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Related Concept Videos

Aqueous Solutions and Heats of Hydration02:42

Aqueous Solutions and Heats of Hydration

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...
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.
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Solubility03:00

Solubility

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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Hydration of cement is a chemical reaction between cement particles and water. This process occurs primarily through two mechanisms: through-solution and topochemical. In the through-solution process, anhydrous compounds dissolve into their constituents, hydrates form in the solution, and then precipitate from the supersaturated solution. The topochemical process involves solid-state reactions at the cement particle surface. The through-solution process dominates the topochemical process at the...
Ionic Strength: Effects on Chemical Equilibria01:19

Ionic Strength: Effects on Chemical Equilibria

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 cation—the calcium...
Solubility Equilibria: Overview01:09

Solubility Equilibria: Overview

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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Preparing Silica Aerogel Monoliths via a Rapid Supercritical Extraction Method
06:54

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Published on: February 28, 2014

Potassium-hydrated silicate solution unfreezable down to 190 K.

Mikio Fukuhara1, Akiyoshi Kokuta

  • 1Institute for Materials Research, Tohoku University, Aoba, Sendai 980-8577, Japan. a80010@tungaloy

Cryo Letters
|October 16, 2009
PubMed
Summary

Researchers created a potassium-hydrated silicate solution, finding a eutectic point of 190 K and a freezing point of 232 K. This solution exhibits unique properties due to hydration and structural bonding, remaining unfrozen at low temperatures.

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Area of Science:

  • Physical Chemistry
  • Materials Science
  • Solution Chemistry

Background:

  • Pure water's freezing point is theoretically 163 K without hydrogen or rotational bonds.
  • Hydrogen bonds significantly influence water's physical properties, including its freezing point.
  • Investigating solutions that resist freezing is crucial for various scientific and industrial applications.

Purpose of the Study:

  • To explore freezing point depression in a novel potassium-hydrated silicate solution.
  • To characterize the structural and thermal properties of the SiO2-KOH-H2O system.
  • To understand the mechanisms behind reduced freezing points in hydrated silicate solutions.

Main Methods:

  • Preparation of a potassium-hydrated silicate solution.
  • Thermal analysis, including differential scanning calorimetry (DSC).
  • Ultrasonic analysis and Fourier-transform infrared (FT-IR) spectroscopy.

Main Results:

  • The SiO2-KOH-H2O system exhibits a eutectic point around 190 K.
  • DSC analysis revealed a sharp exothermal peak at 232 K, indicating the freezing point.
  • FT-IR spectroscopy confirmed the presence of silanol and siloxane structures, with OH and Si-O-Si bonds.

Conclusions:

  • The silicate solution remains unfrozen down to 190 K, demonstrating significant freezing point depression.
  • Hydration and the formation of stable, irrotationally bound siloxane structures contribute to the solution's low-temperature stability.
  • These findings suggest potential applications for such solutions in environments requiring resistance to freezing.