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 dissolved in 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.

Characteristics of Solution[link]

• A solution is a homogenous 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 physically).

Types of solutions[link]

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[link]

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 as mixtures.

Liquid[link]

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 is a less simple example, because the solution is accompanied by a chemical reaction (formation of ions). Note also that the visible bubbles in carbonated 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 or any other salt in water 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 different solutes. They 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 illness or injury.

Solid[link]

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

• Gas in solid:
  • 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[link]

The ability of one compound to dissolve in another compound is called solubility. When a liquid is able to 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[link]

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, mole fraction, and parts per million (PPM).

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 solutions[link]

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 permanent electric dipole moment. Another distinction is whether their molecules are able to 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 of ethanol. 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.

Solution preparation from constituent ingredients[link]

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 V_A is given. Solute mass m_B = C V_A d_A /(100-C/d_B)
• Case 2: amount of solute mass m_B is given. Solvent volume V_A = m_B (100/C-1/ d_B )
• Case 3: amount (mL) of final solution volume Vt is given. Solute mass m_B = C Vt /100; Solvent volume V_A=(100/C-1/ d_B) m_B
• Case 2: solute mass is known, V_A = m_B 100/C
• Case 3: total solution volume is know, same equation as case 1. V_A=Vt; m_B = C V_A /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.
m_B = C V_A =( 2 / 100 ) x 1000 =20 g

See also[link]

Underwater diving portal

Look up solution or solute in Wiktionary, the free dictionary.

• Concentration
• Dissolution
• Molar solution
• Percentage solution
• 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[link]

Nic, M.; Jirat, J.; Kosata, B., eds. (2006–). "solution". IUPAC Compendium of Chemical Terminology (Online ed.). DOI:10.1351/goldbook.S05746. ISBN 0-9678550-9-8. http://goldbook.iupac.org/S05746.html. 

v t e Routes of administration / Dosage forms Oral Digestive tract (enteral) Solids Pill Tablet Capsule Time release technology Osmotic controlled release capsule (OROS) Liquids Solution Softgel Suspension Emulsion Syrup Elixir Tincture Hydrogel 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 pressurized Metered Dose Inhaler (pMDI) Nebulizer Vaporizer 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 or intrasynovial injection Transscleral Central nervous system Intracerebral Intrathecal Epidural Circulatory / Musculoskeletal Intravenous Intracardiac Intramuscular Intraosseous Intraperitoneal Nanocell injection Additional explanation: Mucous membranes are used by the human body to absorb the dosage for all routes of administration, except for "Dermal" and "Injection/Infusion". Administration routes can also be grouped as Topical (local effect) or Systemic (defined as Enteral = Digestive tract/Rectal, or Parenteral = All other routes).

Joel Timothy Houston (born 18 September 1979) is a musician, songwriter and pastor, and leader of the Sydney-based band Hillsong United, the youth worship band of Hillsong Church.

He is currently co-pastor at Hillsong NYC since 2010.^[1]. He is the head of the Christian worship band Hillsong UNITED, for which he sings, plays guitar and writes songs. In 2008, he became the Creative Director at Hillsong Church. He is the oldest son of the church's Senior Pastors and founders Brian and Bobbie Houston and grandson of Frank Houston (who was the Senior Pastor of Sydney Christian Life Centre which is now the City venue of Hillsong Church). He has two siblings, a brother Benjamin and a sister, Laura.^[2] Houston was also the bass player for the band Able, which was composed of Marty Sampson, Michael Guy Chislett and Luke Munns, which won the Channel V Leg Up competition in 2001. ^[3][4][5]

Biography[link]

Early life[link]

Houston began playing piano at a young age, at the suggestion of his parents. As he was not interested in piano, he soon diverted his efforts to playing guitar instead.^[6]

Hillsong United and Hillsong[link]

Houston's first debut with the Hillsong United as a vocalist was in 2002, however he had been playing bass guitar with the band for several years prior to this, and contributing various songs, including the title track from the group's debut full length live album, Everyday. As part of Hillsong United music team, Joel Houston has helped lead worship conferences in North America, South America, Africa, Europe and Asia. He has also contributed to the main Hillsong album recordings as well, which are led by worship pastor Reuben Morgan. Many of the songs he has written or co-written are sung in churches worldwide and have been translated into 32 languages, including Korean and German. His music has been featured on Hillsong albums that have quickly risen on both the Australian and American Christian music charts.[1][2] In March 2007, Hillsong United's eighth album All of the Above debuted at #6 on the ARIA charts.[3] His song, "Everyday", was ranked number 49 on the CCLI top 100 songs^{[citation needed]}. Joel Houston has been the Creative Director of Hillsong since 2008. Joel is currently co-Pastor of Hillsong NYC with Carl Lentz.^[1]

Discography[link]

Albums on which Houston has written and performed songs:

External links[link]

• Christianity Today interview
• "The Story Behind All of the Above" - Written by Joel Houston
• SongDiscovery.com interviews Joel Houston [4], [5]
• A Passion for His Presence article at Beliefnet
• Fresh 103.2 Interview
• BBC Heart-throb rock gods united in song
• The Bulletin interview and photo gallery

References[link]