Solubility.docx

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SolubilityFrom Wikipedia, the free encyclopediaJump to:navigation,search

"Soluble" redirects here. For the algebraic object called asoluble group, seeSolvable group.

Solubility is the property of asolid,liquid, orgaseouschemical substancecalledsolutetodissolvein aliquidsolventto form a homogeneoussolution. The solubility of a substance strongly depends on the

used solvent as well as on temperature and pressure. The extent of the solubility of a substance in a

specific solvent is measured as thesaturationconcentration where adding more solute does not increase

the concentration of the solution.

The solvent is generally a liquid, which can be a pure substance or amixture.[1]

One also speaks of

solid solution, but rarely of solution in a gas (seevapour-liquid equilibriuminstead)

The extent of solubility ranges widely, from infinitely soluble (fullymiscible[2]

) such asethanolin

water, to poorly soluble, such assilver chloridein water. The term insoluble is often applied to poorlyor very poorly soluble compounds.

Under certain conditions theequilibrium solubilitycan be exceeded to give a so-calledsupersaturated

solution, which ismetastable.[3]

Contents[hide] 1 Molecular view 2 Factors affecting solubility

o 2.1 Temperatureo 2.2 Pressure

3 Solubility of gases 4 Polarity 5 Rate of dissolution 6 Quantification of solubility 7 Applications 8 Solubility of ionic compounds in water 9 Solubility of organic compounds 10 Solubility in non-aqueous solvents 11 Solid solution 12 Incongruent dissolution 13 See also 14 External links 15 References

[edit] Molecular viewSolubility occurs under dynamic equilibrium, which means that solubility results from the

simultaneous and opposing processes ofdissolutionandphase separation(e.g.precipitationofsolids).

The solubility equilibrium occurs when the two processes proceed at a constant rate.

The termsolubility is also used in some fields where the solute is altered bysolvolysis. For example,

many metals and theiroxidesare said to be "soluble in hydrochloric acid," whereas the aqueous aciddegrades the solid to irreversibly give soluble products. It is also true that most ionic solids are

degraded by polar solvents, but such processes are reversible. In those cases where the solute is not

recovered upon evaporation of the solvent, the process is referred to as solvolysis. The thermodynamicconcept of solubility does not apply straightforwardly to solvolysis.

When a solute dissolves, it may form several species in the solution. For example, anaqueous

suspensionofferrous hydroxide, Fe(OH)2, will contain the series [Fe(H2O)6 x(OH)x](2 x)+ as well as

otheroligomericspecies. Furthermore, the solubility of ferrous hydroxide and the composition of its

soluble components depends onpH. In general, solubility in the solvent phase can be given only for a

specific solute which is thermodynamically stable, and the value of the solubility will include all the

species in the solution (in the example above, all the iron-containing complexes).[citation needed]

[edit] Factors affecting solubility
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Solubility is defined for specificphases. For example, the solubility ofaragoniteandcalcitein water

are expected to differ, even though they are bothpolymorphsofcalcium carbonateand have the same

chemical formula.

The solubility of one substance in another is determined by the balance ofintermolecular forces

between the solvent and solute, and theentropychange that accompanies the solvation. Factors such as

temperature and pressure will alter this balance, thus changing the solubility.

Solubility may also strongly depend on the presence of other species dissolved in the solvent, forexample,complex-forminganions (ligands) in liquids. Solubility will also depend on the excess or

deficiency of a common ion in the solution, a phenomenon known as thecommon-ion effect. To a

lesser extent, solubility will depend on theionic strengthof solutions. The last two effects can be

quantified using the equation forsolubility equilibrium.

For a solid that dissolves in a redox reaction, solubility is expected to depend on the potential (withinthe range of potentials under which the solid remains the thermodynamically stable phase). For

example, solubility of gold in high-temperature water is observed to be almost an order of magnitude

higher when the redox potential is controlled using a highly-oxidizing Fe3O4-Fe2O3redox bufferthan

with a moderately-oxidizing Ni-NiO buffer.[4]

Solubility (metastable) also depends on the physical size of the crystal or droplet of solute (or, strictlyspeaking, on the specific or molar surface area of the solute). For quantification, see the equation in the

article onsolubility equilibrium. For highly defective crystals, solubility may increase with the

increasing degree of disorder. Both of these effects occur because of the dependence of solubilityconstant on the Gibbs energy of the crystal. The last two effects, although often difficult to measure,

are of practical importance.[citation needed]

For example, they provide the driving force forprecipitate aging

(the crystal size spontaneously increasing with time).

[edit] Temperature
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The solubility of a given solute in a given solvent typically depends on temperature. For many solids

dissolved in liquid water, the solubility increases with temperature up to 100 C.[5]

In liquid water at

high temperatures, (e.g., that approaching thecritical temperature), the solubility of ionic solutes tends

to decrease due to the change of properties and structure of liquid water; the lowerdielectric constant

results in a lesspolar solvent.

Gaseoussolutes exhibit more complex behavior with temperature. As the temperature is raised, gasesusually become less soluble in water (to minimum which is below 120 C for most permanent gases

[6]),

but more soluble in organic solvents.[5]

The chart shows solubility curves for some typical solid inorganic salts.[7]

Many salts behave like

barium nitrateand disodium hydrogen arsenate, and show a large increase in solubility with

temperature. Some solutes (e.g. NaCl in water) exhibit solubility which is fairly independent of

temperature. A few, such as cerium(III) sulfate, become less soluble in water as temperature increases.

This temperature dependence is sometimes referred to as "retrograde" or "inverse" solubility.

Occasionally, a more complex pattern is observed, as withsodium sulfate, where the less soluble

decahydratecrystal loseswater of crystallizationat 32 C to form a more solubleanhydrous

phase.[citation needed]

The solubility oforganic compoundsnearly always increases with temperature. The technique of

recrystallization, used for purification of solids, depends on a solute's different solubilities in hot and

cold solvent. A few exceptions exist, such as certaincyclodextrins.[8]

[edit] PressureFor condensed phases (solids and liquids), the pressure dependence of solubility is typically weak and

usually neglected in practice. Assuming an ideal solution, the dependence can be quantified as:

where the index i iterates the components, Ni is the mole fraction of the ith

component in the solution, P

is the pressure, the index T refers to constant temperature, Vi,aq is thepartial molar volumeof the ith

component in the solution, Vi,cr is the partial molar volume of the ith

component in the dissolving solid,

and R is theuniversal gas constant[9]

.
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The pressure dependence of solubility does occasionally have practical significance. For example,

precipitation foulingof oil fields and wells by calcium sulfate (which decreases its solubility with

decreasing pressure) can result in decreased productivity with time.

[edit] Solubility of gasesHenry's lawis used to quantify the solubility of gases in solvents. The solubility of a gas in a solvent is

directly proportional to thepartial pressureof that gas above the solvent. This relationship is written as:

where k is a temperature-dependent constant (for example, 769.2Latm/molfordioxygen(O2) in water

at 298 K), p is the partial pressure (atm), and c is theconcentrationof the dissolved gas in the liquid

(mol/L).

[edit] PolarityA popularaphorismused for predicting solubility is "like dissolves like".

[10]This statement indicates

that a solute will dissolve best in a solvent that has a similarpolarityto itself. This view is rather

simplistic, since it ignores many solvent-solute interactions, but it is a useful rule of thumb. For

example, a very polar(hydrophilic) solute such asureais very soluble in highly polar water, less

soluble in fairly polarmethanol, and practically insoluble in non-polar solvents such asbenzene. In

contrast, a non-polar orlipophilicsolute such asnaphthaleneis insoluble in water, fairly soluble in

methanol, and highly soluble in non-polar benzene.[11]Liquid solubilities also generally follow this rule. Lipophilic plant oils, such as olive oil and palm oil,

dissolve in non-polar solvents such as alkanes, but are less soluble in polar liquids such as water.

Synthetic chemists often exploit differences in solubilities to separate and purify compounds fromreaction mixtures, using the technique ofliquid-liquid extraction.

Insolubility and spontaneous phase separation does not mean that dissolution is disfavored by enthalpy.

Quite the contrary, in the case of water and hydrophobic substances,hydrophobic hydrationis

reasonably exothermic and enthalpy alone should be favor it. It appears that entropic factors the

reduced freedom of movement of water molecules around hydrophobic molecules lead to an overall

hydrophobic effect.

[edit] Rate of dissolutionDissolutionis not always an instantaneous process. It is fast when salt and sugar dissolve in water but

much slower for a tablet ofaspirinor a large crystal of hydratedcopper(II) sulfate. These observationsare the consequence of two factors: the rate of solubilization is related to the solubility product and the

surface area of the material. The speed at which a solid dissolves may depend on its crystallinity or

lack thereof in the case ofamorphoussolids and the surface area (crystallite size) and the presence of

polymorphism. Many practical systems illustrate this effect, for example in designing methods for

controlleddrug delivery. Critically, the dissolution rate depends on the presence of mixing and other

factors that determine the degree of undersaturation in the liquid solvent film immediately adjacent to

the solid solute crystal. In some cases, solubility equilibria can take a long time to establish (hours,

days, months, or many years; depending on the nature of the solute and other factors). In practice, it

means that the amount of solute in a solution is not always determined by its thermodynamic solubility,

but may depend on kinetics of dissolution (or precipitation).

The rate of dissolution and solubility should not be confused as they are different concepts, kinetic and

thermodynamic, respectively. The solubilization kinetics, as well as apparent solubility can be

improved after complexation of an active ingredient with cyclodextrin. This can be used in the case ofdrug with poor solubility.

[12]

[edit] Quantification of solubilitySolubility is commonly expressed as a concentration, either by mass (g of solute per kg of solvent, g

per dL (100 mL) of solvent),molarity,molality, mole fraction or other similar descriptions of

concentration. The maximum equilibrium amount of solute that can dissolve per amount of solvent is

the solubility of that solute in that solvent under the specified conditions. The advantage of expressing

solubility in this manner is its simplicity, while the disadvantage is that it can strongly depend on the

presence of other species in the solvent (for example, the common ion effect).

Solubility constantsare used to describe saturated solutions of ionic compounds of relatively low

solubility (seesolubility equilibrium). The solubility constant is a special case of anequilibrium

constant. It describes the balance between dissolved ions from the salt and undissolved salt. The

solubility constant is also "applicable" (i.e. useful) toprecipitation, the reverse of the dissolvingreaction. As with other equilibrium constants,temperaturecan affect the numerical value of solubility
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constant. The solubility constant is not as simple as solubility, however the value of this constant is

generally independent of the presence of other species in the solvent.

TheFlory-Huggins solution theoryis a theoretical model describing the solubility of polymers. The

Hansen Solubility Parametersand theHildebrand solubility parametersare empirical methods for the

prediction of solubility. It is also possible to predict solubility from other physical constants such as the

enthalpy of fusion.

Thepartition coefficient(Log P) is a measure of differential solubility of a compound in ahydrophobicsolvent (octanol) and ahydrophilicsolvent (water). The logarithm of these two values enables

compounds to be ranked in terms of hydrophilicity (or hydrophobicity).

[edit] ApplicationsSolubility is of fundamental importance in a large number of scientific disciplines and practical

applications, ranging from ore processing, to the use of medicines, and the transport of pollutants.

Solubility is often said to be one of the "characteristic properties of a substance," which means that

solubility is commonly used to describe the substance, to indicate a substance's polarity, to help to

distinguish it from other substances, and as a guide to applications of the substance. For example,

indigois described as "insoluble in water, alcohol, or ether but soluble in chloroform, nitrobenzene, or

concentrated sulfuric acid".[citation needed]

Solubility of a substance is useful when separating mixtures. For example, a mixture of salt (sodium

chloride) and silica may be separated by dissolving the salt in water, and filtering off the undissolvedsilica. The synthesis of chemical compounds, by the milligram in a laboratory, or by the ton in

industry, both make use of the relative solubilities of the desired product, as well as unreacted starting

materials, byproducts, and side products to achieve separation.

Another example of this is the synthesis ofbenzoic acidfromphenylmagnesium bromideanddry ice.

Benzoic acid is more soluble in an organic solvent such asdichloromethaneordiethyl ether, and when

shaken with this organic solvent in aseparatory funnel, will preferentially dissolve in the organic layer.

The other reaction products, including the magnesium bromide, will remain in the aqueous layer,

clearly showing that separation based on solubility is achieved. This process, known asliquid-liquid

extraction, is an important technique insynthetic chemistry.

[edit] Solubility of ionic compounds in waterSome ionic compounds (salts) dissolve in water, which arises because of the attraction between

positive and negative charges (see:solvation). For example, the salt's positive ions (e.g. Ag

+

) attract thepartially-negative oxygens in H2O. Likewise, the salt's negative ions (e.g. Cl) attract the partially-

positive hydrogens in H2O. Note: oxygen is partially-negative because it is moreelectronegativethan

hydrogen, and vice-versa (see:chemical polarity).

AgCl(s) Ag+

(aq) + Cl

(aq)

However, there is a limit to how much salt can be dissolved in a given volume of water. This amount isgiven by thesolubility product, Ksp. This value depends on the type of salt (AgCl vs. NaCl, for

example), temperature, and the common ion effect.

One can calculate the amount of AgCl that will dissolve in 1 liter of water, some algebra is required.

Ksp = [Ag+] [Cl] (definition of solubility product)

Ksp = 1.8 1010 (from a table of solubility products)

[Ag+] = [Cl], in the absence of other silver or chloride salts,

[Ag+]2 = 1.8 10

10[Ag

+] = 1.34 10

5

The result: 1 liter of water can dissolve 1.34 105molesof AgCl(s) at room temperature. Compared

with other types of salts, AgCl is poorly soluble in water. In contrast, table salt (NaCl) has a higher Ksp

and is, therefore, more soluble.

Main article:Solubility chart

Soluble Insoluble

Group IandNH4+compounds

carbonates(exceptGroup I,NH4+anduranyl

compounds)

nitrates sulfites(exceptGroup IandNH4+compounds)

acetates(ethanoates) (exceptAg+compounds) phosphates(exceptGroup IandNH4

+compounds)

chlorides,bromidesandiodides(exceptAg+,Pb

2+,

Cu+andHg22+)

hydroxidesandoxides(exceptGroup I,NH4+,

Ba2+,Sr2+andTl+)
http://en.wikipedia.org/wiki/Flory-Huggins_solution_theoryhttp://en.wikipedia.org/wiki/Flory-Huggins_solution_theoryhttp://en.wikipedia.org/wiki/Flory-Huggins_solution_theoryhttp://en.wikipedia.org/wiki/Hansen_Solubility_Parametershttp://en.wikipedia.org/wiki/Hansen_Solubility_Parametershttp://en.wikipedia.org/wiki/Hildebrand_solubility_parameterhttp://en.wikipedia.org/wiki/Hildebrand_solubility_parameterhttp://en.wikipedia.org/wiki/Hildebrand_solubility_parameterhttp://en.wikipedia.org/wiki/Enthalpy_of_fusionhttp://en.wikipedia.org/wiki/Enthalpy_of_fusionhttp://en.wikipedia.org/wiki/Partition_coefficienthttp://en.wikipedia.org/wiki/Partition_coefficienthttp://en.wikipedia.org/wiki/Partition_coefficienthttp://en.wikipedia.org/wiki/Log_Phttp://en.wikipedia.org/wiki/Log_Phttp://en.wikipedia.org/wiki/Log_Phttp://en.wikipedia.org/wiki/Hydrophobehttp://en.wikipedia.org/wiki/Hydrophobehttp://en.wikipedia.org/wiki/Hydrophobehttp://en.wikipedia.org/wiki/Octanolhttp://en.wikipedia.org/wiki/Octanolhttp://en.wikipedia.org/wiki/Octanolhttp://en.wikipedia.org/wiki/Hydrophilehttp://en.wikipedia.org/wiki/Hydrophilehttp://en.wikipedia.org/wiki/Hydrophilehttp://en.wikipedia.org/wiki/Waterhttp://en.wikipedia.org/wiki/Waterhttp://en.wikipedia.org/wiki/Waterhttp://en.wikipedia.org/w/index.php?title=Solubility&action=edit&section=9http://en.wikipedia.org/w/index.php?title=Solubility&action=edit&section=9http://en.wikipedia.org/wiki/Indigo_dye#Chemical_propertieshttp://en.wikipedia.org/wiki/Indigo_dye#Chemical_propertieshttp://en.wikipedia.org/wiki/Wikipedia:Citation_neededhttp://en.wikipedia.org/wiki/Wikipedia:Citation_neededhttp://en.wikipedia.org/wiki/Wikipedia:Citation_neededhttp://en.wikipedia.org/wiki/Sodium_chloridehttp://en.wikipedia.org/wiki/Sodium_chloridehttp://en.wikipedia.org/wiki/Sodium_chloridehttp://en.wikipedia.org/wiki/Sodium_chloridehttp://en.wikipedia.org/wiki/Benzoic_acidhttp://en.wikipedia.org/wiki/Benzoic_acidhttp://en.wikipedia.org/wiki/Benzoic_acidhttp://en.wikipedia.org/wiki/Phenylmagnesium_bromidehttp://en.wikipedia.org/wiki/Phenylmagnesium_bromidehttp://en.wikipedia.org/wiki/Phenylmagnesium_bromidehttp://en.wikipedia.org/wiki/Dry_icehttp://en.wikipedia.org/wiki/Dry_icehttp://en.wikipedia.org/wiki/Dry_icehttp://en.wikipedia.org/wiki/Dichloromethanehttp://en.wikipedia.org/wiki/Dichloromethanehttp://en.wikipedia.org/wiki/Dichloromethanehttp://en.wikipedia.org/wiki/Diethyl_etherhttp://en.wikipedia.org/wiki/Diethyl_etherhttp://en.wikipedia.org/wiki/Diethyl_etherhttp://en.wikipedia.org/wiki/Separatory_funnelhttp://en.wikipedia.org/wiki/Separatory_funnelhttp://en.wikipedia.org/wiki/Separatory_funnelhttp://en.wikipedia.org/wiki/Liquid-liquid_extractionhttp://en.wikipedia.org/wiki/Liquid-liquid_extractionhttp://en.wikipedia.org/wiki/Liquid-liquid_extractionhttp://en.wikipedia.org/wiki/Liquid-liquid_extractionhttp://en.wikipedia.org/wiki/Synthetic_chemistryhttp://en.wikipedia.org/wiki/Synthetic_chemistryhttp://en.wikipedia.org/wiki/Synthetic_chemistryhttp://en.wikipedia.org/w/index.php?title=Solubility&action=edit&section=10http://en.wikipedia.org/w/index.php?title=Solubility&action=edit&section=10http://en.wikipedia.org/wiki/Saltshttp://en.wikipedia.org/wiki/Saltshttp://en.wikipedia.org/wiki/Saltshttp://en.wikipedia.org/wiki/Solvationhttp://en.wikipedia.org/wiki/Solvationhttp://en.wikipedia.org/wiki/Solvationhttp://en.wikipedia.org/wiki/Electronegativityhttp://en.wikipedia.org/wiki/Electronegativityhttp://en.wikipedia.org/wiki/Electronegativityhttp://en.wikipedia.org/wiki/Chemical_polarityhttp://en.wikipedia.org/wiki/Chemical_polarityhttp://en.wikipedia.org/wiki/Chemical_polarityhttp://en.wikipedia.org/wiki/Solubility_producthttp://en.wikipedia.org/wiki/Solubility_producthttp://en.wikipedia.org/wiki/Solubility_producthttp://en.wikipedia.org/wiki/Mole_%28unit%29http://en.wikipedia.org/wiki/Mole_%28unit%29http://en.wikipedia.org/wiki/Mole_%28unit%29http://en.wikipedia.org/wiki/Solubility_charthttp://en.wikipedia.org/wiki/Solubility_charthttp://en.wikipedia.org/wiki/Solubility_charthttp://en.wikipedia.org/wiki/Alkali_metalhttp://en.wikipedia.org/wiki/Alkali_metalhttp://en.wikipedia.org/wiki/Ammoniumhttp://en.wikipedia.org/wiki/Ammoniumhttp://en.wikipedia.org/wiki/Ammoniumhttp://en.wikipedia.org/wiki/Ammoniumhttp://en.wikipedia.org/wiki/Ammoniumhttp://en.wikipedia.org/wiki/Carbonatehttp://en.wikipedia.org/wiki/Carbonatehttp://en.wikipedia.org/wiki/Alkali_metalhttp://en.wikipedia.org/wiki/Alkali_metalhttp://en.wikipedia.org/wiki/Alkali_metalhttp://en.wikipedia.org/wiki/Ammoniumhttp://en.wikipedia.org/wiki/Ammoniumhttp://en.wikipedia.org/wiki/Ammoniumhttp://en.wikipedia.org/wiki/Ammoniumhttp://en.wikipedia.org/wiki/Ammoniumhttp://en.wikipedia.org/wiki/Uranylhttp://en.wikipedia.org/wiki/Uranylhttp://en.wikipedia.org/wiki/Uranylhttp://en.wikipedia.org/wiki/Nitratehttp://en.wikipedia.org/wiki/Nitratehttp://en.wikipedia.org/wiki/Sulfitehttp://en.wikipedia.org/wiki/Sulfitehttp://en.wikipedia.org/wiki/Alkali_metalhttp://en.wikipedia.org/wiki/Alkali_metalhttp://en.wikipedia.org/wiki/Alkali_metalhttp://en.wikipedia.org/wiki/Ammoniumhttp://en.wikipedia.org/wiki/Ammoniumhttp://en.wikipedia.org/wiki/Ammoniumhttp://en.wikipedia.org/wiki/Ammoniumhttp://en.wikipedia.org/wiki/Ammoniumhttp://en.wikipedia.org/wiki/Acetatehttp://en.wikipedia.org/wiki/Acetatehttp://en.wikipedia.org/wiki/Silverhttp://en.wikipedia.org/wiki/Silverhttp://en.wikipedia.org/wiki/Silverhttp://en.wikipedia.org/wiki/Silverhttp://en.wikipedia.org/wiki/Phosphatehttp://en.wikipedia.org/wiki/Phosphatehttp://en.wikipedia.org/wiki/Alkali_metalhttp://en.wikipedia.org/wiki/Alkali_metalhttp://en.wikipedia.org/wiki/Alkali_metalhttp://en.wikipedia.org/wiki/Ammoniumhttp://en.wikipedia.org/wiki/Ammoniumhttp://en.wikipedia.org/wiki/Ammoniumhttp://en.wikipedia.org/wiki/Ammoniumhttp://en.wikipedia.org/wiki/Ammoniumhttp://en.wikipedia.org/wiki/Chloridehttp://en.wikipedia.org/wiki/Chloridehttp://en.wikipedia.org/wiki/Bromidehttp://en.wikipedia.org/wiki/Bromidehttp://en.wikipedia.org/wiki/Bromidehttp://en.wikipedia.org/wiki/Iodidehttp://en.wikipedia.org/wiki/Iodidehttp://en.wikipedia.org/wiki/Iodidehttp://en.wikipedia.org/wiki/Silverhttp://en.wikipedia.org/wiki/Silverhttp://en.wikipedia.org/wiki/Silverhttp://en.wikipedia.org/wiki/Silverhttp://en.wikipedia.org/wiki/Leadhttp://en.wikipedia.org/wiki/Leadhttp://en.wikipedia.org/wiki/Leadhttp://en.wikipedia.org/wiki/Leadhttp://en.wikipedia.org/wiki/Copperhttp://en.wikipedia.org/wiki/Copperhttp://en.wikipedia.org/wiki/Copperhttp://en.wikipedia.org/wiki/Mercury_%28element%29http://en.wikipedia.org/wiki/Mercury_%28element%29http://en.wikipedia.org/wiki/Mercury_%28element%29http://en.wikipedia.org/wiki/Mercury_%28element%29http://en.wikipedia.org/wiki/Mercury_%28element%29http://en.wikipedia.org/wiki/Hydroxidehttp://en.wikipedia.org/wiki/Hydroxidehttp://en.wikipedia.org/wiki/Oxidehttp://en.wikipedia.org/wiki/Oxidehttp://en.wikipedia.org/wiki/Oxidehttp://en.wikipedia.org/wiki/Alkali_metalhttp://en.wikipedia.org/wiki/Alkali_metalhttp://en.wikipedia.org/wiki/Alkali_metalhttp://en.wikipedia.org/wiki/Ammoniumhttp://en.wikipedia.org/wiki/Ammoniumhttp://en.wikipedia.org/wiki/Ammoniumhttp://en.wikipedia.org/wiki/Ammoniumhttp://en.wikipedia.org/wiki/Ammoniumhttp://en.wikipedia.org/wiki/Bariumhttp://en.wikipedia.org/wiki/Bariumhttp://en.wikipedia.org/wiki/Bariumhttp://en.wikipedia.org/wiki/Strontiumhttp://en.wikipedia.org/wiki/Strontiumhttp://en.wikipedia.org/wiki/Strontiumhttp://en.wikipedia.org/wiki/Strontiumhttp://en.wikipedia.org/wiki/Thalliumhttp://en.wikipedia.org/wiki/Thalliumhttp://en.wikipedia.org/wiki/Thalliumhttp://en.wikipedia.org/wiki/Thalliumhttp://en.wikipedia.org/wiki/Thalliumhttp://en.wikipedia.org/wiki/Strontiumhttp://en.wikipedia.org/wiki/Bariumhttp://en.wikipedia.org/wiki/Ammoniumhttp://en.wikipedia.org/wiki/Alkali_metalhttp://en.wikipedia.org/wiki/Oxidehttp://en.wikipedia.org/wiki/Hydroxidehttp://en.wikipedia.org/wiki/Mercury_%28element%29http://en.wikipedia.org/wiki/Copperhttp://en.wikipedia.org/wiki/Leadhttp://en.wikipedia.org/wiki/Silverhttp://en.wikipedia.org/wiki/Iodidehttp://en.wikipedia.org/wiki/Bromidehttp://en.wikipedia.org/wiki/Chloridehttp://en.wikipedia.org/wiki/Ammoniumhttp://en.wikipedia.org/wiki/Alkali_metalhttp://en.wikipedia.org/wiki/Phosphatehttp://en.wikipedia.org/wiki/Silverhttp://en.wikipedia.org/wiki/Acetatehttp://en.wikipedia.org/wiki/Ammoniumhttp://en.wikipedia.org/wiki/Alkali_metalhttp://en.wikipedia.org/wiki/Sulfitehttp://en.wikipedia.org/wiki/Nitratehttp://en.wikipedia.org/wiki/Uranylhttp://en.wikipedia.org/wiki/Ammoniumhttp://en.wikipedia.org/wiki/Alkali_metalhttp://en.wikipedia.org/wiki/Carbonatehttp://en.wikipedia.org/wiki/Ammoniumhttp://en.wikipedia.org/wiki/Alkali_metalhttp://en.wikipedia.org/wiki/Solubility_charthttp://en.wikipedia.org/wiki/Mole_%28unit%29http://en.wikipedia.org/wiki/Solubility_producthttp://en.wikipedia.org/wiki/Chemical_polarityhttp://en.wikipedia.org/wiki/Electronegativityhttp://en.wikipedia.org/wiki/Solvationhttp://en.wikipedia.org/wiki/Saltshttp://en.wikipedia.org/w/index.php?title=Solubility&action=edit&section=10http://en.wikipedia.org/wiki/Synthetic_chemistryhttp://en.wikipedia.org/wiki/Liquid-liquid_extractionhttp://en.wikipedia.org/wiki/Liquid-liquid_extractionhttp://en.wikipedia.org/wiki/Separatory_funnelhttp://en.wikipedia.org/wiki/Diethyl_etherhttp://en.wikipedia.org/wiki/Dichloromethanehttp://en.wikipedia.org/wiki/Dry_icehttp://en.wikipedia.org/wiki/Phenylmagnesium_bromidehttp://en.wikipedia.org/wiki/Benzoic_acidhttp://en.wikipedia.org/wiki/Sodium_chloridehttp://en.wikipedia.org/wiki/Sodium_chloridehttp://en.wikipedia.org/wiki/Wikipedia:Citation_neededhttp://en.wikipedia.org/wiki/Indigo_dye#Chemical_propertieshttp://en.wikipedia.org/w/index.php?title=Solubility&action=edit&section=9http://en.wikipedia.org/wiki/Waterhttp://en.wikipedia.org/wiki/Hydrophilehttp://en.wikipedia.org/wiki/Octanolhttp://en.wikipedia.org/wiki/Hydrophobehttp://en.wikipedia.org/wiki/Log_Phttp:/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sulfates(exceptAg+,Pb

2+,Ba

2+,Sr

2+andCa

2+)

sulfides(exceptGroup I,Group IIandNH4+

compounds)

[edit] Solubility of organic compoundsThe principle outlined above underpolarity, that like dissolves like, is the usual guide to solubility with

organic systems. For example,petroleum jellywill dissolve ingasolinebecause both petroleum jelly

and gasoline are hydrocarbons. It will not, on the other hand, dissolve in alcohol or water, since thepolarity of these solvents is too high. Sugar will not dissolve in gasoline, since sugar is too polar in

comparison with gasoline. A mixture of gasoline and sugar can therefore be separated byfiltration, or

extractionwith water.

[edit] Solubility in non-aqueous solventsMost publicly available solubility values are those for solubility in water.

[13]The reference also lists

some for non-aqueous solvents. Solubility data for non-aqueous solvents is currently being collected

via anopen notebook sciencecrowdsourcingproject.[14][15]

[edit] Solid solutionThis term is often used in the field ofmetallurgyto refer to the extent that analloyingelement will

dissolve into thebase metalwithout forming a separate phase. The solubility line (or curve) is the line

(or lines) on aphase diagramwhich give the limits of solute addition. That is, the lines show themaximum amount of a component that can be added to another component and still be insolid

solution. In the solid's crystalline structure, the 'solute' element can either take the place of the matrix

within the lattice (a subtitutional position, for example: chromium in iron) or can take a place in a

space between the lattice points (an interstitial position, for example: carbon in iron).

In microelectronic fabrication, solid solubility refers to the maximum concentration of impurities one

can place into the substrate.

[edit] Incongruent dissolutionMany substances dissolve congruently, i.e., the composition of the solid and the dissolved solute

stoichiometrically match. However, some substances may dissolveincongruently, whereby the

composition of the solute in solution does not match that of the solid. This solubilization is

accompanied by alteration of the "primary solid" and possibly formation of a secondary solid phase.

However, generally, some primary solid also remains and a complex solubility equilibrium establishes.For example, dissolution ofalbitemay result in formation ofgibbsite.[16]

NaAlSi3O8(s) + H+

+ 7H2O = Na+

+ Al(OH)3(s) + 3H4SiO4.

In this case, the solubility of albite is expected to depend on the solid-to-solvent ratio. This kind ofsolubility is of great importance in geology, where it results in formation ofmetamorphic rocks.
http://en.wikipedia.org/wiki/Sulfatehttp://en.wikipedia.org/wiki/Sulfatehttp://en.wikipedia.org/wiki/Silverhttp://en.wikipedia.org/wiki/Silverhttp://en.wikipedia.org/wiki/Silverhttp://en.wikipedia.org/wiki/Silverhttp://en.wikipedia.org/wiki/Leadhttp://en.wikipedia.org/wiki/Leadhttp://en.wikipedia.org/wiki/Leadhttp://en.wikipedia.org/wiki/Leadhttp://en.wikipedia.org/wiki/Bariumhttp://en.wikipedia.org/wiki/Bariumhttp://en.wikipedia.org/wiki/Bariumhttp://en.wikipedia.org/wiki/Bariumhttp://en.wikipedia.org/wiki/Strontiumhttp://en.wikipedia.org/wiki/Strontiumhttp://en.wikipedia.org/wiki/Strontiumhttp://en.wikipedia.org/wiki/Strontiumhttp://en.wikipedia.org/wiki/Calciumhttp://en.wikipedia.org/wiki/Calciumhttp://en.wikipedia.org/wiki/Calciumhttp://en.wikipedia.org/wiki/Calciumhttp://en.wikipedia.org/wiki/Sulfidehttp://en.wikipedia.org/wiki/Sulfidehttp://en.wikipedia.org/wiki/Alkali_metalhttp://en.wikipedia.org/wiki/Alkali_metalhttp://en.wikipedia.org/wiki/Alkali_metalhttp://en.wikipedia.org/wiki/Alkaline_earth_metalhttp://en.wikipedia.org/wiki/Alkaline_earth_metalhttp://en.wikipedia.org/wiki/Alkaline_earth_metalhttp://en.wikipedia.org/wiki/Ammoniumhttp://en.wikipedia.org/wiki/Ammoniumhttp://en.wikipedia.org/wiki/Ammoniumhttp://en.wikipedia.org/wiki/Ammoniumhttp://en.wikipedia.org/wiki/Ammoniumhttp://en.wikipedia.org/w/index.php?title=Solubility&action=edit&section=11http://en.wikipedia.org/w/index.php?title=Solubility&action=edit&section=11http://en.wikipedia.org/wiki/Solubility#Polarityhttp://en.wikipedia.org/wiki/Solubility#Polarityhttp://en.wikipedia.org/wiki/Solubility#Polarityhttp://en.wikipedia.org/wiki/Petroleum_jellyhttp://en.wikipedia.org/wiki/Petroleum_jellyhttp://en.wikipedia.org/wiki/Petroleum_jellyhttp://en.wikipedia.org/wiki/Gasolinehttp://en.wikipedia.org/wiki/Gasolinehttp://en.wikipedia.org/wiki/Gasolinehttp://en.wikipedia.org/wiki/Filtrationhttp://en.wikipedia.org/wiki/Filtrationhttp://en.wikipedia.org/wiki/Filtrationhttp://en.wikipedia.org/wiki/Solvent_extractionhttp://en.wikipedia.org/wiki/Solvent_extractionhttp://en.wikipedia.org/w/index.php?title=Solubility&action=edit&section=12http://en.wikipedia.org/w/index.php?title=Solubility&action=edit&section=12http://en.wikipedia.org/wiki/Solubility#cite_note-12http://en.wikipedia.org/wiki/Solubility#cite_note-12http://en.wikipedia.org/wiki/Solubility#cite_note-12http://en.wikipedia.org/wiki/Open_notebook_sciencehttp://en.wikipedia.org/wiki/Open_notebook_sciencehttp://en.wikipedia.org/wiki/Crowdsourcinghttp://en.wikipedia.org/wiki/Crowdsourcinghttp://en.wikipedia.org/wiki/Crowdsourcinghttp://en.wikipedia.org/wiki/Solubility#cite_note-13http://en.wikipedia.org/wiki/Solubility#cite_note-13http://en.wikipedia.org/wiki/Solubility#cite_note-13http://en.wikipedia.org/w/index.php?title=Solubility&action=edit&section=13http://en.wikipedia.org/w/index.php?title=Solubility&action=edit&section=13http://en.wikipedia.org/wiki/Metallurgyhttp://en.wikipedia.org/wiki/Metallurgyhttp://en.wikipedia.org/wiki/Metallurgyhttp://en.wikipedia.org/wiki/Alloyhttp://en.wikipedia.org/wiki/Alloyhttp://en.wikipedia.org/wiki/Alloyhttp://en.wikipedia.org/wiki/Base_metalhttp://en.wikipedia.org/wiki/Base_metalhttp://en.wikipedia.org/wiki/Base_metalhttp://en.wikipedia.org/wiki/Phase_diagramhttp://en.wikipedia.org/wiki/Phase_diagramhttp://en.wikipedia.org/wiki/Phase_diagramhttp://en.wikipedia.org/wiki/Solid_solutionhttp://en.wikipedia.org/wiki/Solid_solutionhttp://en.wikipedia.org/wiki/Solid_solutionhttp://en.wikipedia.org/wiki/Solid_solutionhttp://en.wikipedia.org/w/index.php?title=Solubility&action=edit&section=14http://en.wikipedia.org/w/index.php?title=Solubility&action=edit&section=14http://en.wikipedia.org/wiki/Incongruent_transitionhttp://en.wikipedia.org/wiki/Incongruent_transitionhttp://en.wikipedia.org/wiki/Incongruent_transitionhttp://en.wikipedia.org/wiki/Albitehttp://en.wikipedia.org/wiki/Albitehttp://en.wikipedia.org/wiki/Albitehttp://en.wikipedia.org/wiki/Gibbsitehttp://en.wikipedia.org/wiki/Gibbsitehttp://en.wikipedia.org/wiki/Solubility#cite_note-15http://en.wikipedia.org/wiki/Solubility#cite_note-15http://en.wikipedia.org/wiki/Solubility#cite_note-15http://en.wikipedia.org/wiki/Metamorphic_rockhttp://en.wikipedia.org/wiki/Metamorphic_rockhttp://en.wikipedia.org/wiki/Metamorphic_rockhttp://en.wikipedia.org/wiki/Metamorphic_rockhttp://en.wikipedia.org/wiki/Solubility#cite_note-15http://en.wikipedia.org/wiki/Gibbsitehttp://en.wikipedia.org/wiki/Albitehttp://en.wikipedia.org/wiki/Incongruent_transitionhttp://en.wikipedia.org/w/index.php?title=Solubility&action=edit&section=14http://en.wikipedia.org/wiki/Solid_solutionhttp://en.wikipedia.org/wiki/Solid_solutionhttp://en.wikipedia.org/wiki/Phase_diagramhttp://en.wikipedia.org/wiki/Base_metalhttp://en.wikipedia.org/wiki/Alloyhttp://en.wikipedia.org/wiki/Metallurgyhttp://en.wikipedia.org/w/index.php?title=Solubility&action=edit&section=13http://en.wikipedia.org/wiki/Solubility#cite_note-13http://en.wikipedia.org/wiki/Solubilit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Solubility.docx