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.

• 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.

• 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.

• Enone Reactions

  • The cis-syn isomer shown above is the chief dimer formed by irradiation of DNA, or from frozen aqueous solutions of thymine or uracil.
  • Other isomers are formed in varying amounts from room temperature solutions of these bases.
  • These products were formed either by hydrogen atom delivery to both radical sites (giving saturated compounds) or hydrogen delivery followed by hydrogen abstraction by HSe•.

• Fatty Acids

  • Natural fatty acids may be saturated or unsaturated, and as the following data indicate, the saturated acids have higher melting points than unsaturated acids of corresponding size.
  • The higher melting points of the saturated fatty acids reflect the uniform rod-like shape of their molecules.

• Fats & Oils

  • As might be expected from the properties of the fatty acids, fats have a predominance of saturated fatty acids, and oils are composed largely of unsaturated acids.
  • These saturated and trans-fatty acid glycerides in the diet have been linked to long-term health issues such as atherosclerosis.
  • These occur when the cis-double bonds in the fatty acid chains are not completely saturated in the hydrogenation process.

• Cycloalkanes

  • Cycloalkanes are saturated hydrocarbons that contain a ring in their carbon backbones.
  • Cycloalkanes are saturated hydrocarbons that contain a ring in their carbon backbones.

• Using Molarity in Calculations of Solutions

  • In chemistry, molar concentration, or molarity, is defined as moles of solute per total liters of solution.
  • What is the molarity of a solution containing 0.32 moles of NaCl in 3.4 liters of solution?
  • Molarity is a measurement of concentration, with units of mol solute per liter solution.
  • Also, molarity is a ratio that describes the moles of solute per liter of solution.
  • Translate between molarity, grams of solute in solution, and volume of solution.

• Cyclohexadienone Reactions

  • As the name suggests, substrates exhibiting this rearrangement are comprised of two π-functions separated by a saturated (sp3-hybrid) carbon atom (designated by a red dot in the illustration).
  • In dioxane or benzene solution irradiation with 254 nm light gave a high yield of a tetracyclic isomer named lumisantonin.