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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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Common Ion Effect03:24

Common Ion Effect

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Compared with pure water, the solubility of an ionic compound is less in aqueous solutions containing a common ion (one also produced by dissolution of the ionic compound). This is an example of a phenomenon known as the common ion effect, which is a consequence of the law of mass action that may be explained using Le Châtelier’s principle. Consider the dissolution of silver iodide:
34.2K
Electrolytes: van't Hoff Factor03:08

Electrolytes: van't Hoff Factor

31.0K
Colligative Properties of ElectrolytesThe 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 dissolved...
31.0K
Chemical Equilibria: Redefining Equilibrium Constant01:20

Chemical Equilibria: Redefining Equilibrium Constant

1.5K
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.
To calculate the equilibrium constants of solutions of moderately high ionic strength, one must account for the salt effect. This redefined...
1.5K
Formation of Complex Ions03:45

Formation of Complex Ions

18.8K
A type of Lewis acid-base chemistry involves the formation of a complex ion (or a coordination complex) comprising a central atom, typically a transition metal cation, surrounded by ions or molecules called ligands. These ligands can be neutral molecules like H2O or NH3, or ions such as CN− or OH−. Often, the ligands act as Lewis bases, donating a pair of electrons to the central atom. These types of Lewis acid-base reactions are examples of a broad subdiscipline called coordination...
18.8K
Determining the pH of Salt Solutions04:08

Determining the pH of Salt Solutions

41.4K
The pH of a salt solution is determined by its component anions and cations. Salts that contain pH-neutral anions and the hydronium ion-producing cations form a solution with a pH less than 7. For example, in ammonium nitrate (NH4NO3) solution, NO3− ions do not react with water whereas NH4+ ions produce the hydronium ions resulting in the acidic solution. In contrast, salts that contain pH-neutral cations and the hydroxide ion-producing anions form a solution with a pH greater than 7.
41.4K

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Controlling the Size, Shape and Stability of Supramolecular Polymers in Water
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Specific cation effects on hemoglobin aggregation below and at physiological salt concentration.

Luca Medda1, Cristina Carucci, Drew F Parsons

  • 1Department of Chemical and Geological Sciences, University of Cagliari-CSGI and CNBS, Cittadella Universitaria , S.S. 554 bivio Sestu, 09042 Monserrato (CA), Italy.

Langmuir : the ACS Journal of Surfaces and Colloids
|November 22, 2013
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Summary
This summary is machine-generated.

Ion specific effects on hemoglobin aggregation were studied. Different salt concentrations altered cation binding preferences, explained by electrostatic and dispersion forces, impacting biological systems.

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Area of Science:

  • Biochemistry
  • Physical Chemistry
  • Protein Science

Background:

  • Hemoglobin (Hb) aggregation is influenced by ion concentration and pH.
  • Understanding ion-specific interactions is crucial for biological systems.

Purpose of the Study:

  • To investigate ion-specific aggregation of hemoglobin (Hb) across varying salt concentrations and pH.
  • To elucidate the mechanisms behind observed cation series in Hb aggregation.

Main Methods:

  • Turbidity titrations were employed to monitor Hb aggregation.
  • Experiments were conducted in the pH range of 4.5-9.5.
  • Ion-specific effects were analyzed at 50 mM and 150 mM salt concentrations.

Main Results:

  • Cation-induced Hb aggregation order varied with salt concentration (e.g., Rb(+) > K(+) ~ Na(+) > Cs(+) > Li(+) at 50 mM; K(+) > Rb(+) > Na(+) > Li(+) > Cs(+) at 150 mM).
  • A model incorporating nonelectrostatic forces (dispersion) alongside electrostatic interactions explained ion binding.
  • Kosmotropic and chaotropic ion behaviors were rationalized by binding to specific protein sites (carboxylates, uncharged patches).

Conclusions:

  • Ion-specific nonelectrostatic forces, including dispersion, are key to understanding hemoglobin aggregation.
  • The law of matching water affinities (LMWA) and ion binding to uncharged patches are explained by combined electrostatic and dispersion forces.
  • These findings have broader implications for ion-specific effects in various biological systems beyond hemoglobin.