,N-diethyl-4-nitroaniline, 4-nitroaniline, pyrene, and pyrene-1-carboxaldehyde) within ILs.
  • To determine the influence of temperature on dipolarity, polarizability, and hydrogen bonding characteristics.

Main Methods:

  • Utilized absorbance and fluorescence spectroscopy to monitor probe responses.
  • Employed betaine dye 33 for ETN values (dipolarity/polarizability and HBD acidity).
  • Applied Kamlet-Taft parameters (pi*, alpha, beta) and probe band intensity ratios (Py) to quantify solvent properties.
  • Studied ILs: 1-butyl-3-methylimidazolium hexafluorophosphate ([bmim][PF6]) and 1-butyl-3-methylimidazolium tetrafluoroborate ([bmim][BF4]), and their aqueous mixtures.

Main Results:

  • ETN and dipolarity/polarizability (pi*) decreased linearly with increasing temperature in both ILs.
  • Hydrogen bond donating acidity (alpha) also decreased linearly with temperature, while hydrogen bond accepting basicity (beta) remained temperature-independent.
  • The first-to-third band intensity ratio of pyrene (Py) showed a linear decrease with temperature, similar to ETN and pi*.
  • Pyrene-1-carboxaldehyde (PyCHO) fluorescence maxima were insensitive to temperature changes within the ILs but sensitive in aqueous solutions.
  • Temperature dependence of dipolarity/polarizability was more pronounced in aqueous IL mixtures than in neat ILs or water.

Conclusions:

  • The temperature-dependent behavior of solvatochromic probes in [bmim][PF6], [bmim][BF4], and their aqueous mixtures is probe-specific.
  • Dipolarity and HBD acidity generally decrease with increasing temperature in these IL systems.
  • The sensitivity of solvent properties to temperature varies between neat ILs and their aqueous mixtures, with pi* sensitivity increasing upon IL addition to water.
  • PyCHO exhibits remarkable temperature insensitivity in IL environments, highlighting its utility for specific applications.