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Acid
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This article is about acids in chemistry. For the drug, see Lysergic acid diethylamide. For other uses, see Acid (disambiguation).
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Zinc, a typical metal, reacting with hydrochloric acid, a typical acid
Acids and bases
pH
Reaction
Titration
Extraction
Dissociation constant (acid)
Acid strength
Acidity function
Buffer solutions
Proton affinity
Self-ionization of water
Amphoterism
Acid types
Brønsted
Lewis
Mineral
Organic
Strong
Superacids
Weak
Monobasic acid
Dibasic acid
Tribasic acid
Solid
Base types
Brønsted
Lewis
Organic
Strong
Superbases
Non-nucleophilic
Weak
v
t
e
An acid is a molecule or ion capable of donating a hydron (proton or hydrogen ion H+), or, alternatively, capable of forming a covalent bond with an electron pair (a Lewis acid).[1]
The first category of acids is the proton donors or Brønsted acids. In the special case of aqueous solutions, proton donors form the hydronium ion H3O+ and are known as Arrhenius acids. Brønsted and Lowry generalized the Arrhenius theory to include non-aqueous solvents. A Brønsted or Arrhenius acid usually contains a hydrogen atom bonded to a chemical structure that is still energetically favorable after loss of H+.
Aqueous Arrhenius acids have characteristic properties which provide a practical description of an acid.[2] Acids form aqueous solutions with a sour taste, can turn blue litmus red, and react with bases and certain metals (like calcium) to form salts. The word acid is derived from the Latin acidus/acēre meaning sour.[3] An aqueous solution of an acid has a pH less than 7 and is colloquially also referred to as 'acid' (as in 'dissolved in acid'), while the strict definition refers only to the solute.[1] A lower pH means a higher acidity, and thus a higher concentration of positive hydrogen ions in the solution. Chemicals or substances having the property of an acid are said to be acidic.
Common aqueous acids include hydrochloric acid (a solution of hydrogen chloride which is found in gastric acid in the stomach and activates digestive enzymes), acetic acid (vinegar is a dilute aqueous solution of this liquid), sulfuric acid (used in car batteries), and citric acid (found in citrus fruits). As these examples show, acids (in the colloquial sense) can be solutions or pure substances, and can be derived from acids (in the strict[1] sense) that are solids, liquids, or gases. Strong acids and some concentrated weak acids are corrosive, but there are exceptions such as carboranes and boric acid.
The second category of acids are Lewis acids, which form a covalent bond with an electron pair. An example is boron trifluoride (BF3), whose boron atom has a vacant orbital which can form a covalent bond by sharing a lone pair of electrons on an atom in a base, for example the nitrogen atom in ammonia (NH3). Lewis considered this as a generalization of the Brønsted definition, so that an acid is a chemical species that accepts electron pairs either directly or by releasing protons (H+) into the solution, which then accept electron pairs. However, hydrogen chloride, acetic acid, and most other Brønsted-Lowry acids cannot form a covalent bond with an electron pair and are therefore not Lewis acids.[4] Conversely, many Lewis acids are not Arrhenius or Brønsted-Lowry acids. In modern terminology, an acid is implicitly a Brønsted acid and not a Lewis acid, since chemists almost always refer to a Lewis acid explicitly as a Lewis acid.[4]
Contents
[hide]
1 Definitions and concepts
1.1 Arrhenius acids
1.2 Brønsted–Lowry acids
1.3 Lewis acids
2 Dissociation and equilibrium
3 Nomenclature
4 Acid strength
5 Chemical characteristics
5.1 Monoprotic acids
5.2 Polyprotic acids
5.3 Neutralization
5.4 Weak acid–weak base equilibrium
6 Applications of acids
6.1 Acid catalysis
7 Biological occurrence
8 Common acids
8.1 Mineral acids (inorganic acids)
8.2 Sulfonic acids
8.3 Carboxylic acids
8.4 Halogenated carboxylic acids
8.5 Vinylogous carboxylic acids
8.6 Nucleic acids
9 References
10 External links
Definitions and concepts
Main article: Acid–base reaction
Modern definitions are concerned with the fundamental chemical reactions common to all acids.
Most acids encountered in everyday life are aqueous solutions, or can be dissolved in water, so the Arrhenius and Brønsted-Lowry definitions are the most relevant.
The Brønsted-Lowry definition is the most widely used definition; unless otherwise specified, acid-base reactions are assumed to involve the transfer of a proton (H+) from an acid to a base.
Hydronium ions are acids according to all three definitions. Interestingly, although alcohols and amines can be Brønsted-Lowry acids, they can also function as Lewis bases due to the lone pairs of electrons on their oxygen and nitrogen atoms.
Arrhenius acids
Svante Arrhenius
The Swedish chemist Svante Arrhenius attributed the properties of acidity to hydrogen ions (H+) or protons in 1884. An Arrhenius acid is a substance that, when added to water, increases the concentration of H+ ions in the water.[4][5] Note that chemists often write H+(aq) and refer to the hydrogen ion when describing acid-base reactions but the free hydrogen nucleus, a proton, does not exist alone in water, it exists as the hydronium ion, H3O+. Thus, an Arrhenius acid can also be described as a substance that increases the concentration of hydronium ions when added to water. Examples include molecular substances such as HCl and acetic acid.
An Arrhenius base, on the other hand, is a substance which increases the concentration of hydroxide (OH−) ions when dissolved in water. This decreases the concentration of hydronium because the ions react to form H2O molecules:
H3O+
(aq) + OH−
(aq) ⇌ H2O(l) + H2O(l)
Due to this equilibrium, any increase in the concentration of hydronium is accompanied by a decrease in the concentration of hydroxide. Thus, an Arrhenius acid could also be said to be one that decreases hydroxide concentration, while an Arrhenius base increases it.
In an acidic solution, the concentration of hydronium ions is greater than 10−7 moles per liter. Since pH is defined as the negative logarithm of the concentration of hydronium ions, acidic solutions thus have a pH of less than 7.
Brønsted–Lowry acids
Main article: Brønsted–Lowry acid–base theory
Acetic acid, a weak acid, donates a proton (hydrogen ion, highlighted in green) to water in an equilibrium reaction to give the acetate ion and the hydronium ion. Red: oxygen, black: carbon, white: hydrogen.
While the Arrhenius concept is useful for describing many reactions, it is also quite limited in its scope. In 1923 chemists Johannes Nicolaus Brønsted and Thomas Martin Lowry independently recognized that acid-base reactions involve the transfer of a proton. A Brønsted-Lowry acid (or simply Brønsted acid) is a species that donates a proton to a Brønsted-Lowry base.[5] Brønsted-Lowry acid-base theory has several advantages over Arrhenius theory. Consider the following reactions of acetic acid (CH3COOH), the organic acid that gives vinegar its characteristic taste:
CH
3COOH + H
2O ⇌ CH
3COO−
+ H
3O+
CH
3COOH + NH
3 ⇌ CH
3COO−
+ NH+
4
Both theories easily describe the first reaction: CH3COOH acts as an Arrhenius acid because it acts as a source of H3O+ when dissolved in water, and it acts as a Brønsted acid by donating a proton to water. In the second example CH3COOH undergoes the same transformation, in this case donating a proton to ammonia (NH3), but does not relate to the Arrhenius definition of an acid because the reaction does not produce hydronium. Nevertheless, CH3COOH is both an Arrhenius and a Brønsted-Lowry acid.
Brønsted-Lowry theory can be used to describe reactions of molecular compounds in nonaqueous solution or the gas phase. Hydrogen chloride (HCl) and ammonia combine under several different conditions to form ammonium chloride, NH4Cl. In aqueous solution HCl behaves as hydrochloric acid and exists as hydronium and chloride ions. The following reactions illustrate the limitations of Arrhenius's definition:
H3O+
(aq) + Cl−
(aq) + NH3 → Cl−
(aq) + NH+
4(aq) + H2O
HCl(benzene) + NH3(benzene) → NH4Cl(s)
HCl(g) + NH3(g) → NH4Cl(s)
As with the acetic acid reactions, both definitions work for the first example, where water is the solvent and hydronium ion is formed by the HCl solute. The next two reactions do not involve the formation of ions but are still proton-transfer reactions. In the second reaction hydrogen chloride and ammonia (dissolved in benzene) react to form solid ammonium chloride in a benzene solvent and in the third gaseous HCl and NH3 combine to form the solid.
Lewis acids
Main article: Lewis acids and bases
A third, only marginally related concept was proposed in 1923 by Gilbert N. Lewis, which includes reactions with acid-base characteristics that do not involve a proton transfer. A Lewis acid is a species that accepts a pair of electrons from another species; in other words, it is an electron pair acceptor.[5] Brønsted acid-base reactions are proton transfer reactions while Lewis acid-base reactions are electron pair transfers. Many Lewis acids are not Brønsted-Lowry acids. Contrast how the following reactions are described in terms of acid-base chemistry:
In the first reaction a fluoride ion, F−, gives up an electron pair to boron trifluoride to form the product tetrafluoroborate. Fluoride "loses" a pair of valence electrons because the electrons shared in the B—F bond are located in the region of space between the two atomic nuclei and are therefore more distant from the fluoride nucleus than they are in the lone fluoride ion. BF3 is a Lewis acid because it accepts the electron pair from fluoride. This reaction cannot be described in terms of Brønsted theory because there is no proton transfer. The second reaction can be described using either theory. A proton is transferred from an unspecified Brønsted acid to ammonia, a Brønsted base; alternatively, ammonia acts as a Lewis base and transfers a lone pair of electrons to form a bond with a hydrogen ion. The species that gains the electron pair is the Lewis acid; for example, the oxygen atom in H3O+ gains a pair of electrons when one of the H—O bonds is broken and the electrons shared in the bond become localized on oxygen. Depending on the context, a Lewis acid may also be described as an oxidizer or an electrophile. Organic Brønsted acids, such as acetic, citric, or oxalic acid, are not Lewis acids.[4] They dissociate in water to produce a Lewis acid, H+, but at the same time also yield an equal amount of a Lewis base (acetate, citrate, or oxalate, respectively, for the acids mentioned). Few, if any, of the acids discussed in the following are Lewis acids.
Dissociation and equilibrium
Reactions of acids are often generalized in the form HA ⇌ H+ + A−, where HA represents the acid and A− is the conjugate base. This reaction is referred to as protolysis. The protonated form (HA) of an acid is also sometimes referred to as the free acid.[6]
Acid-base conjugate pairs differ by one proton, and can be interconverted by the addition or removal of a proton (protonation and deprotonation, respectively). Note that the acid can be the charged species and the conjugate base can be neutral in which case the generalized reaction scheme could be written as HA+ ⇌ H+ + A. In solution there exists an equilibrium between the acid and its conjugate base. The equilibrium constant K is an expression of the equilibrium concentrations of the molecules or the ions in solution. Brackets indicate concentration, such that [H2O] means the concentration of H2O. The acid dissociation constant Ka is generally used in the context of acid-base reactions. The numerical value of Ka is equal to the product of the concentrations of the products divided by the concentration of the reactants, where the reactant is the acid (HA) and the products are the conjugate base and H+.
K a = [ H + ] [ A − ] [ HA ] {\displaystyle K_{a}={\frac {\ce {[H+][A^{-}]}}{\ce {[HA]}}}}
The stronger of two acids will have a higher Ka than the weaker acid; the ratio of hydrogen ions to acid will be higher for the stronger acid as the stronger acid has a greater tendency to lose its proton. Because the range of possible values for Ka spans many orders of magnitude, a more manageable constant, pKa is more frequently used, where pKa = −log10 Ka. Stronger acids have a smaller pKa than weaker acids. Experimentally determined pKa at 25 °C in aqueous solution are often quoted in textbooks and reference material.
Nomenclature
In the classical naming system, acids are named according to their anions. That ionic suffix is dropped and replaced with a new suffix (and sometimes prefix), according to the table below. For example, HCl has chloride as its anion, so the -ide suffix makes it take the form hydrochloric acid. In the IUPAC naming system, "aqueous" is simply added to the name of the ionic compound. Thus, for hydrogen chloride, the IUPAC name would be aqueous hydrogen chloride. The prefix "hydro-" is added only if the acid is made up of just hydrogen and one other element.
Classical naming system:
Anion prefix
Anion suffix
Acid prefix
Acid suffix
Example
per ate per ic acid perchloric acid (HClO4)
ate ic acid chloric acid (HClO3)
ite ous acid chlorous acid (HClO2)
hypo ite hypo ous acid hypochlorous acid (HClO)
ide hydro ic acid hydrochloric acid (HCl)
Acid strength
Main article: Acid strength
The strength of an acid refers to its ability or tendency to lose a proton. A strong acid is one that completely dissociates in water; in other words, one mole of a strong acid HA dissolves in water yielding one mole of H+ and one mole of the conjugate base, A−, and none of the protonated acid HA. In contrast, a weak acid only partially dissociates and at equilibrium both the acid and the conjugate base are in solution. Examples of strong acids are hydrochloric acid (HCl), hydroiodic acid (HI), hydrobromic acid (HBr), perchloric acid (HClO4), nitric acid (HNO3) and sulfuric acid (H2SO4). In water each of these essentially ionizes 100%. The stronger an acid is, the more easily it loses a proton, H+. Two key factors that contribute to the ease of deprotonation are the polarity of the H—A bond and the size of atom A, which determines the strength of the H—A bond. Acid strengths are also often discussed in terms of the stability of the conjugate base.
Stronger acids have a larger Ka and a more negative pKa than weaker acids.
Sulfonic acids, which are organic oxyacids, are a class of strong acids. A common example is toluenesulfonic acid (tosylic acid). Unlike sulfuric acid itself, sulfonic acids can be solids. In fact, polystyrene functionalized into polystyrene sulfonate is a solid strongly acidic plastic that is filterable.
Superacids are acids stronger than 100% sulfuric acid. Examples of superacids are fluoroantimonic acid, magic acid and perchloric acid. Superacids can permanently protonate water to give ionic, crystalline hydronium "salts". They can also quantitatively stabilize carbocations.
While Ka measures the strength of an acid compound, the strength of an aqueous acid solution is measured by pH, which is an indication of the concentration of hydronium in the solution. The pH of a simple solution of an acid compound in water is determined by the dilution of the compound and the compound's Ka.
Chemical characteristics
Monoprotic acids
Monoprotic acids are those acids that are able to donate one proton per molecule during the process of dissociation (sometimes called ionization) as shown below (symbolized by HA):
HA(aq) + H2O(l) ⇌ H3O+
(aq) + A−
(aq) Ka
Common examples of monoprotic acids in mineral acids include hydrochloric acid (HCl) and nitric acid (HNO3). On the other hand, for organic acids the term mainly indicates the presence of one carboxylic acid group and sometimes these acids are known as monocarboxylic acid. Examples in organic acids include formic acid (HCOOH), acetic acid (CH3COOH) and benzoic acid (C6H5COOH).
See also: Acid dissociation constant § Monoprotic acids
Polyprotic acids
Polyprotic acids, also known as polybasic acids, are able to donate more than one proton per acid molecule, in contrast to monoprotic acids that only donate one proton per molecule. Specific types of polyprotic acids have more specific names, such as diprotic acid (two potential protons to donate) and triprotic acid (three potential protons to donate).
A diprotic acid (here symbolized by H2A) can undergo one or two dissociations depending on the pH. Each dissociation has its own dissociation constant, Ka1 and Ka2.
H2A(aq) + H2O(l) ⇌ H3O+
(aq) + HA−
(aq) Ka1
HA−
(aq) + H2O(l) ⇌ H3O+
(aq) + A2−
(aq) Ka2
The first dissociation constant is typically greater than the second; i.e., Ka1 > Ka2. For example, sulfuric acid (H2SO4) can donate one proton to form the bisulfate anion (HSO−
4), for which Ka1 is very large; then it can donate a second proton to form the sulfate anion (SO2−
4), wherein the Ka2 is intermediate strength. The large Ka1 for the first dissociation makes sulfuric a strong acid. In a similar manner, the weak unstable carbonic acid (H2CO3) can lose one proton to form bicarbonate anion (HCO−
3) and lose a second to form carbonate anion (CO2−
3). Both Ka values are small, but Ka1 > Ka2 .
A triprotic acid (H3A) can undergo one, two, or three dissociations and has three dissociation constants, where Ka1 > Ka2 > Ka3.
H3A(aq) + H2O(l) ⇌ H3O+
(aq) + H2A−
(aq) Ka1
H2A−
(aq) + H2O(l) ⇌ H3O+
(aq) + HA2−
(aq) Ka2
HA2−
(aq) + H2O(l) ⇌ H3O+
(aq) + A3−
(aq) Ka3
An inorganic example of a triprotic acid is orthophosphoric acid (H3PO4), usually just called phosphoric acid. All three protons can be successively lost to yield H2PO−
4, then HPO2−
4, and finally PO3−
4, the orthophosphate ion, usually just called phosphate. Even though the positions of the three protons on the original phosphoric acid molecule are equivalent, the successive Ka values differ since it is energetically less favorable to lose a proton if the conjugate base is more negatively charged. An organic example of a triprotic acid is citric acid, which can successively lose three protons to finally form the citrate ion.
Although the subsequent loss of each hydrogen ion is less favorable, all of the conjugate bases are present in solution. The fractional concentration, α (alpha), for each species can be calculated. For example, a generic diprotic acid will generate 3 species in solution: H2A, HA−, and A2−. The fractional concentrations can be calculated as below when given either the pH (which can be converted to the [H+]) or the concentrations of the acid with all its conjugate bases:
α H 2 A = [ H + ] 2 [ H + ] 2 + [ H + ] K 1 + K 1 K 2 = [ H 2 A ] [ H 2 A ] + [ HA − ] + [ A 2 − ] α HA − = [ H + ] K 1 [ H + ] 2 + [ H + ] K 1 + K 1 K 2 = [ HA − ] [ H 2 A ] + [ HA − ] + [ A 2 − ] α A 2 − = K 1 K 2 [ H + ] 2 + [ H + ] K 1 + K 1 K 2 = [ A 2 − ] [ H 2 A ] + [ HA − ] + [ A 2 − ] {\displaystyle {\begin{aligned}\alpha _{\ce {H2A}}&={\frac {\ce {[H+]^{2}}}{{\ce {[H+]^{2}}}+[{\ce {H+}}]K_{1}+K_{1}K_{2}}}={\frac {\ce {[H2A]}}{\ce {{[H2A]}+{[HA^{-}]}+{[A^{2-}]}}}}\\\alpha _{\ce {HA^{-}}}&={\frac {[{\ce {H+}}]K_{1}}{{\ce {[H+]^{2}}}+[{\ce {H+}}]K_{1}+K_{1}K_{2}}}={\frac {\ce {[HA^{-}]}}{\ce {{[H2A]}+{[HA^{-}]}+{[A^{2-}]}}}}\\\alpha _{\ce {A^{2-}}}&={\frac {K_{1}K_{2}}{{\ce {[H+]^{2}}}+[{\ce {H+}}]K_{1}+K_{1}K_{2}}}={\frac {\ce {[A^{2-}]}}{\ce {{[H2A]}+{[HA^{-}]}+{[A^{2-}]}}}}\end{aligned}}}
A plot of these fractional concentrations against pH, for given K1 and K2, is known as a Bjerrum plot. A pattern is observed in the above equations and can be expanded to the general n -protic acid that has been deprotonated i -times:
α H n − i A i − = [ H + ] n − i ∏ j = 0 i K j ∑ i = 0 n [ [ H + ] n − i ∏ j = 0 i K j ] {\displaystyle \alpha _{{\ce {H}}_{n-i}A^{i-}}={{[{\ce {H+}}]^{n-i}\displaystyle \prod _{j=0}^{i}K_{j}} \over {\displaystyle \sum _{i=0}^{n}{\Big [}[{\ce {H+}}]^{n-i}\displaystyle \prod _{j=0}^{i}K_{j}}{\Big ]}}}
where K0 = 1 and the other K-terms are the dissociation constants for the acid.
See also: Acid dissociation constant § Polyprotic acids
Neutralization
Hydrochloric acid (in beaker) reacting with ammonia fumes to produce ammonium chloride (white smoke).
Neutralization is the reaction between an acid and a base, producing a salt and neutralized base; for example, hydrochloric acid and sodium hydroxide form sodium chloride and water:
HCl(aq) + NaOH(aq) → H2O(l) + NaCl(aq)
Neutralization is the basis of titration, where a pH indicator shows equivalence point when the equivalent number of moles of a base have been added to an acid. It is often wrongly assumed that neutralization should result in a solution with pH 7.0, which is only the case with similar acid and base strengths during a reaction.
Neutralization with a base weaker than the acid results in a weakly acidic salt. An example is the weakly acidic ammonium chloride, which is produced from the strong acid hydrogen chloride and the weak base ammonia. Conversely, neutralizing a weak acid with a strong base gives a weakly basic salt, e.g. sodium fluoride from hydrogen fluoride and sodium hydroxide.
Weak acid–weak base equilibrium
Main article: Henderson–Hasselbalch equation
In order for a protonated acid to lose a proton, the pH of the system must rise above the pKa of the acid. The decreased concentration of H+ in that basic solution shifts the equilibrium towards the conjugate base form (the deprotonated form of the acid). In lower-pH (more acidic) solutions, there is a high enough H+ concentration in the solution to cause the acid to remain in its protonated form.
Solutions of weak acids and salts of their conjugate bases form buffer solutions.
Applications of acids
There are numerous uses for acids. Acids are often used to remove rust and other corrosion from metals in a process known as pickling. They may be used as an electrolyte in a wet cell battery, such as sulfuric acid in a car battery.
Strong acids, sulfuric acid in particular, are widely used in mineral processing. For example, phosphate minerals react with sulfuric acid to produce phosphoric acid for the production of phosphate fertilizers, and zinc is produced by dissolving zinc oxide into sulfuric acid, purifying the solution and electrowinning.
In the chemical industry, acids react in neutralization reactions to produce salts. For example, nitric acid reacts with ammonia to produce ammonium nitrate, a fertilizer. Additionally, carboxylic acids can be esterified with alcohols, to produce esters.
Acids are used as additives to drinks and foods, as they alter their taste and serve as preservatives. Phosphoric acid, for example, is a component of cola drinks. Acetic acid is used in day-to-day life as vinegar. Carbonic acid is an important part of some cola drinks and soda. Citric acid is used as a preservative in sauces and pickles.
Tartaric acid is an important component of some commonly used foods like unripened mangoes and tamarind. Natural fruits and vegetables also contain acids. Citric acid is present in oranges, lemon and other citrus fruits. Oxalic acid is present in tomatoes, spinach, and especially in carambola and rhubarb; rhubarb leaves and unripe carambolas are toxic because of high concentrations of oxalic acid.
Ascorbic acid (Vitamin C) is an essential vitamin for the human body and is present in such foods as amla (Indian gooseberry), lemon, citrus fruits, and guava.
Certain acids are used as drugs. Acetylsalicylic acid (Aspirin) is used as a pain killer and for bringing down fevers.
Acids play important roles in the human body. The hydrochloric acid present in the stomach aids in digestion by breaking down large and complex food molecules. Amino acids are required for synthesis of proteins required for growth and repair of body tissues. Fatty acids are also required for growth and repair of body tissues. Nucleic acids are important for the manufacturing of DNA and RNA and transmitting of traits to offspring through genes. Carbonic acid is important for maintenance of pH equilibrium in the body.
Acid catalysis
Main article: Acid catalysis
Acids are used as catalysts in industrial and organic chemistry; for example, sulfuric acid is used in very large quantities in the alkylation process to produce gasoline. Strong acids, such as sulfuric, phosphoric and hydrochloric acids also effect dehydration and condensation reactions. In biochemistry, many enzymes employ acid catalysis.[7]
Biological occurrence
Basic structure of an amino acid.
Many biologically important molecules are acids. Nucleic acids, which contain acidic phosphate groups, include DNA and RNA. Nucleic acids contain the genetic code that determines many of an organism's characteristics, and is passed from parents to offspring. DNA contains the chemical blueprint for the synthesis of proteins which are made up of amino acid subunits. Cell membranes contain fatty acid esters such as phospholipids.
An α-amino acid has a central carbon (the α or alpha carbon) which is covalently bonded to a carboxyl group (thus they are carboxylic acids), an amino group, a hydrogen atom and a variable group. The variable group, also called the R group or side chain, determines the identity and many of the properties of a specific amino acid. In glycine, the simplest amino acid, the R group is a hydrogen atom, but in all other amino acids it is contains one or more carbon atoms bonded to hydrogens, and may contain other elements such as sulfur, oxygen or nitrogen. With the exception of glycine, naturally occurring amino acids are chiral and almost invariably occur in the L-configuration. Peptidoglycan, found in some bacterial cell walls contains some D-amino acids. At physiological pH, typically around 7, free amino acids exist in a charged form, where the acidic carboxyl group (-COOH) loses a proton (-COO−) and the basic amine group (-NH2) gains a proton (-NH+
3). The entire molecule has a net neutral charge and is a zwitterion, with the exception of amino acids with basic or acidic side chains. Aspartic acid, for example, possesses one protonated amine and two deprotonated carboxyl groups, for a net charge of −1 at physiological pH.
Fatty acids and fatty acid derivatives are another group of carboxylic acids that play a significant role in biology. These contain long hydrocarbon chains and a carboxylic acid group on one end. The cell membrane of nearly all organisms is primarily made up of a phospholipid bilayer, a micelle of hydrophobic fatty acid esters with polar, hydrophilic phosphate "head" groups. Membranes contain additional components, some of which can participate in acid-base reactions.
In humans and many other animals, hydrochloric acid is a part of the gastric acid secreted within the stomach to help hydrolyze proteins and polysaccharides, as well as converting the inactive pro-enzyme, pepsinogen into the enzyme, pepsin. Some organisms produce acids for defense; for example, ants produce formic acid.
Acid-base equilibrium plays a critical role in regulating mammalian breathing. Oxygen gas (O2) drives cellular respiration, the process by which animals release the chemical potential energy stored in food, producing carbon dioxide (CO2) as a byproduct. Oxygen and carbon dioxide are exchanged in the lungs, and the body responds to changing energy demands by adjusting the rate of ventilation. For example, during periods of exertion the body rapidly breaks down stored carbohydrates and fat, releasing CO2 into the blood stream. In aqueous solutions such as blood CO2 exists in equilibrium with carbonic acid and bicarbonate ion.
CO2 + H2O ⇌ H2CO3 ⇌ H+ + HCO−
3
It is the decrease in pH that signals the brain to breathe faster and deeper, expelling the excess CO2 and resupplying the cells with O2.
Aspirin (acetylsalicylic acid) is a carboxylic acid.
Cell membranes are generally impermeable to charged or large, polar molecules because of the lipophilic fatty acyl chains comprising their interior. Many biologically important molecules, including a number of pharmaceutical agents, are organic weak acids which can cross the membrane in their protonated, uncharged form but not in their charged form (i.e. as the conjugate base). For this reason the activity of many drugs can be enhanced or inhibited by the use of antacids or acidic foods. The charged form, however, is often more soluble in blood and cytosol, both aqueous environments. When the extracellular environment is more acidic than the neutral pH within the cell, certain acids will exist in their neutral form and will be membrane soluble, allowing them to cross the phospholipid bilayer. Acids that lose a proton at the intracellular pH will exist in their soluble, charged form and are thus able to diffuse through the cytosol to their target. Ibuprofen, aspirin and penicillin are examples of drugs that are weak acids.
Common acids
Mineral acids (inorganic acids)
Hydrogen halides and their solutions: hydrofluoric acid (HF), hydrochloric acid (HCl), hydrobromic acid (HBr), hydroiodic acid (HI)
Halogen oxoacids: hypochlorous acid (HClO), chlorous acid (HClO2), chloric acid (HClO3), perchloric acid (HClO4), and corresponding analogs for bromine and iodine
Hypofluorous acid (HFO), the only known oxoacid for fluorine.
Sulfuric acid (H2SO4)
Fluorosulfuric acid (HSO3F)
Nitric acid (HNO3)
Phosphoric acid (H3PO4)
Fluoroantimonic acid (HSbF6)
Fluoroboric acid (HBF4)
Hexafluorophosphoric acid (HPF6)
Chromic acid (H2CrO4)
Boric acid (H3BO3)
Sulfonic acids
A sulfonic acid has the general formula RS(=O)2–OH, where R is an organic radical.
Methanesulfonic acid (or mesylic acid, CH3SO3H)
Ethanesulfonic acid (or esylic acid, CH3CH2SO3H)
Benzenesulfonic acid (or besylic acid, C6H5SO3H)
p-Toluenesulfonic acid (or tosylic acid, CH3C6H4SO3H)
Trifluoromethanesulfonic acid (or triflic acid, CF3SO3H)
Polystyrene sulfonic acid (sulfonated polystyrene, [CH2CH(C6H4)SO3H]n)
Carboxylic acids
A carboxylic acid has the general formula R-C(O)OH, where R is an organic radical. The carboxyl group -C(O)OH contains a carbonyl group, C=O, and a hydroxyl group, O-H.
Acetic acid (CH3COOH)
Citric acid (C6H8O7)
Formic acid (HCOOH)
Gluconic acid HOCH2-(CHOH)4-COOH
Lactic acid (CH3-CHOH-COOH)
Oxalic acid (HOOC-COOH)
Tartaric acid (HOOC-CHOH-CHOH-COOH)
Halogenated carboxylic acids
Halogenation at alpha position increases acid strength, so that the following acids are all stronger than acetic acid.
Fluoroacetic acid
Trifluoroacetic acid
Chloroacetic acid
Dichloroacetic acid
Trichloroacetic acid
Vinylogous carboxylic acids
Normal carboxylic acids are the direct union of a carbonyl group and a hydroxyl group. In vinylogous carboxylic acids, a carbon-carbon double bond separates the carbonyl and hydroxyl groups.
Ascorbic acid
Nucleic acids
Deoxyribonucleic acid (DNA)
Ribonucleic acid (RNA)
References
^ Jump up to: a b c IUPAC Gold Book - acid
Jump up ^ Petrucci R.H., Harwood, R.S. and Herring, F.G. General Chemistry (8th ed., Prentice-Hall 2002) p.146 ISBN 0-13-014329-4
Jump up ^ Merriam-Webster's Online Dictionary: acid
^ Jump up to: a b c d Oxtoby, D. W; Gillis, H.P., Butler, L. J. (2015).Principles of Modern Chemistry, Brooks Cole. p. 617. ISBN 978-1305079113
^ Jump up to: a b c Ebbing, D.D., & Gammon, S. D. (2005). General chemistry (8th ed.). Boston, MA: Houghton Mifflin. ISBN 0-618-51177-6
Jump up ^ Stahl PH, Nakamo M (2008). "Pharmaceutical Aspects of the Salt Form". In Stahl PH, Warmth CG. Handbook of Pharmaceutical Salts: Properties, Selection, and Use. Weinheim: Wiley-VCH. pp. 92–94. ISBN 978-3-906390-58-1.
Jump up ^ Voet, Judith G.; Voet, Donald (2004). Biochemistry. New York: J. Wiley & Sons. pp. 496–500. ISBN 978-0-471-19350-0.
Listing of strengths of common acids and bases
IUPAC Gold Book - acid
Zumdahl, Chemistry, 4th Edition.
Ebbing, D.D., & Gammon, S. D. (2005). General chemistry (8th ed.). Boston, MA: Houghton Mifflin. ISBN 0-618-51177-6
Pavia, D.L., Lampman, G.M., & Kriz, G.S. (2004). Organic chemistry volume 1: Organic chemistry 351. Mason, OH: Cenage Learning. ISBN 0-7593-4727-1
External links
Curtipot: Acid-Base equilibria diagrams, pH calculation and titration curves simulation and analysis – freeware
Authority control
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values: Acetic acid, CH3COOH, is composed of a methyl group, CH3, bound chemically to a carboxylate group, COOH. The carboxylate group can lose a proton and donate it to a water molecule, H20, leaving behind an acetate anion CH3COO- and creating a hydronium cation H3O. This is an equilibrium reaction, so the reverse process can also take place.

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text:
List of Academy Awards ceremonies
From Wikipedia, the free encyclopedia
Jump to: navigation, search
This is a list of Academy Awards ceremonies.[1][2][3]
This list is current as of the 90th Academy Awards ceremony held on March 4, 2018.
Contents
[hide]
1 Venues
2 Networks
3 Ceremonies
4 Multiple ceremonies hosted
5 Nominated hosts
6 See also
7 References
8 External links
Venues[edit]
1929: Hollywood Roosevelt Hotel
1930–1943: Alternated between the Ambassador Hotel and the Biltmore Hotel
1944–1946: Grauman's Chinese Theatre
1947–1948: Shrine Auditorium
1949: Academy Award Theater
1950–1960: Pantages Theatre
1961–1968: Santa Monica Civic Auditorium
1969–1987: Dorothy Chandler Pavilion
1988–2001: Alternated between the Dorothy Chandler Pavilion and the Shrine Auditorium
2002–present: Dolby Theatre (also known as Kodak Theatre, 2002-2011; Hollywood and Highland Centre, 2012)
Networks[edit]
U.S. network
Years
# of years
NBC 1953–1960 8
ABC 1961–1970 10
NBC 1971–1975 5
ABC 1976–2028 53 (43 years to date)
Ceremonies[edit]
Beginning with the 7th Academy Awards, held in February 1935, each year's awards are presented for films that were first shown during the full preceding calendar year from January 1 to December 31 in Los Angeles County, California. For the first five ceremonies, the eligibility period spanned twelve months from August 1 to July 31.[4] For the 6th ceremony, held in 1934, the eligibility period lasted from August 1, 1932 to December 31, 1933.[4]
When citing each ceremony, Academy conventions may either list the year(s) of its eligibility period,[5] or the year in which the ceremony was actually held.[6]
#
Date
Time
Local Time (PST/UTC-8)
Year(s)
Honored
Best Picture Winner
Length of Ceremony
Number of Viewers
Rating
Host(s)
Venue
Broadcast Partner(s)
1st May 16, 1929 8:00 p.m. 1927/28 Wings 015 !0 hours, 15 minutes 270 — Douglas Fairbanks, William C. deMille Hollywood Roosevelt Hotel None
2nd April 3, 1930 1928/29 broadway !The Broadway Melody 110 !1 hour, 50 minutes — — William C. deMille Ambassador Hotel KNX-AM.
One hour of the ceremony was broadcast live.[7]
3rd November 5, 1930 1929/30 All Quiet on the Western Front 133 !2 hours, 13 minutes — — Conrad Nagel KNX-AM.
One hour of the ceremony was broadcast live.
4th November 10, 1931 1930/31 Cimarron 123 !2 hours, 3 minutes — — Lawrence Grant Biltmore Hotel KHJ-AM.
45 minutes of the ceremony was broadcast live. Simulcast live on CBS network affiliates on the West Coast.
5th November 18, 1932 1931/32 Grand Hotel 112 !1 hour, 52 minutes — — Lionel Barrymore, Conrad Nagel Ambassador Hotel KECA-AM.
30 minutes of the ceremony was broadcast live. Simulcast live on NBC Blue Network affiliates on the West Coast.
6th March 16, 1934 1932/33 Cavalcade 110 !1 hour, 50 minutes — — Will Rogers None
7th February 27, 1935 1934 It Happened One Night 105 !1 hour, 45 minutes — — Irvin S. Cobb Biltmore Hotel None
8th March 5, 1936 1935 Mutiny on the Bounty 132 !2 hours, 12 minutes — — Frank Capra None
9th March 4, 1937 1936 The Great Ziegfeld 176 !2 hours, 56 minutes — — George Jessel None
10th March 10, 1938 8:15 p.m. 1937 The Life of Emile Zola 116 !1 hour, 56 minutes — — Bob Burns None
11th February 23, 1939 8:30 p.m. 1938 You Can't Take It With You 126 !2 hours, 6 minutes — — None KHJ-AM.
About 12 minutes of the ceremony broadcast live.
Partial broadcast of the 11th Academy Awards ceremony was shut down after about ten minutes because KHJ did not have permission to broadcast live. (The radio host was whispering the names of the winners as they were announced, out of sight in the balcony.) Later in the evening, at the conclusion of the ceremony, KHJ broadcast a full announcement of winners, live from the ceremony venue, as per its original agreement with the Academy.
12th February 29, 1940 8:30 p.m. 1939 Gone with the Wind 232 !3 hours, 52 minutes — — Bob Hope Ambassador Hotel
(Cocoanut Grove) KNX-AM.
Announcement of winners only at the conclusion of the ceremony, live from the ceremony venue.
13th February 27, 1941 8:45 p.m. 1940 Rebecca 130 !2 hours, 10 minutes — — Biltmore Hotel
(Biltmore Bowl) KECA-AM.
30 minutes of the ceremony was broadcast live.
Simulcast live on NBC Blue Network affiliates on the West Coast.
14th February 26, 1942 7:45 p.m. 1941 How Green Was My Valley 108 !1 hour, 48 minutes — — KNX-AM.
30 minutes of the ceremony was broadcast live.
Simulcast live on CBS network affiliates on the West Coast.
15th March 4, 1943 8:30 p.m. 1942 Mrs. Miniver 134 !2 hours, 14 minutes — — Ambassador Hotel
(Cocoanut Grove) KNX-AM.
Partial broadcast.
16th March 2, 1944 8:00 p.m. 1943 Casablanca 102 !1 hour, 42 minutes — — Jack Benny Grauman's Chinese Theater KNX-AM.
30 minutes of the ceremony was broadcast live.
Ceremony simulcast live on CBS network affiliates on the West Coast.
17th March 15, 1945 1944 Going My Way 130 !2 hours, 9 minutes — — Bob Hope, John Cromwell ABC Radio.
First coast-to-coast broadcast.
The 17th Academy Awards marked the first coast-to-coast broadcast of the ceremony, and first broadcast of the complete event. All subsequent ceremonies have been broadcast nationally in the USA. This was also the first ceremony in which film clips were used to introduce awards nominees.
18th March 7, 1946 8:00 p.m. 1945 The Lost Weekend 101 !1 hour, 41 minutes — — Bob Hope, James Stewart Grauman's Chinese Theater Radio: ABC Radio
Television: None
19th March 13, 1947 8:45 p.m. 1946 The Best Years of Our Lives 172 !2 hours, 52 minutes — — Jack Benny Shrine Auditorium
20th March 20, 1948 8:15 p.m. 1947 Gentleman's Agreement 118 !1 hour, 58 minutes — — Agnes Moorehead, Dick Powell
21st March 24, 1949 8:00 p.m. 1948 Hamlet 095 !1 hour, 35 minutes — — Robert Montgomery academy !The Academy Theater
22nd March 23, 1950 1949 All the King's Men 110 !1 hour, 50 minutes — — Paul Douglas Pantages Theatre
23rd March 29, 1951 1950 All About Eve 138 !2 hours, 18 minutes — — Fred Astaire
24th March 20, 1952 1951 An American in Paris 113 !1 hour, 53 minutes — — Danny Kaye
25th March 19, 1953 7:30 p.m. 1952 The Greatest Show on Earth 092 !1 hour, 32 minutes 40 million — Bob Hope, Conrad Nagel Pantages Theatre /
NBC International Theatre Radio: NBC Radio
Television: NBC-TV
26th March 25, 1954 8:00 p.m. 1953 From Here to Eternity 118 !1 hour, 58 minutes 43 million — Donald O'Connor, Fredric March Pantages Theatre /
NBC Century Theatre
27th March 30, 1955 7:30 p.m. 1954 On the Waterfront 108 !1 hour, 48 minutes — — Bob Hope, Thelma Ritter
28th March 21, 1956 1955 Marty 090 !1 hour, 30 minutes — — Jerry Lewis, Claudette Colbert, Joseph L. Mankiewicz
29th March 27, 1957 1956 Around the World in 80 Days 188 !3 hours, 8 minutes — — Jerry Lewis, Celeste Holm
30th March 26, 1958 1957 The Bridge on the River Kwai 161 !2 hours, 41 minutes — — Bob Hope, David Niven, James Stewart, Jack Lemmon, Rosalind Russell, Donald Duck[8] Pantages Theatre
31st April 6, 1959 1958 Gigi 115 !1 hour, 55 minutes — — Bob Hope, David Niven, Tony Randall, Mort Sahl, Laurence Olivier, Jerry Lewis
32nd April 4, 1960 1959 Ben-Hur 100 !1 hour, 40 minutes — — Bob Hope
33rd April 17, 1961 1960 The Apartment 125 !2 hours, 5 minutes — — Santa Monica Civic Auditorium Radio: ABC Radio
Television: ABC-TV
34th April 9, 1962 1961 West Side Story 130 !2 hours, 10 minutes — —
35th April 8, 1963 7:00 p.m. 1962 Lawrence of Arabia 150 !2 hours, 30 minutes — — Frank Sinatra
36th April 13, 1964 1963 Tom Jones 128 !2 hours, 8 minutes — — Jack Lemmon
37th April 5, 1965 1964 My Fair Lady 170 !2 hours, 50 minutes — — Bob Hope
38th April 18, 1966 1965 The Sound of Music 174 !2 hours, 54 minutes — —
39th April 10, 1967 1966 A Man for All Seasons 151 !2 hours, 31 minutes — —
40th April 10, 1968 1967 In the Heat of the Night 110 !1 hour, 50 minutes — —
The 40th Academy Awards ceremony marked the final year that the ceremony was simulcast live on the radio.
41st April 14, 1969 7:00 p.m. 1968 Oliver! 153 !2 hours, 33 minutes — — None Dorothy Chandler Pavilion ABC-TV
42nd April 7, 1970 1969 Midnight Cowboy 145 !2 hours, 25 minutes — 43.40
43rd April 15, 1971 1970 Patton 172 !2 hours, 52 minutes — — NBC-TV
44th April 10, 1972 1971 The French Connection 104 !1 hour, 44 minutes — — Helen Hayes, Alan King, Sammy Davis Jr., Jack Lemmon
45th March 27, 1973 1972 The Godfather 158 !2 hours, 38 minutes — — Carol Burnett, Michael Caine, Charlton Heston, Rock Hudson
46th April 2, 1974 1973 The Sting 203 !3 hours, 23 minutes — — John Huston, Burt Reynolds, David Niven, Diana Ross
47th April 8, 1975 1974 The Godfather Part II 200 !3 hours, 20 minutes — — Sammy Davis Jr., Bob Hope, Shirley MacLaine, Frank Sinatra
48th March 29, 1976 1975 One Flew Over the Cuckoo's Nest 192 !3 hours, 12 minutes — — Goldie Hawn, Gene Kelly, Walter Matthau, George Segal, Robert Shaw ABC-TV
49th March 28, 1977 1976 Rocky 218 !3 hours, 38 minutes — — Warren Beatty, Ellen Burstyn, Jane Fonda, Richard Pryor
50th April 3, 1978 1977 Annie Hall 210 !3 hours, 30 minutes 39.73 million 31.10 Bob Hope
51st April 9, 1979 1978 The Deer Hunter 205 !3 hours, 25 minutes — — Johnny Carson
52nd April 14, 1980 6:00 p.m. 1979 Kramer vs. Kramer 192 !3 hours, 12 minutes — —
53rd March 31, 1981 7:00 p.m. 1980 Ordinary People 193 !3 hours, 13 minutes — —
54th March 29, 1982 6:00 p.m. 1981 Chariots of Fire 204 !3 hours, 24 minutes — —
55th April 11, 1983 1982 Gandhi 195 !3 hours, 15 minutes — — Liza Minnelli, Dudley Moore, Richard Pryor, Walter Matthau
56th April 9, 1984 1983 Terms of Endearment 222 !3 hours, 42 minutes — 38.00 Johnny Carson
57th March 25, 1985 1984 Amadeus 190 !3 hours, 10 minutes — — Jack Lemmon
58th March 24, 1986 1985 Out of Africa 182 !3 hours, 2 minutes 38.65 million 25.71 Alan Alda, Jane Fonda, Robin Williams
59th March 30, 1987 1986 Platoon 199 !3 hours, 19 minutes 39.72 million 25.94 Chevy Chase, Goldie Hawn, Paul Hogan
60th April 11, 1988 1987 The Last Emperor 213 !3 hours, 33 minutes 42.04 million 27.80 Chevy Chase Shrine Auditorium
61st March 29, 1989 1988 Rain Man 199 !3 hours, 19 minutes 42.77 million 28.41 None
62nd March 26, 1990 1989 Driving Miss Daisy 217 !3 hours, 37 minutes 40.22 million 26.42 Billy Crystal Dorothy Chandler Pavilion
63rd March 25, 1991 1990 Dances with Wolves 215 !3 hours, 35 minutes 42.79 million 28.06 Shrine Auditorium
64th March 30, 1992 1991 The Silence of the Lambs 213 !3 hours, 33 minutes 44.44 million 29.84 Dorothy Chandler Pavilion
65th March 29, 1993 1992 Unforgiven 210 !3 hours, 30 minutes 45.84 million 32.85
66th March 21, 1994 1993 Schindler's List 198 !3 hours, 18 minutes 46.26 million 31.86 Whoopi Goldberg
67th March 27, 1995 1994 Forrest Gump 215 !3 hours, 35 minutes 48.87 million 33.47 David Letterman Shrine Auditorium
68th March 25, 1996 1995 Braveheart 218 !3 hours, 38 minutes 44.81 million 30.48 Whoopi Goldberg Dorothy Chandler Pavilion
69th March 24, 1997 1996 The English Patient 214 !3 hours, 34 minutes 40.83 million 25.83 Billy Crystal Shrine Auditorium
70th March 23, 1998 1997 Titanic 227 !3 hours, 47 minutes 57.25 million 35.32
71st March 21, 1999 5:30 p.m. 1998 Shakespeare in Love 242 !4 hours, 2 minutes 45.63 million 28.51 Whoopi Goldberg Dorothy Chandler Pavilion
72nd March 26, 2000 1999 American Beauty 244 !4 hours, 9 minutes 46.53 million 29.64 Billy Crystal Shrine Auditorium
73rd March 25, 2001 2000 Gladiator 203 !3 hours, 23 minutes 42.93 million 25.86 Steve Martin
74th March 24, 2002 2001 A Beautiful Mind 263 !4 hours, 23 minutes 40.54 million 25.13 Whoopi Goldberg Kodak Theatre
(then name of the Dolby Theatre)
75th March 23, 2003 2002 Chicago 210 !3 hours, 30 minutes 33.04 million 20.58 Steve Martin
76th February 29, 2004 2003 The Lord of the Rings:
The Return of the King 224 !3 hours, 44 minutes 43.56 million 26.68 Billy Crystal
77th February 27, 2005 2004 Million Dollar Baby 194 !3 hours, 14 minutes 42.16 million 25.29 Chris Rock
78th March 5, 2006 5:00 p.m. 2005 Crash 213 !3 hours, 33 minutes 38.64 million 22.91 Jon Stewart
79th February 25, 2007 2006 The Departed 231 !3 hours, 51 minutes 39.92 million 23.65 Ellen DeGeneres
80th February 24, 2008 2007 No Country for Old Men 201 !3 hours, 21 minutes 31.76 million 18.66 Jon Stewart
81st February 22, 2009 2008 Slumdog Millionaire 210 !3 hours, 30 minutes 36.94 million 20.88 Hugh Jackman
82nd March 7, 2010 2009 The Hurt Locker 217 !3 hours, 37 minutes 41.62 million 24.89 Steve Martin, Alec Baldwin
83rd February 27, 2011 2010 The King's Speech 195 !3 hours, 15 minutes 37.9 million 21.2 James Franco, Anne Hathaway
84th February 26, 2012 5:30 p.m. 2011 The Artist 194 !3 hours, 14 minutes 39.46 million 23.91 Billy Crystal Hollywood and Highland Center
(intermediate name of the Dolby Theatre)
85th February 24, 2013 2012 Argo 215 !3 hours, 35 minutes 40.38 million 24.47 Seth MacFarlane Dolby Theatre
86th March 2, 2014 2013 12 Years a Slave 215 !3 hours, 34 minutes 43.74 million 24.7 Ellen DeGeneres
87th February 22, 2015 2014 Birdman or (The Unexpected Virtue of Ignorance) 220 !3 hours, 43 minutes 37.26 million 20.6 Neil Patrick Harris
88th February 28, 2016 2015 Spotlight 217 !3 hours, 37 minutes 34.43 million 23.4 Chris Rock
89th February 26, 2017 2016 Moonlight 217 !3 hours, 49 minutes 33.0 million 22.4 Jimmy Kimmel
90th March 4, 2018 5:00 p.m. 2017 The Shape of Water 217 !3 hours, 53 minutes 26.5 million 18.9
Multiple ceremonies hosted[edit]
The following individuals have hosted (or co-hosted) the Academy Awards ceremony on two or more occasions.
Host
Number of Ceremonies
Bob Hope 19
Billy Crystal 9
Johnny Carson 5
Whoopi Goldberg 4
Jack Lemmon
Jerry Lewis 3
Steve Martin
Conrad Nagel
David Niven
Jack Benny 2
Chevy Chase
Sammy Davis Jr.
Ellen DeGeneres
Jane Fonda
Goldie Hawn
Jimmy Kimmel
Walter Matthau
Richard Pryor
Chris Rock
Frank Sinatra
James Stewart
Jon Stewart
Nominated hosts[edit]
The following individuals have hosted (or co-hosted) the Academy Awards ceremony on the same year in which the individual was also a nominee.
Host
Ceremony
Date
Category
Film
Result
David Niven 31st Academy Awards April 6, 1959 Academy Award for Best Actor Separate Tables Won
Michael Caine 45th Academy Awards March 27, 1973 Academy Award for Best Actor Sleuth Nominated
Walter Matthau 48th Academy Awards March 29, 1976 Academy Award for Best Actor The Sunshine Boys Nominated
Paul Hogan 59th Academy Awards March 30, 1987 Academy Award for Best Original Screenplay "Crocodile" Dundee Nominated
James Franco 83rd Academy Awards February 27, 2011 Academy Award for Best Actor 127 Hours Nominated
Seth MacFarlane 85th Academy Awards February 24, 2013 Academy Award for Best Original Song Ted Nominated
See also[edit]
Academy Award
List of presenters of Best Picture Academy Award
References[edit]
Jump up ^ Scott Bowles (26 February 2008). "Low Oscar Ratings Cue Soul-Searching". USA Today. Retrieved 19 March 2008.
Jump up ^ Nikki Finke (26 February 2007). "UPDATE: 39.9 Million Watch 79th Oscars". Nikki Finke's Deadline Hollywood Daily. LA Weekly. Retrieved 21 February 2011.
Jump up ^ Bill Gorman (8 March 2010). "Academy Awards Averages 41.3 Million Viewers; Most Since 2005". TVbytheNumbers. Archived from the original on 10 March 2010. Retrieved 12 March 2010.
^ Jump up to: a b Levy, Emanuel (2003). All About Oscar: The History and Politics of the Academy Awards. New York, United States: Continuum International Publishing Group. p. 52. ISBN 978-0-8264-1452-6.
Jump up ^ Crouse, Richard (2005). Reel Winners: Movie Award Trivia. Toronto, Ontario, Canada: University of Toronto Press. p. 257. ISBN 978-1-55002-574-3.
Jump up ^ "Oscars Ceremonies". oscars.org. Academy of Motion Picture Arts and Sciences. Retrieved March 4, 2017.
Jump up ^ "An Unofficial History of the Academy Awards on Radio". tripod.com.
Jump up ^ "Best, worst and weirdest Oscar hosts of all time". CNN. 22 February 2013.
External links[edit]
The Academy Awards, USA at the Internet Movie Database
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Footnote
‡ Dates and years listed for each ceremony were the eligibility period of film release in Los Angeles County. For the first five ceremonies, the eligibility period was done on a seasonal basis, from August to July. For the 6th ceremony, held in 1934, the eligibility period lasted from August 1, 1932 to December 31, 1933. Since the 7th ceremony held in 1935, the period of eligibility became the full previous calendar year from January 1 to December 31.
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text:
Orange Sky Laundry
From Wikipedia, the free encyclopedia
Jump to: navigation, search
‹ The template Infobox organization is being considered for merging. ›
Orange Sky Laundry
Established
4 September 2014 (2014-09-04)[1]
Operating since 10 October 2014; 2 years ago (2014-10-10)[2]
Founders
Nic Marchesi
Lucas Patchett
Founded at
Brisbane
Registration no.
85890622990
Services
Free laundry for homeless
Website
www.orangeskylaundry.com.au
Orange Sky Laundry is a charity based in Brisbane, Queensland, Australia that offers a free mobile laundry service for the homeless. It was established on 4 September 2014[1] and began operations on 10 October 2014.[2] In January 2016 its founders, Nic Marchesi and Lucas Patchett, were awarded joint Young Australians of the Year for their social entrepreneurship.[3]
Contents
[hide]
1 Background
2 Expansion
3 Awards
4 Orange Sky Showers
5 See also
6 References
7 External links
Background[edit]
Marchesi describes himself and Patchett as "two normal everyday blokes who had a crazy idea".[4] They had previously volunteered at food vans and other outreach programs while still at school, and had a passion to help the homeless. Their idea "started as a fun test project — to see if it would work. From there, it took a life of its own.”[5] They took the name for their service from the Alexi Murdoch song "Orange Sky", which is about lending a hand to those in need.[6]
Orange Sky Laundry is a government registered charity.[1] The service is believed to be a world first.[4]
In February 2015, five months after they started with the first van in Brisbane in October 2014,[7] and two weeks after their expansion into Cairns, Cyclone Marcia hit the central Queensland coast and the then 20-year-olds headed to the area to offer their free service to affected communities.[8] Similarly, in January 2016, they travelled to Victoria to provide laundry services to people affected by the Great Ocean Road bushfires.[9]
The laundry vans filled a service gap and not only offered clean clothes and blankets but also dignity. Marchesi says the human connections enabled to the isolated is the most important aspect of their initiative.[10] Each van also carries six orange chairs. During the time the laundry is being washed and dried in the vans, the volunteers sit and socialise with the visitors.[11]
Expansion[edit]
Orange Sky began operating its second van (in Cairns) by February 2015,[12] and its third in Melbourne in June.[13] Their first birthday, and World Homeless Day 2015,[2] were celebrated with a new service in south east Victoria, funded by partners The Good Guys[14] (who provided half of the funding for the van[15]), the Jelley Family Foundation, and the Bennelong Foundation.[2] Other vans began operating in Sydney in November 2015,[6][16] Gold Coast in January 2016,[17] Perth in February 2016,[18][19] Adelaide in March 2016,[20][21] Sunshine Coast in April 2016,[10] Canberra in April 2016,[20][22][23] and Hobart in July 2016.[24]
By July 2016, Orange Sky had 10 vans and 600 volunteers, and were estimated to be washing nearly six tonnes of laundry each week.[25] As of September 2016[update] there are services in all Australian states plus the Australian Capital Territory.[1] They have plans to expand to the US.[26]
Awards[edit]
On Australia Day 2016, the two co-founders were jointly named Young Australians of the Year.[27] In their acceptance speeches after being announced as winners by the Australian prime minister, Malcolm Turnbull, Patchett said "we can restore respect, raise health standards and be a catalyst for conversation". Marchesi continued "It's so crazy and humbling to think such a simple idea has had such a significant impact".[28]
In June 2016 they were invited to Frankfurt, Germany to receive a Global Best Practices Award: Special Award for Corporate Social Responsibility.[29]
Orange Sky Showers[edit]
On 23 August 2016, Orange Sky launched a new mobile service: free hot showers for the homeless. One of the homeless to first try the shower van described it as "bloody awesome".[30] The first van is being trialled in Brisbane, but will then be permanently moved to Melbourne as it was funded by the Shine On Foundation which is based in Melbourne.[31]
See also[edit]
Australia portal
Homelessness in Australia
References[edit]
^ Jump up to: a b c d "Orange Sky Laundry INC". Melbourne: Australian Charities and Not-for-profits Commission. 4 September 2014. Retrieved 17 September 2016.
^ Jump up to: a b c d "SE Melbourne – Orange Sky Laundry". Orange Sky Laundry. 10 October 2015. Retrieved 16 September 2016. On Orange Sky Laundry's 1st Birthday, and World Homeless Day (10 October 2015), we launched our 4th service into the community of South East Victoria.
Jump up ^ "Nic Marchesi and Lucas Patchett". Canberra: National Australia Day Council. 26 January 2016. Retrieved 24 August 2016.
^ Jump up to: a b Huntsdale, Justin (7 July 2016). "Homeless washing van planned for Wollongong as Orange Sky Laundry team visits city". ABC News. Illawarra. Retrieved 24 August 2016.
Jump up ^ Chan, Allison (23 June 2016). "Orange Sky Laundry: Young Australians of the Year". Australia Plus. Australia. Retrieved 24 August 2016.
^ Jump up to: a b Browne, Rachel (6 November 2015). "Orange Sky Laundry offers free washing service for Sydney's homeless". The Sydney Morning Herald. Sydney. Retrieved 24 August 2016.
Jump up ^ Leonov, Tatyana (9 April 2015). "Australian small firms take to four wheels". BBC News. Retrieved 16 September 2016.
Jump up ^ Atfield, Cameron (22 February 2015). "Cyclone Marcia: Orange Sky cleans up after the storm". Brisbane Times. Brisbane. Retrieved 24 August 2016.
Jump up ^ Chalkley-Rhoden, Stephanie (30 December 2015). "Great Ocean Road fires: Devastation leads to outpouring of community spirit". ABC News. Melbourne. Retrieved 24 August 2016.
^ Jump up to: a b Tatham, Harriet (13 April 2016). "Orange Sky Laundry launches on Sunshine Coast, tackling housing, employment with clean clothes". ABC News. Sunshine Coast. Retrieved 24 August 2016.
Jump up ^ "Orange Sky Laundry – What We Do". Orange Sky Laundry. Retrieved 17 September 2016. Orange Sky Laundry is a catalyst for conversation. In the one hour time it takes to wash and dry someone's clothes there is absolutely nothing to do but sit down on one of our 6 orange chairs and have a positive and genuine conversation between our everyday volunteers and everyday friends on the street.
Jump up ^ Clarke, Harry (13 February 2015). "Unique Brisbane charity Orange Sky Laundry launches second mobile laundry van for Cairns’ homeless". Cairns Post. Cairns. Retrieved 24 August 2016.
Jump up ^ Webb, Carolyn (1 July 2016). "Orange Sky Laundry van provides a boost for Melbourne's homeless". The Age. Melbourne. Retrieved 24 August 2016.
Jump up ^ "Orange Sky Laundry Co-Founders Are Truly Good Guys". The Good Guys. Retrieved 17 September 2016.
Jump up ^ Ly, Sophie (10 October 2015). "Orange Sky Laundry". 2SER Radio - Saturday Breakfast. Event occurs at 02:47. Retrieved 17 September 2016.
Jump up ^ "Orange Sky Laundry Services – now operating in Sydney". Sydney: NSW Govt Family & Community Services. 26 November 2015. Retrieved 24 August 2016.
Jump up ^ Bedo, Stephanie (14 January 2016). "Orange Sky Laundry launches on the Gold Coast washing clothes for homeless". Gold Coast Bulletin. Gold Coast. Retrieved 24 August 2016.
Jump up ^ Tyrrell, Claire (19 February 2016). "Orange Sky homeless laundry service comes to Perth". The West Australian. Perth. Retrieved 24 August 2016.
Jump up ^ Young, Emma (28 March 2016). "Orange Sky mobile laundry service for the homeless celebrates Perth launch". WAtoday. Perth. Retrieved 24 August 2016.
^ Jump up to: a b Harrison Plesse, Richelle (30 March 2016). "Clean streets: the mobile laundry service helping Australia's homeless". The Guardian. London. Retrieved 24 August 2016.
Jump up ^ Campbell, Claire (30 March 2016). "Orange Sky Laundry service for the homeless extended to Adelaide". ABC News. Adelaide. Retrieved 24 August 2016.
Jump up ^ Doherty, Megan (28 April 2016). "Young Australians of the Year wash the clothes of the homeless as Orange Sky Laundry launches in Canberra". The Canberra Times. Canberra. Retrieved 24 August 2016.
Jump up ^ Maher, Louise (28 April 2016). "Orange Sky Laundry offers clean clothes and conversation for homeless in Canberra". ABC News. Canberra. Retrieved 24 August 2016.
Jump up ^ Smiley, Stephen (27 July 2016). "Orange Sky homeless laundry service kicks off in Hobart". ABC News. Hobart. Retrieved 24 August 2016.
Jump up ^ Hinchliffe, Jessica (1 July 2016). "Orange Sky Laundry road trip: Young Australians of the Year search for people making a difference". ABC News. Brisbane. Retrieved 24 August 2016.
Jump up ^ Calhoun, Marissa (14 July 2016). "Aussie's 'fun idea' inspires a movement". CNN. USA. Retrieved 24 August 2016.
Jump up ^ "Honour roll Young Australian of the Year National Recipient". Canberra: National Australia Day Council. 26 January 2016. Retrieved 24 August 2016.
Jump up ^ Allyson Horn (17 August 2016). "Australia Wide August 20". ABC News. Australian Broadcasting Corporation. Event occurs at 05:24. Retrieved 3 September 2016.
Jump up ^ "Global Best Practices Awards 2016". Ophemert Netherlands: CINET. 12 June 2016. Retrieved 24 August 2016.
Jump up ^ Hamilton-Smith, Lexy (23 August 2016). "Mobile shower van for homeless hits Brisbane streets thanks to Orange Sky pair". ABC News. Brisbane. Retrieved 24 August 2016.
Jump up ^ "Orange Sky have just launched their first portable shower for the homeless in Brisbane". The Catholic Leader. 23 August 2016. Retrieved 3 September 2016.
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