solution

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Solution From Wikipedia, the free encyclopedia This article is about chemical solutions. For other uses, see Solution (disambiguation). Making a saline water solution by dissolving table salt (NaCl) in water. The salt is the solute and the water the solvent. In chemistry, a solution is a homogeneous mixture composed of only one phase. In such a mixture, a solute is a substance dissolvedin another substance, known as a solvent. The solvent does the dissolving. The solution more or less takes on the characteristics of the solvent including its phase, and the solvent is commonly the major fraction of the mixture. The concentration of a solute in a solution is a measure of how much of that solute is dissolved in the solvent.

Contents [hide]

1 Characteristics

2 Types

2.1 Gas

2.2 Liquid

2.3 Solid

3 Solubility

4 Properties

5 Liquid5.1 Preparation from constituent ingredients

6 See also

7 References

Characteristics[edit]

A solution is a homogeneous mixture

The particles of solute in solution cannot be seen by naked eye.

The solution does not allow beam of light to scatter.

A solution is stable.

The solute from the solution cannot be separated by filtration (or mechanically).

Types[edit] Homogeneous means that the components of the mixture form a single phase. The properties of the mixture (such as concentration, temperature, and density) can be uniformly distributed through the volume but only in absence of diffusion phenomena or after their completion. Usually, the substance present in the greatest amount is considered the solvent. Solvents can be gases, liquids or solids. One or more components present in the solution other than the solvent are called solutes. The solution has the same physical state as the solvent.

Gas[edit] If the solvent is a gas, only gases are dissolved under a given set of conditions. An example of a gaseous solution is air (oxygen and other gases dissolved in nitrogen). Since interactions between molecules play almost no role, dilute gases form rather trivial solutions. In part of the literature, they are not even classified as solutions, but addressed asmixtures.

Liquid[edit] If the solvent is a liquid, then gases, liquids, and solids can be dissolved. Here are some examples:

Gas in liquid:

Oxygen in water

Carbon dioxide in water – a less simple example, because the solution is accompanied by a chemical reaction (formation of ions). Note also that the visible bubbles incarbonated water are not the dissolved gas, but only an effervescence of carbon dioxide that has come out of solution; the dissolved gas itself is not visible since it is dissolved on a molecular level.

Liquid in liquid:

The mixing of two or more substances of the same chemistry but different concentrations to form a constant. (Homogenization of solutions)

Alcoholic beverages are basically solutions of ethanol in water.

Solid in liquid:

Sucrose (table sugar) in water

Sodium chloride (table salt) or any other salt in water, which forms an electrolyte: When dissolving, salt dissociates into ions.

Counterexamples are provided by liquid mixtures that are not homogeneous: colloids, suspensions, emulsions are not considered solutions.

Body fluids are examples for complex liquid solutions, containing many solutes. Many of these are electrolytes, since they contain solute ions, such as potassium. Furthermore, they contain solute molecules like sugar and urea. Oxygen and carbon dioxide are also essential components of blood chemistry, where significant changes in their concentrations may be a sign of severe illness or injury.

Solid[edit] If the solvent is a solid, then gases, liquids and solids can be dissolved.

Gas in solids:

Hydrogen dissolves rather well in metals, especially in palladium; this is studied as a means of hydrogen storage.

Liquid in solid:

Mercury in gold, forming an amalgam

Hexane in paraffin wax

Solid in solid:

Steel, basically a solution of carbon atoms in a crystalline matrix of iron atoms.

Alloys like bronze and many others.

Polymers containing plasticizers.

Solubility[edit] Main article: Solubility Main article: Solvation The ability of one compound to dissolve in another compound is called solubility. When a liquid can completely dissolve in another liquid the two liquids are miscible. Two substances that can never mix to form a solution are called immiscible.

All solutions have a positive entropy of mixing. The interactions between different molecules or ions may be energetically favored or not. If interactions are unfavorable, then the free energy decreases with increasing solute concentration. At some point the energy loss outweighs the entropy gain, and no more solute particles can be dissolved; the solution is said to be saturated. However, the point at which a solution can become saturated can change significantly with different environmental factors, such as temperature, pressure, and contamination. For some solute-solvent combinations a supersaturated solution can be prepared by raising the solubility (for example by increasing the temperature) to dissolve more solute, and then lowering it (for example by cooling).

Usually, the greater the temperature of the solvent, the more of a given solid solute it can dissolve. However, most gases and some compounds exhibit solubilities that decrease with increased temperature. Such behavior is a result of an exothermic enthalpy of solution. Some surfactants exhibit this behaviour. The solubility of liquids in liquids is generally less temperature-sensitive than that of solids or gases.

Properties[edit] The physical properties of compounds such as melting point and boiling point change when other compounds are added. Together they are called colligative properties. There are several ways to quantify the amount of one compound dissolved in the other compounds collectively called concentration. Examples include molarity, volume fraction, and mole fraction.

The properties of ideal solutions can be calculated by the linear combination of the properties of its components. If both solute and solvent exist in equal quantities (such as in a 50% ethanol, 50% water solution), the concepts of "solute" and "solvent" become less relevant, but the substance that is more often used as a solvent is normally designated as the solvent (in this example, water).

Liquid[edit] See also: Solvent#Solvent classifications In principle, all types of liquids can behave as solvents: liquid noble gases, molten metals, molten salts, molten covalent networks, and molecular liquids. In the practice of chemistry and biochemistry, most solvents are molecular liquids. They can be classified into polar and non-polar, according to whether their molecules possess a permanentelectric dipole moment. Another distinction is whether their molecules can form hydrogen bonds (protic and aprotic solvents). Water, the most commonly used solvent, is both polar and sustains hydrogen bonds.

Water is a good solvent because the molecules are polar and capable of forming hydrogen bonds(1). Salts dissolve in polar solvents, forming positive and negative ions that are attracted to the negative and positive ends of the solvent molecule, respectively. If the solvent is water, hydration occurs when the charged solute ions become surrounded by water molecules. A standard example is aqueous saltwater. Such solutions are called electrolytes.

For non-ionic solutes, the general rule is: like dissolves like.

Polar solutes dissolve in polar solvents, forming polar bonds or hydrogen bonds. As an example, all alcoholic beverages are aqueous solutions ofethanol. On the other hand, non-polar solutes dissolve better in non-polar solvents. Examples are hydrocarbons such as oil and grease that easily mix with each other, while being incompatible with water.

An example for the immiscibility of oil and water is a leak of petroleum from a damaged tanker, that does not dissolve in the ocean water but rather floats on the surface.

Preparation from constituent ingredients[edit] It is common practice in laboratories to make a solution directly from its constituent ingredients. There are three cases in practical calculation:

Case 1: amount of solvent volume is given.

Case 2: amount of solute mass is given.

Case 3: amount of final solution volume is given.

In the following equations, A is solvent, B is solute, and C is concentration. Solute volume contribution is considered through ideal solution model.

Case 1: amount (mL) of solvent volume VA is given. Solute mass mB = C VA dA /(100-C/dB)

Case 2: amount of solute mass mB is given. Solvent volume VA = mB (100/C-1/ dB )

Case 3: amount (mL) of final solution volume Vt is given. Solute mass mB = C Vt /100; Solvent volume VA=(100/C-1/ dB) mB

Case 2: solute mass is known, VA = mB 100/C

Case 3: total solution volume is know, same equation as case 1. VA=Vt; mB = C VA /100

Example: Make 2 g/100mL of NaCl solution with 1 L water Water (properties). The density of resulting solution is considered to be equal to that of water, statement holding especially for dilute solutions, so the density information is not required.

mB = C VA =( 2 / 100 ) x 1000 =20 g

See also[edit] Underwater diving portal Look up solution or solute in Wiktionary, the free dictionary.

Solvation

Molar solution

Percentage solution (disambiguation)

Solubility equilibrium

Stock solution

Total dissolved solids is a common term in a range of disciplines, and can have different meanings depending on the analytical method used. In water quality, it refers to the amount of residue remaining after evaporation of water from a sample.

Upper critical solution temperature

Lower critical solution temperature

Coil-globule transition

References[edit]

IUPAC, Compendium of Chemical Terminology, 2nd ed. (the "Gold Book") (1997). Online corrected version: (2006–) "solution".

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Time release technology

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Liquids

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Herbal tea

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Molecular encapsulation

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Solution

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Smoking device

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Liquids

Anaesthetic vaporizer

Vaporizer

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metered-dose inhaler (MDI)

Gas

Oxygen mask

Oxygen concentrator

Anaesthetic machine

Relative analgesia machine

Ophthalmic /

Otologic / Nasal

Nasal spray

Ear drops

Eye drops

Ointment

Hydrogel

Nanosphere suspension

Mucoadhesive microdisc (microsphere tablet)

Urogenital

Ointment

Pessary (vaginal suppository)

Vaginal ring

Vaginal douche

Intrauterine device (IUD)

Extra-amniotic infusion

Intravesical infusion

Rectal (enteral)

Ointment

Suppository

Enema

Solution

Hydrogel

Murphy drip

Nutrient enema

Dermal

Ointment

Liniment

Paste

Film

Hydrogel

Liposomes

Transfersome vesicles

Cream

Lotion

Lip balm

Medicated shampoo

Dermal patch

Transdermal patch

Transdermal spray

Jet injector

Injection / Infusion

(into tissue/blood) Skin

Intradermal

Subcutaneous

Transdermal implant

Organs

Intracavernous

Intravitreal

Intra-articular injection

Transscleral

Central nervous system

Intracerebral

Intrathecal

Epidural

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Intravenous

Intracardiac

Intramuscular

Intraosseous

Intraperitoneal

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Solution

From Wikipedia, the free encyclopedia This article is about chemical solutions. For other uses, see Solution (disambiguation). Making a saline water solution by dissolving table salt (NaCl) in water. The salt is the solute and the water the solvent. In chemistry, a solution is a homogeneous mixture composed of only one phase. In such a mixture, a solute is a substance dissolvedin another substance, known as a solvent. The solvent does the dissolving. The solution more or less takes on the characteristics of the solvent including its phase, and the solvent is commonly the major fraction of the mixture. The concentration of a solute in a solution is a measure of how much of that solute is dissolved in the solvent.

Contents [hide]

1 Characteristics

2 Types

2.1 Gas

2.2 Liquid

2.3 Solid

3 Solubility

4 Properties

5 Liquid5.1 Preparation from constituent ingredients

6 See also

7 References

Characteristics[edit]

A solution is a homogeneous mixture

The particles of solute in solution cannot be seen by naked eye.

The solution does not allow beam of light to scatter.

A solution is stable.

The solute from the solution cannot be separated by filtration (or mechanically).

Types[edit] Homogeneous means that the components of the mixture form a single phase. The properties of the mixture (such as concentration, temperature, and density) can be uniformly distributed through the volume but only in absence of diffusion phenomena or after their completion. Usually, the substance present in the greatest amount is considered the solvent. Solvents can be gases, liquids or solids. One or more components present in the solution other than the solvent are called solutes. The solution has the same physical state as the solvent.

Gas[edit] If the solvent is a gas, only gases are dissolved under a given set of conditions. An example of a gaseous solution is air (oxygen and other gases dissolved in nitrogen). Since interactions between molecules play almost no role, dilute gases form rather trivial solutions. In part of the literature, they are not even classified as solutions, but addressed asmixtures.

Liquid[edit] If the solvent is a liquid, then gases, liquids, and solids can be dissolved. Here are some examples:

Gas in liquid:

Oxygen in water

Carbon dioxide in water – a less simple example, because the solution is accompanied by a chemical reaction (formation of ions). Note also that the visible bubbles incarbonated water are not the dissolved gas, but only an effervescence of carbon dioxide that has come out of solution; the dissolved gas itself is not visible since it is dissolved on a molecular level.

Liquid in liquid:

The mixing of two or more substances of the same chemistry but different concentrations to form a constant. (Homogenization of solutions)

Alcoholic beverages are basically solutions of ethanol in water.

Solid in liquid:

Sucrose (table sugar) in water

Sodium chloride (table salt) or any other salt in water, which forms an electrolyte: When dissolving, salt dissociates into ions.

Counterexamples are provided by liquid mixtures that are not homogeneous: colloids, suspensions, emulsions are not considered solutions.

Body fluids are examples for complex liquid solutions, containing many solutes. Many of these are electrolytes, since they contain solute ions, such as potassium. Furthermore, they contain solute molecules like sugar and urea. Oxygen and carbon dioxide are also essential components of blood chemistry, where significant changes in their concentrations may be a sign of severe illness or injury.

Solid[edit] If the solvent is a solid, then gases, liquids and solids can be dissolved.

Gas in solids:

Hydrogen dissolves rather well in metals, especially in palladium; this is studied as a means of hydrogen storage.

Liquid in solid:

Mercury in gold, forming an amalgam

Hexane in paraffin wax

Solid in solid:

Steel, basically a solution of carbon atoms in a crystalline matrix of iron atoms.

Alloys like bronze and many others.

Polymers containing plasticizers.

Solubility[edit] Main article: Solubility Main article: Solvation The ability of one compound to dissolve in another compound is called solubility. When a liquid can completely dissolve in another liquid the two liquids are miscible. Two substances that can never mix to form a solution are called immiscible.

All solutions have a positive entropy of mixing. The interactions between different molecules or ions may be energetically favored or not. If interactions are unfavorable, then the free energy decreases with increasing solute concentration. At some point the energy loss outweighs the entropy gain, and no more solute particles can be dissolved; the solution is said to be saturated. However, the point at which a solution can become saturated can change significantly with different environmental factors, such as temperature, pressure, and contamination. For some solute-solvent combinations a supersaturated solution can be prepared by raising the solubility (for example by increasing the temperature) to dissolve more solute, and then lowering it (for example by cooling).

Usually, the greater the temperature of the solvent, the more of a given solid solute it can dissolve. However, most gases and some compounds exhibit solubilities that decrease with increased temperature. Such behavior is a result of an exothermic enthalpy of solution. Some surfactants exhibit this behaviour. The solubility of liquids in liquids is generally less temperature-sensitive than that of solids or gases.

Properties[edit] The physical properties of compounds such as melting point and boiling point change when other compounds are added. Together they are called colligative properties. There are several ways to quantify the amount of one compound dissolved in the other compounds collectively called concentration. Examples include molarity, volume fraction, and mole fraction.

The properties of ideal solutions can be calculated by the linear combination of the properties of its components. If both solute and solvent exist in equal quantities (such as in a 50% ethanol, 50% water solution), the concepts of "solute" and "solvent" become less relevant, but the substance that is more often used as a solvent is normally designated as the solvent (in this example, water).

Liquid[edit] See also: Solvent#Solvent classifications In principle, all types of liquids can behave as solvents: liquid noble gases, molten metals, molten salts, molten covalent networks, and molecular liquids. In the practice of chemistry and biochemistry, most solvents are molecular liquids. They can be classified into polar and non-polar, according to whether their molecules possess a permanentelectric dipole moment. Another distinction is whether their molecules can form hydrogen bonds (protic and aprotic solvents). Water, the most commonly used solvent, is both polar and sustains hydrogen bonds.

Water is a good solvent because the molecules are polar and capable of forming hydrogen bonds(1). Salts dissolve in polar solvents, forming positive and negative ions that are attracted to the negative and positive ends of the solvent molecule, respectively. If the solvent is water, hydration occurs when the charged solute ions become surrounded by water molecules. A standard example is aqueous saltwater. Such solutions are called electrolytes.

For non-ionic solutes, the general rule is: like dissolves like.

Polar solutes dissolve in polar solvents, forming polar bonds or hydrogen bonds. As an example, all alcoholic beverages are aqueous solutions ofethanol. On the other hand, non-polar solutes dissolve better in non-polar solvents. Examples are hydrocarbons such as oil and grease that easily mix with each other, while being incompatible with water.

An example for the immiscibility of oil and water is a leak of petroleum from a damaged tanker, that does not dissolve in the ocean water but rather floats on the surface.

Preparation from constituent ingredients[edit] It is common practice in laboratories to make a solution directly from its constituent ingredients. There are three cases in practical calculation:

Case 1: amount of solvent volume is given.

Case 2: amount of solute mass is given.

Case 3: amount of final solution volume is given.

In the following equations, A is solvent, B is solute, and C is concentration. Solute volume contribution is considered through ideal solution model.

Case 1: amount (mL) of solvent volume VA is given. Solute mass mB = C VA dA /(100-C/dB)

Case 2: amount of solute mass mB is given. Solvent volume VA = mB (100/C-1/ dB )

Case 3: amount (mL) of final solution volume Vt is given. Solute mass mB = C Vt /100; Solvent volume VA=(100/C-1/ dB) mB

Case 2: solute mass is known, VA = mB 100/C

Case 3: total solution volume is know, same equation as case 1. VA=Vt; mB = C VA /100

Example: Make 2 g/100mL of NaCl solution with 1 L water Water (properties). The density of resulting solution is considered to be equal to that of water, statement holding especially for dilute solutions, so the density information is not required.

mB = C VA =( 2 / 100 ) x 1000 =20 g

See also[edit] Underwater diving portal Look up solution or solute in Wiktionary, the free dictionary.

Solvation

Molar solution

Percentage solution (disambiguation)

Solubility equilibrium

Stock solution

Total dissolved solids is a common term in a range of disciplines, and can have different meanings depending on the analytical method used. In water quality, it refers to the amount of residue remaining after evaporation of water from a sample.

Upper critical solution temperature

Lower critical solution temperature

Coil-globule transition

References[edit]

IUPAC, Compendium of Chemical Terminology, 2nd ed. (the "Gold Book") (1997). Online corrected version: (2006–) "solution".

[show]

v

t

e

Articles related to solutions [hide]

v

t

e

Routes of administration / Dosage forms Oral Digestive tract(enteral) Solids

Pill

Tablet

Capsule

Time release technology

Osmotic delivery system (OROS)

Liquids

Elixir

Emulsion

Herbal tea

Hydrogel

Molecular encapsulation

Softgel

Solution

Suspension

Syrup

Tincture

Buccal(Sublabial)Sublingual Solids

Orally disintegrating tablet (ODT)

Film

Lollipop

Lozenges

Chewing gum

Liquids

Mouthwash

Toothpaste

Ointment

Oral spray

Respiratory

tract Solids

Smoking device

Dry powder inhaler (DPI)

Liquids

Anaesthetic vaporizer

Vaporizer

Nebulizer

metered-dose inhaler (MDI)

Gas

Oxygen mask

Oxygen concentrator

Anaesthetic machine

Relative analgesia machine

Ophthalmic /

Otologic / Nasal

Nasal spray

Ear drops

Eye drops

Ointment

Hydrogel

Nanosphere suspension

Mucoadhesive microdisc (microsphere tablet)

Urogenital

Ointment

Pessary (vaginal suppository)

Vaginal ring

Vaginal douche

Intrauterine device (IUD)

Extra-amniotic infusion

Intravesical infusion

Rectal (enteral)

Ointment

Suppository

Enema

Solution

Hydrogel

Murphy drip

Nutrient enema

Dermal

Ointment

Liniment

Paste

Film

Hydrogel

Liposomes

Transfersome vesicles

Cream

Lotion

Lip balm

Medicated shampoo

Dermal patch

Transdermal patch

Transdermal spray

Jet injector

Injection / Infusion

(into tissue/blood) Skin

Intradermal

Subcutaneous

Transdermal implant

Organs

Intracavernous

Intravitreal

Intra-articular injection

Transscleral

Central nervous system

Intracerebral

Intrathecal

Epidural

Circulatory /Musculoskeletal

Intravenous

Intracardiac

Intramuscular

Intraosseous

Intraperitoneal

Nanocell injection

[show]

v

t

e

Routes of administration by organ system

solution