Shopping on line can be easy, simple and save you lots of money. It can also take a lot of your time, frustrate you, and result in unwanted purchases. Now the same can be said for regular high street shopping, but with the vast opportunity presented by the Internet it will pay you to spend a few minutes reading this and understanding how to better optimize your Solubility shopping experience:
1. Compare - without doubt the biggest advantage that the Solubility offers shoppers today is the ability to compare thousands of Solubility at a time. This is a great thing, but not necessarily all the time! Too much can be daunting at times so take advantage of the great comparison sites and where possible let them do the hard work for you.
2. Research - if it has been said it will be on the internet. Ignorance is no longer a justifiable reason for buying the wrong thing. Take the time to research in detail everything that you could possible want to know about
3. Testimonials - don't know anybody that has bought a Solubility? Wrong! If the Solubility is good the internet will let you know. Use the Internet as a friend and get testimonials before you buy.
4. Questions - Got a question about Solubility then search the Forums, FAQ's, Blogs etc. Don't be afraid to ask .....
5. Reputation - Never heard of the company selling Solubility? Don't worry, no reason why you should know every company in the world, but you know someone that does! Use the internet to find out what people are saying about Solubility and build up a picture of their reputation for sales, returns, customer service, delivery etc.
6. Returns - still worried that even after all of the above your Solubility wont be what you want? Check out the returns policy. There is so much competition now that someone, somewhere is bound to offer the terms that you are comfortable with.
7. Feedback - happy with your Solubility then let people know, after all you are depending on others people input in your buying decision, so why not give a little back.
8. Security - check for the yellow padlock on the Solubility site before you buy, and the s after http:/ /i.e. https:// = a secure site
9. Contact - got a question about Solubility, or want to leave a comment then check out the sites contact page. Reputable companies have them and respond.
10. Payment - ready to pay for your Solubility, then use your credit card or PayPal! Be aware of companies that don't accept them, there may be genuine reasons but given the huge amount of choice you have when buying online there is no reason at all not to buy via credit card or PayPal.
Solubility is a
physical property referring to the ability for a given substance, the
solute, to dissolve in a
solvent.
Atkins' Physical Chemistry, 7th Ed. by Julio De Paula, P.W. Atkins ISBN 0198792859 It is measured in terms of the maximum amount of solute
dissolved in a solvent at
chemical equilibrium. The resulting solution is called a saturated solution. Certain substances are soluble in all proportions with a given solvent, such as
ethanol in
water. This property is known as
miscible.
Under various conditions, the equilibrium solubility can be exceeded to give a so-called
supersaturation solution, which is Metastability in molecules. The solvent is often a liquid, which can be a pure substance or a
mixture. The species that dissolves, the solute, can be a gas, another liquid, or a solid. Solubilities range widely, from infinitely soluble such as
ethanol in water, to poorly soluble, such as silver chloride in water. The term
insoluble is often applied to poorly soluble compounds, though strictly speaking there are very few cases where there is absolutely no material dissolved.
Molecular view
The process of dissolving, called
dissolution, is relatively straightforward for covalent bond substances such as ethanol. When ethanol dissolves in water, the ethanol molecules remain intact but form new
hydrogen bonds with the water. When, however, an ionic bond compound such as sodium chloride (NaCl) dissolves in water, the sodium chloride Crystal structure Dissociation (chemistry) into separate ions which are
solvation (wrapped) with a coating of water molecules. Nonetheless, NaCl is said to dissolve in water, because evaporation of the solvent returns crystalline NaCl.
Sometimes the term "dissolving" is applied to an irreversible
chemical reaction, as with iron in nitric acid, but in such a case the thermodynamic concept of solubility does not apply.
When it dissolves, a solute may form several species in the solution. For example, water above the crystals of ferrous hydroxide, Fe(OH)2, will, at equilibrium, contain Fe2+, Fe(OH)+, Fe(OH)2, Fe(OH)3- and possibly other complexes. Therefore, the solubility of ferrous hydroxide depends on pH. In general, solubility in the solvent phase can be given only for a specific solute which is thermodynamically stable, and the value of the solublity will include all the species in the solution (in the example above, all the iron-containing complexes).
Factors affecting solubility
Solubility is defined for specific
phase (matter). For example, the solubility of
aragonite and
calcite in water are expected to be different, even though both are the same chemical substance (calcium carbonate).
The solubility of one substance dissolving in another is determined by the balance of intermolecular forces between the solvent and solute and the entropy change 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, for example,
complex (chemistry)forming anions (
ligands) in liquids. Solubility will also depend on the excess (or deficiency) of a common ion (common-ion effect) in the solution. To a lesser extent, solubility will depend on the
ionic strength of liquid solutions. The last two effects can be quantified using the equation for solubility equilibrium.
There is also a number of less common factors which may affect solubility. Solubility may depend on the crystal (or droplet) size of the solute phase (typically, solubility will increase with the decreasing crystal size for crystals much smaller than 1 μm). For highly defective crystals, solubility may increase with the increasing degree of disorder. The last two effects, although of great practical importance, are not true solubility effects because true solubility occurs at equilbrium, which requires a perfect monocrystal. For substances dissolving in an
electrochemical reaction, solubility is expected to depend on the potential of the solute phase.
Temperature
The solubility of a given solute in a given solvent typically depends on temperature. For around 95% of solid solutes, the solubility increases with temperature,John W. Hill, Ralph H. Petrucci,
General Chemistry, 2nd edition, Prentice Hall, 1999. but
gaseous solutes exhibit more complex behavior. As the temperature is raised gases usually become less soluble in water, but more soluble in organic solvents.
The chart shows solubility curves for some typical inorganic salts (all solids). Data taken from the
Handbook of Chemistry and Physics, 27th edition, Chemical Rubber Publishing Co., Cleveland, Ohio, 1943. Many salts behave like barium nitrate and 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 is sometimes referred to as "retrograte" or "inverse" solubility. Occasionally, a more complex pattern is observed, as with sodium sulfate, where the less soluble decahydrate crystal loses water of crystallization at 32 °C to form a more soluble anhydrous phase.
Organic compounds nearly always become soluble as the temperature is raised, in most solvents. The technique of
recrystallization, used for purification of solids, depends on this differences in solubility in hot and cold solvent. There are a few exceptions, such as certain
cyclodextrins.
Pressure
For condensed phases (solids and liquids), the pressure dependence of solubility is typically weak and usually neglected in practice.
Henry's law states that the solubility of a gas in a liquid is directly proportional to the
partial pressure of that gas above the liquid, which may be written as:
p = kc \,
where k is a temperature-dependent constant (for example, 769.2 L•atm/mol for
dioxygen (O2) in water at 298 K), p is the partial pressure (atm), and c is the concentration of the dissolved gas in the liquid (mol/L).
Polarity
A popular aphorism used for predicting solubility is "
Like dissolves like"Kenneth J. Williamson,
Macroscale and Microscale Organic Experiments, p40, 2nd edition, D. C, Heath, Lexington, Mass., 1994. This indicates that a solute will dissolve best in a solvent that has a similar
Chemical polarity to itself. This is a rather simplistic view, since it ignores many solvent-solute interactions, but it is a useful rule-of-thumb. For example, a very polar (
hydrophile) solute such as
urea is highly soluble in highly polar water, less soluble in fairly polar
methanol, and practically insoluble in non-polar solvents such as
benzene. In contrast, a non-polar or
lipophilic solute such as
naphthalene is insoluble in water, fairly soluble in methanol, and highly soluble in non-polar benzene.Data taken from the
Merck Index, 7th edition, Merck & Co., 1960.
Liquid solubilities also generally follow this rule. Lipophilic plant oils, such as olive oil and palm oil, dissolve in non-polar gasoline (petrol), but polar liquids like water will not mix with gasoline.
Synthetic chemists often use the different solubilities of compounds to separate and purify compounds from reaction mixtures.
Rate of dissolution
Solvation is not always an instantaneous process. It is fast when salt and sugar dissolve in water but much slower for a tablet of aspirin or a large crystal of hydrated
copper(II) sulfate. The speed at which a solid dissolves may depend on its crystalline properties (crystalline vs amorphous, crystal size) and the presence of Polymorphism (materials science). This is especially important in designing methods for controlled
drug 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. The rate of dissolution and solubility should not be confused--they are different concepts (kinetic and thermodynamic, respectively).
Quantification of solubility
Solubility is commonly expressed as a concentration, either mass concentration (g of solute per kg of solvent, or g per 100 mL of solvent) or molarity,
molality, or mole fraction or similar. 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 constants are used to describe saturated solutions of ionic compounds of relatively low solubility (see solubility equilibrium). The solubility constant is a special case of an equilibrium constant. It describes the balance between dissolved ions from the salt and undissolved salt. The solubility constant is also "applicable" (i.e. useful) to precipitation (chemistry), the reverse of the dissolving reaction. As with other equilibrium constants,
temperature can affect the numerical value of solubility constant. The solubility constant is more complicated than solubility. However, the value of this constant is generally independent of the presence of other species in the solvent.
Henry's law is used to quantify the solubility of gases in liquids as a function of the gas's partial pressure. It is a special case of a solubility equilibrium.
The Flory-Huggins solution theory is a theoretical model describing the solubility of polymers. The Hansen Solubility Parameters and the Hildebrand solubility parameters are empirical methods for the prediction of solubility. it is also possible to predict solubility from other physical constants such as the
enthalpy of fusion.
The
partition coefficient (Log P) is a measure of differential solubility of a compound in a
hydrophobe solvent (
octanol) and a hydrophile solvent (water). The logarithm of these two values enables compounds to be ranked in terms of hydrophilicity (or hydrophobicity).
Applications
The solubility of a substance is very useful when separating mixtures of compounds. For example, a mixture of salt (
sodium chloride) and silica may be separated by dissolving the salt in water, and filtering off the undissolved silica. 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 would be the synthesis of benzoic acid from phenylmagnesium bromide and
dry ice. Benzoic acid is more soluble in an organic solvent such as dichloromethane or
diethyl ether, and when shaken with this organic solvent in an separatory funnel, will preferentially dissolve in the organic layer. The other reaction products, i.e. the magnesium bromide will remain in the aqueous layer, clearly showing that separation based on solubility is achieved. (On a practical note, the benzoic acid obtained after evaporating the organic solvent should ideally be purified by recrystallizing from hot water.)
Solubility of ionic compounds in water
The solubility of a salt which ionizes in water is determined by the solubility product (Ksp) which is a constant at a given temperature.
Silver chloride is a relatively insoluble salt in water. It ionizes:
Ag+ + Cl- ↔ AgCl (s)
The solubility product of AgCl, 1.8E-10 is also the equilibrium constant of this reaction which is calculated by multiplying the concentrations of silver and chloride ions in a saturated solution, i.e. . Thus the maximum concentration of a pure solution of silver chloride possible is sqrt(1.8E-10) = 1.34 E-5 M. However, if there chloride ions were added, perhaps as a sodium chloride solution, the equilibrium will shift according to le Chatelier's principle, and silver chloride will precipitate from the solution.
SolubleInsolubleAlkali metal and
Ammonium compounds
carbonates (except Alkali metal, Ammonium and
uranyl compounds)nitrates
sulfites (except
Alkali metal and
Ammonium)
acetates (ethanoates)
phosphates (except
Alkali metal and
Ammonium compounds)
chlorides,
bromides and iodides (except
Silver, Lead,
Copper and Mercury (element))hydroxides and
oxides (except
Alkali metal, Ammonium,
Barium, Strontium and Thallium)sulfates (except
Silver, Lead, Barium, Strontium and Calcium)
sulfides (except Alkali metal,
Alkaline earth metal and Ammonium compounds)
Solubility of organic compounds
The principle outlined above under #Polarity, that
like dissolves like, is the usual guide to solubility with organic systems. For example,
vaseline will dissolve in
gasoline; both of which are lipophilic. This is because vaseline jelly consists of long carbon chains, as does the gasoline. It will not, on the other hand, dissolve in alcohol or water, since the polarity 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 by
filtration, or
solvent extraction with water.
Solid solubility
The term is often used in the field of metallurgy to refer to extent that an alloying element will dissolve into the base metal without forming a separate phase. The Solubility Line (or curve) is the line (or lines) on a
phase diagram which give the limits of solute addition. That is, the lines show the maximum amount of a component that can be added to another component and still be in solid solution. In microelectronic fabrication, solid solubility refers to the maximum concentration of impurities one can place into the substrate.
See also
External links
- ALOGPS interactive calculation of aqueous solubility of compounds at Virtual Computational Chemistry Laboratory using several algorithms
- QUANTUM web based calculation of aqueous and DMSO solubility of compounds QUANTUM web based prediction of aqueous and DMSO solubility of compounds
- ACD/Solubility DB aqueous solubility prediction
References
Solubility is a
physical property referring to the ability for a given substance, the solute, to dissolve in a solvent.
Atkins' Physical Chemistry, 7th Ed. by Julio De Paula, P.W. Atkins ISBN 0198792859 It is measured in terms of the maximum amount of solute
dissolved in a solvent at
chemical equilibrium. The resulting solution is called a saturated
solution. Certain substances are soluble in all proportions with a given solvent, such as
ethanol in water. This property is known as
miscible.
Under various conditions, the equilibrium solubility can be exceeded to give a so-called supersaturation solution, which is Metastability in molecules. The solvent is often a liquid, which can be a pure substance or a mixture. The species that dissolves, the solute, can be a gas, another liquid, or a solid. Solubilities range widely, from infinitely soluble such as ethanol in
water, to poorly soluble, such as
silver chloride in water. The term
insoluble is often applied to poorly soluble compounds, though strictly speaking there are very few cases where there is absolutely no material dissolved.
Molecular view
The process of dissolving, called
dissolution, is relatively straightforward for
covalent bond substances such as ethanol. When ethanol dissolves in water, the ethanol molecules remain intact but form new hydrogen bonds with the water. When, however, an ionic bond compound such as sodium chloride (NaCl) dissolves in water, the sodium chloride
Crystal structure Dissociation (chemistry) into separate ions which are solvation (wrapped) with a coating of water molecules. Nonetheless, NaCl is said to dissolve in water, because evaporation of the solvent returns crystalline NaCl.
Sometimes the term "dissolving" is applied to an irreversible chemical reaction, as with iron in
nitric acid, but in such a case the thermodynamic concept of solubility does not apply.
When it dissolves, a solute may form several species in the solution. For example, water above the crystals of ferrous hydroxide, Fe(OH)2, will, at equilibrium, contain Fe2+, Fe(OH)+, Fe(OH)2, Fe(OH)3- and possibly other complexes. Therefore, the solubility of ferrous hydroxide depends on pH. In general, solubility in the solvent phase can be given only for a specific solute which is thermodynamically stable, and the value of the solublity will include all the species in the solution (in the example above, all the iron-containing complexes).
Factors affecting solubility
Solubility is defined for specific
phase (matter). For example, the solubility of
aragonite and
calcite in water are expected to be different, even though both are the same chemical substance (calcium carbonate).
The solubility of one substance dissolving in another is determined by the balance of
intermolecular forces between the solvent and solute and the entropy change 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, for example, complex (chemistry)forming anions (
ligands) in liquids. Solubility will also depend on the excess (or deficiency) of a common ion (
common-ion effect) in the solution. To a lesser extent, solubility will depend on the ionic strength of liquid solutions. The last two effects can be quantified using the equation for solubility equilibrium.
There is also a number of less common factors which may affect solubility. Solubility may depend on the crystal (or droplet) size of the solute phase (typically, solubility will increase with the decreasing crystal size for crystals much smaller than 1 μm). For highly defective crystals, solubility may increase with the increasing degree of disorder. The last two effects, although of great practical importance, are not true solubility effects because true solubility occurs at equilbrium, which requires a perfect monocrystal. For substances dissolving in an electrochemical reaction, solubility is expected to depend on the potential of the solute phase.
Temperature
The solubility of a given solute in a given solvent typically depends on temperature. For around 95% of solid solutes, the solubility increases with temperature,John W. Hill, Ralph H. Petrucci,
General Chemistry, 2nd edition, Prentice Hall, 1999. but gaseous solutes exhibit more complex behavior. As the temperature is raised gases usually become less soluble in water, but more soluble in organic solvents.
The chart shows solubility curves for some typical inorganic salts (all solids). Data taken from the
Handbook of Chemistry and Physics, 27th edition, Chemical Rubber Publishing Co., Cleveland, Ohio, 1943. Many salts behave like
barium nitrate and 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 is sometimes referred to as "retrograte" or "inverse" solubility. Occasionally, a more complex pattern is observed, as with
sodium sulfate, where the less soluble decahydrate crystal loses water of crystallization at 32 °C to form a more soluble anhydrous phase.
Organic compounds nearly always become soluble as the temperature is raised, in most solvents. The technique of
recrystallization, used for purification of solids, depends on this differences in solubility in hot and cold solvent. There are a few exceptions, such as certain cyclodextrins.
Pressure
For condensed phases (solids and liquids), the pressure dependence of solubility is typically weak and usually neglected in practice.
Henry's law states that the solubility of a gas in a liquid is directly proportional to the partial pressure of that gas above the liquid, which may be written as:
p = kc \,
where k is a temperature-dependent constant (for example, 769.2 L•atm/mol for dioxygen (O2) in water at 298 K), p is the partial pressure (atm), and c is the concentration of the dissolved gas in the liquid (mol/L).
Polarity
A popular
aphorism used for predicting solubility is "
Like dissolves like"Kenneth J. Williamson,
Macroscale and Microscale Organic Experiments, p40, 2nd edition, D. C, Heath, Lexington, Mass., 1994. This indicates that a solute will dissolve best in a solvent that has a similar
Chemical polarity to itself. This is a rather simplistic view, since it ignores many solvent-solute interactions, but it is a useful rule-of-thumb. For example, a very polar (
hydrophile) solute such as
urea is highly soluble in highly polar water, less soluble in fairly polar
methanol, and practically insoluble in non-polar solvents such as
benzene. In contrast, a non-polar or lipophilic solute such as naphthalene is insoluble in water, fairly soluble in methanol, and highly soluble in non-polar benzene.Data taken from the
Merck Index, 7th edition, Merck & Co., 1960.
Liquid solubilities also generally follow this rule. Lipophilic plant oils, such as olive oil and palm oil, dissolve in non-polar gasoline (petrol), but polar liquids like water will not mix with gasoline.
Synthetic chemists often use the different solubilities of compounds to separate and purify compounds from reaction mixtures.
Rate of dissolution
Solvation is not always an instantaneous process. It is fast when salt and sugar dissolve in water but much slower for a tablet of
aspirin or a large crystal of hydrated copper(II) sulfate. The speed at which a solid dissolves may depend on its crystalline properties (crystalline vs
amorphous, crystal size) and the presence of
Polymorphism (materials science). This is especially important in designing methods for controlled drug 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. The rate of dissolution and solubility should not be confused--they are different concepts (kinetic and thermodynamic, respectively).
Quantification of solubility
Solubility is commonly expressed as a concentration, either mass concentration (g of solute per kg of solvent, or g per 100 mL of solvent) or molarity,
molality, or mole fraction or similar. 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 constants are used to describe saturated solutions of ionic compounds of relatively low solubility (see
solubility equilibrium). The solubility constant is a special case of an
equilibrium constant. It describes the balance between dissolved ions from the salt and undissolved salt. The solubility constant is also "applicable" (i.e. useful) to
precipitation (chemistry), the reverse of the dissolving reaction. As with other equilibrium constants, temperature can affect the numerical value of solubility constant. The solubility constant is more complicated than solubility. However, the value of this constant is generally independent of the presence of other species in the solvent.
Henry's law is used to quantify the solubility of gases in liquids as a function of the gas's partial pressure. It is a special case of a solubility equilibrium.
The Flory-Huggins solution theory is a theoretical model describing the solubility of polymers. The Hansen Solubility Parameters and the
Hildebrand solubility parameters are empirical methods for the prediction of solubility. it is also possible to predict solubility from other physical constants such as the enthalpy of fusion.
The partition coefficient (Log P) is a measure of differential solubility of a compound in a hydrophobe solvent (
octanol) and a
hydrophile solvent (
water). The logarithm of these two values enables compounds to be ranked in terms of hydrophilicity (or hydrophobicity).
Applications
The solubility of a substance is very useful when separating mixtures of compounds. For example, a mixture of salt (
sodium chloride) and silica may be separated by dissolving the salt in water, and filtering off the undissolved silica. 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 would be the synthesis of benzoic acid from
phenylmagnesium bromide and dry ice. Benzoic acid is more soluble in an organic solvent such as
dichloromethane or diethyl ether, and when shaken with this organic solvent in an
separatory funnel, will preferentially dissolve in the organic layer. The other reaction products, i.e. the magnesium bromide will remain in the aqueous layer, clearly showing that separation based on solubility is achieved. (On a practical note, the benzoic acid obtained after evaporating the organic solvent should ideally be purified by recrystallizing from hot water.)
Solubility of ionic compounds in water
The solubility of a salt which ionizes in water is determined by the solubility product (Ksp) which is a constant at a given temperature.
Silver chloride is a relatively insoluble salt in water. It ionizes:
Ag+ + Cl- ↔ AgCl (s)
The solubility product of AgCl, 1.8E-10 is also the equilibrium constant of this reaction which is calculated by multiplying the concentrations of silver and chloride ions in a saturated solution, i.e. . Thus the maximum concentration of a pure solution of silver chloride possible is sqrt(1.8E-10) = 1.34 E-5 M. However, if there chloride ions were added, perhaps as a sodium chloride solution, the equilibrium will shift according to
le Chatelier's principle, and silver chloride will precipitate from the solution.
SolubleInsoluble
Alkali metal and
Ammonium compounds
carbonates (except Alkali metal, Ammonium and
uranyl compounds)nitrates
sulfites (except Alkali metal and Ammonium)acetates (ethanoates)
phosphates (except Alkali metal and Ammonium compounds)
chlorides,
bromides and
iodides (except
Silver, Lead, Copper and
Mercury (element))
hydroxides and oxides (except
Alkali metal, Ammonium,
Barium,
Strontium and
Thallium)sulfates (except
Silver,
Lead, Barium,
Strontium and Calcium)sulfides (except
Alkali metal,
Alkaline earth metal and
Ammonium compounds)
Solubility of organic compounds
The principle outlined above under
#Polarity, that
like dissolves like, is the usual guide to solubility with organic systems. For example, vaseline will dissolve in gasoline; both of which are lipophilic. This is because vaseline jelly consists of long carbon chains, as does the gasoline. It will not, on the other hand, dissolve in alcohol or water, since the polarity 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 by
filtration, or
solvent extraction with water.
Solid solubility
The term is often used in the field of metallurgy to refer to extent that an alloying element will dissolve into the base metal without forming a separate phase. The Solubility Line (or curve) is the line (or lines) on a phase diagram which give the limits of solute addition. That is, the lines show the maximum amount of a component that can be added to another component and still be in solid solution. In microelectronic fabrication, solid solubility refers to the maximum concentration of impurities one can place into the substrate.
See also
External links
- ALOGPS interactive calculation of aqueous solubility of compounds at Virtual Computational Chemistry Laboratory using several algorithms
- QUANTUM web based calculation of aqueous and DMSO solubility of compounds QUANTUM web based prediction of aqueous and DMSO solubility of compounds
- ACD/Solubility DB aqueous solubility prediction
References
Solubility - Wikipedia, the free encyclopedia
Solubility is a characteristic physical property referring to the ability for a given substance, the solute, to dissolve in a solvent. [1] It is measured in terms of the maximum ...
Solubility equilibrium - Wikipedia, the free encyclopedia
Solubility equilibrium is any type chemical equilibrium between solid and dissolved states of a compound at saturation. Solubility equilibria involve application of chemical ...
solubility - definition of solubility by the Free Online Dictionary ...
Definition of solubility in the Online Dictionary. Meaning of solubility. Pronunciation of solubility. Translations of solubility. solubility synonyms, solubility antonyms.
Ionic solubility
Superficially this is a bewildering field." W.E. Dasent (1). Solubility and Hess’s Law: enthalpies. The standard argument in many A level texts (including mine (2), but I try to ...
Solubility of the hydroxides, sulphates and carbonates of the Group 2 ...
States the trends in solubility of the hydroxides, sulphates and carbonates of Group 2 elements as you go down the Group.
Problems in explaining the solubility of Group 2 compounds
Discusses some problems in the usual explanations for trends in solubility of Group 2 compounds and attempts a more accurate explanation.
Solubility Challenge
Can You Predict Solubilities of Thirty-Two Molecules Using a Database of One Hundred Reliable Measurements? J. Chem. Inf. Modeling 2008, 48, 1289-1303.
bite Sized tutorials, ionic product and solubility product
What is Ionic Product. When a salt dissolves in a solvent, usually water, the dissociated ions are present in the solvent phase in the same ...
Solubility rule - Hutchinson encyclopedia article about Solubility ...
Hutchinson encyclopedia article about Solubility rule. Solubility rule. Information about Solubility rule in the Hutchinson encyclopedia.
GCSE SCIENCE CHEMISTRY HIGH SCHOOL - Water - Solubility - Ions - All ...
gcsescience.com gcsescience.com. Water - Solubility - Ions
