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Mechanisms of the viscosity decrease and increase of aqueous CsCl.

Max Moncada Cohen1, Laura Kacenauskaite1,2, Tristan R Heck1

  • 1Department of Chemistry, Stanford University, Stanford, CA 94305.

Proceedings of the National Academy of Sciences of the United States of America
|January 9, 2026
PubMed
Summary
This summary is machine-generated.

Cesium chloride (CsCl) initially lowers water viscosity by weakening hydrogen bonds. At high concentrations, water clusters form, slowing dynamics and increasing viscosity.

Keywords:
cesium chloridehydrogen bondingsalt solutionsultrafast dynamicsviscosity

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Area of Science:

  • Physical Chemistry
  • Chemical Physics
  • Geochemistry

Background:

  • Aqueous salt solutions are ubiquitous in science.
  • Most salts increase solution viscosity with concentration.
  • Cesium chloride (CsCl) exhibits unusual viscosity behavior, decreasing then increasing with concentration, with underlying mechanisms unclear.

Purpose of the Study:

  • To elucidate the molecular mechanisms behind CsCl's unique viscosity effects in water.
  • To investigate the impact of Cs+ ions on water dynamics, interactions, and structure.

Main Methods:

  • Ultrafast optical heterodyne-detected optical Kerr effect (OHD-OKE).
  • Infrared (IR) pump-probe spectroscopy using HOD in H2O.
  • Density functional theory (DFT) calculations.

Main Results:

  • OHD-OKE revealed water hydrogen bond (H-bond) network dynamics govern CsCl solution viscosity.
  • IR spectra showed Cs+ weakens water H-bonds, unlike high-density cations (e.g., Na+, Li+).
  • Weakened H-bonds in the Cs+ second solvation shell accelerate dynamics, reducing viscosity at low concentrations. At high concentrations, water clustering slows dynamics, increasing viscosity.

Conclusions:

  • Cs+ ions uniquely interact with water, weakening H-bonds due to low charge density.
  • The concentration-dependent viscosity of CsCl solutions arises from competing effects on water H-bond dynamics and structure.
  • Understanding these ion-specific effects is crucial for aqueous solution chemistry, biology, and geology.