saturated solution

Examples of saturated solution in the following topics:

• Solubility

  • Solubility is the relative ability of a solute (solid, liquid, or gas) to dissolve into a solvent and form a solution.
  • Solubility is the ability of a solid, liquid, or gaseous chemical substance (referred to as the solute) to dissolve in solvent (usually a liquid) and form a solution.
  • The solubility of a substance in a particular solvent is measured by the concentration of the saturated solution.
  • A solution is considered saturated when adding additional solute no longer increases the concentration of the solution.
  • Pressure has a negligible effect on the solubility of solid and liquid solutes, but it has a strong effect on solutions with gaseous solutes.

• Molar Solubility and Relative Solubility

  • Molar solubility is the number of moles of a solute that can be dissolved per liter of solution before the solution becomes saturated.
  • Molar solubility, which is directly related to the solubility product, is the number of moles of the solute that can be dissolved per liter of solution before the solution becomes saturated.
  • Once a solution is saturated, any additional solute precipitates out of the solution.
  • The solute will always move at the same fraction of the distance of the solvent as long as temperature is held constant.
  • The distance that the solute travels in a particular solvent can be used to identify the compound.

• Extremely Halophilic Archaea

  • These compatible solutes can be accumulated from the environment or synthesized.
  • The most common compatible solutes are neutral or zwitterionic, and include amino acids, sugars, polyols, betaines and ectoines, as well as derivatives of some of these compounds.
  • In the compatible solute adaptation, little or no adjustment is required of intracellular macromolecules – in fact, the compatible solutes often act as general stress protectants as well as osmoprotectants.
  • The extremely halophilic Haloarchaea require at least a 2 M salt concentration and are usually found in saturated solutions (about 36% w/v salts).

• The Common Ion Effect

  • The common ion effect describes the changes that occur with the introduction of ions to a solution containing that same ion.
  • However, if more table salt is continuously added, the solution will reach a point at which no more can be dissolved; in other words, the solution is saturated, and the table salt has effectively reached its solubility limit.
  • The amount of NaCl that could dissolve to reach the saturation point would be lowered.
  • Addition of excess ions will alter the pH of the buffer solution.
  • In the case of an an acidic buffer, the hydrogen ion concentration decreases, and the resulting solution is less acidic than a solution containing the pure weak acid.

• RBC Physiology

  • As a result, the oxygen-binding curve of hemoglobin (also called the oxygen saturation or dissociation curve) is sigmoidal, or S-shaped, as opposed to the normal hyperbolic curve associated with noncooperative binding.
  • This curve shows the saturation of oxygen bound to hemoglobin compared to the partial pressure of oxygen (concentration) in blood.
  • That's because most carbon dioxide travels through the blood as a bicarbonate ion, which is the dissociated form of carbonic acid in solution.
  • This dissociates in solution into bicarbonate and hydrogen ions, the driving force of pH in the blood.
  • This decrease in hemoglobin's affinity for oxygen by the binding of carbon dioxide is known as the Bohr effect, which results in a rightward shift to the O2-saturation curve.

• Irreversible Addition Reactions

  • Reduction of α,β-unsaturated ketones by metal hydride reagents sometimes leads to a saturated alcohol, especially with sodium borohydride.
  • This product is formed by an initial conjugate addition of hydride to the β-carbon atom, followed by ketonization of the enol product and reduction of the resulting saturated ketone (equation 1 below).
  • If the saturated alcohol is the desired product, catalytic hydrogenation prior to (or following) the hydride reduction may be necessary.
  • Before leaving this topic it should be noted that diborane, B2H6, a gas that was used in ether solution to prepare alkyl boranes from alkenes, also reduces many carbonyl groups.
  • Carbonyl groups and conjugated π-electron systems are reduced by metals such as Li, Na and K, usually in liquid ammonia solution.

• Stages in the Product Life Cycle

  • Other competitors enter the market with alternative solutions, making competition in the market fierce.
  • In the decline stage of the product life cycle, sales will begin to decline as the product reaches its saturation point.

• Pressure, Gravity, and Matric Potential

  • A plant can manipulate Ψp via its ability to manipulate Ψs (solute potential) and by the process of osmosis.
  • If a plant cell increases the cytoplasmic solute concentration:
  • In a dry system, it can be as low as –2 MPa in a dry seed or as high as zero in a water-saturated system.
  • Ψm is similar to solute potential because the hydrogen bonds remove energy from the total system.
  • However, in solute potential, the other components are soluble, hydrophilic solute molecules, whereas in Ψm, the other components are insoluble, hydrophilic molecules of the plant cell wall. m cannot be manipulated by the plant and is typically ignored in well-watered roots, stems, and leaves.

• Marketing Orientation

  • Following the second world war, it soon became obvious that products were not selling as easily as during the Industrial era due to a saturated market.
  • Using this customer intelligence, companies could produce products that supported their overall business strategy, competed effectively in an increasingly global and competitive market, and delivered solutions for current and future customer needs.

• Lipid Molecules

  • Fats and oils, which may be saturated or unsaturated, can be unhealthy but also serve important functions for plants and animals.
  • Fatty acids may be saturated or unsaturated.
  • Saturated fatty acids are saturated with hydrogen since single bonds increase the number of hydrogens on each carbon.
  • Stearic acid and palmitic acid, which are commonly found in meat, are examples of saturated fats.
  • Saturated fatty acids have hydrocarbon chains connected by single bonds only.