अम्ल

**अम्ल** (मराठी: ऍसिड) (यक्व थासय् जेनेरिक सूत्र कथं **HA** [H+A−]) सांस्कृतिक कथं रसायनिक कम्पाउण्ड ख। थ्व कम्पाउण्डयात लःया सम्पर्कय् तयेबिले छगू सोलुसन पिकई गुकिया हायड्रोजन आयन ऍक्टिव्हिटी शुद्ध लया स्वया अप्व जुइ, वा pH ७.० स्वया म्हो जुइ। थ्व परिभाषा अम्लया आधुनिक परिभाषाया नापं ला। आधुनिक परिभाषाय् जोहानेस निकोलस ब्रोन्स्टेड व मार्टिन लौरीया परिभाषा दु, इमिसं स्वतन्त्र कथं अम्लयात क्षारयात हायड्रोजन आयन (H+) बीइगु कम्पाउन्ड धका परिभाषित याना तःगु दु । साधारण दसुलि ऍसेटिक ऍसिड (व्हिनेगरय्) व सल्फ्युरिक अम्ल (कार बॅटरीइ छ्य्‌लिगु) आदि ला। अम्ल/क्षार व्यवस्था रिडक्स रिऍक्शन स्वया पा। अम्ल/क्षार व्यवस्थाय् रिडक्सय् थें ऑक्सिडेशन स्टेट पाइमखु।

## परिभाषा

"अम्ल" धाःगु खँग्वः संस्कृत शब्दं वःगु ख। रसायन शास्त्रय् दुथने धुंका थ्व खँग्वःयात निश्चित रसायनिक अर्थय् छ्येलिगु या। अम्लयात परिभाषित यायेगु प्यंगु साधारण प्रकृया दु:
* **आर्हेनियस**: According to this definition developed by the Swedish chemist Svante Arrhenius, an acid is a substance that increases the concentration of hydrogen ions (H+), which are carried as hydronium ions (H3O+) when dissolved in water, while bases are substances that increase the concentration of hydroxide ions (OH-). This definition limits acids and bases to substances that can dissolve in water. Around 1800, many French chemists, including Antoine Lavoisier, incorrectly believed that all acids contained oxygen. Indeed the modern German word for oxygen is *Sauerstoff* (lit. sour substance), as is the Afrikaans word for oxygen *suurstof*, with the same meaning. English chemists, including Sir Humphry Davy, at the same time believed all acids contained hydrogen.  Arrhenius used this belief to develop this definition of acid.
* **[[ब्रोन्स्टेड-लौरी]]**: According to this definition, an acid is a proton (hydrogen nucleus) donor and a base is a proton acceptor. The acid is said to be dissociated after the proton is donated. An acid and the corresponding base are referred to as conjugate acid-base pairs. Brønsted and Lowry independently formulated this definition, which includes water-insoluble substances not in the Arrhenius definition. Acids according to this definition are variously referred to as Brønsted acids, Brønsted-Lowry acids, proton acids, protic acids, or protonic acids. 
* **सल्भेण्ट-सिस्टम परिभाषा**: According to this definition, an acid is a substance that, when dissolved in an autodissociating solvent, increases the concentration of the solvonium cations, such as H3O+ in water, NH4+ in liquid ammonia, NO+ in liquid N2O4, SbCl2+ in SbCl3, etc. Base is defined as the substance that increases the concentration of the solvate anions, respectively OH-, NH2-, NO3-, or SbCl4-. This definition extends acid-base reactions to non-aqueous systems and even some aprotic systems, where no hydrogen nuclei are involved in the reactions. This definition is not absolute, a compound acting as acid in one solvent may act as a base in another.
* **लिवाइस**: According to this definition developed by Gilbert N. Lewis, an acid is an electron-pair acceptor and a base is an electron-pair donor. (These are frequently referred to as "Lewis acids" and "Lewis bases," and are electrophiles and nucleophiles, respectively, in organic chemistry; Lewis bases are also ligands in coordination chemistry.)  Lewis acids include substances with no transferable protons (ie H+ hydrogen ions), such as iron(III) chloride, and hence the Lewis definition of an acid has wider application than the Brønsted-Lowry definition. In fact, the term **Lewis acid** is often used to exclude protic (Brønsted-Lowry) acids. The Lewis definition can also be explained with molecular orbital theory. In general, an acid can receive an electron pair in its lowest unoccupied orbital (LUMO) from the highest occupied orbital (HOMO) of a base. That is, the HOMO from the base and the LUMO from the acid combine to a bonding molecular orbital.

दक्ले साधारण सिद्धान्त मजुसां ब्रोन्स्टेड-लौरी सिद्धान्त व परिभाषा दक्ले आपालं छ्य्‌लातःगु खने दु। अम्लया क्षमता, थ्व परिभाषा कथं, हाइड्रोनियमया स्टेबिलिटी व डिसोसियसनय् सोल्भेन्ट कञ्जुगेट बेसय् आधारित दु। कञ्जुगेट क्षारया अप्वइगु वा म्हो स्टेबिलिटीं कम्पाउण्डय् दैगु अप्व या म्हो अम्लीयतायात असर याइ। अम्लीयताया विचाः आपालं अर्‍ग्यानिक अम्ल दसु कार्बोक्जिलिक अम्लय् छ्येलिगु या। मोलेकुलर अर्बिटल परिभाषां (अन्-फिल्ड प्रोटोन अर्बाइटलं लोन पेयरयात ओभरल्याप याइगु विचा) लिवाइस परिभाषानाप स्वापू तः।

## गुण

ब्रोन्स्टेड-लौरी अम्ल:

* आपालं पाउंसे च्वंगु स्वाद दै
* Strong or concentrated acids often produce a stinging feeling on mucous membranes
* Change the color of pH indicators as follows: turn blue litmus and methyl orange red, turn phenolphthalein colorless
* React with metals to produce a metal salt and hydrogen
* React with metal carbonates to produce water, CO2 and a salt
* React with a base to produce a salt and water
* React with a metal oxide to produce water and a salt
* Conduct electricity, depending on the degree of dissociation
* Produce solvonium ions, such as oxonium (H3O+) ions in water

Acids are/can be gases, liquids, or solids. Respective examples (at 20&nbsp;°C and 1 atm) are hydrogen chloride, sulfuric acid and citric acid. Solutions of acids in water are liquids, such as hydrochloric acid - an aqueous solution of hydrogen chloride. At 20&nbsp;°C and 1 atm, linear carboxylic acids are liquids up to nonanoic acid (nine carbon atoms) and solids beginning from decanoic acid (ten carbon atoms). Aromatic carboxylic acids, the simplest being benzoic acid, are solids.

Strong acids and many concentrated acids, being corrosive, can be dangerous; causing severe burns for even minor contact. Generally, acid burns on the skin are treated by rinsing the affected area abundantly with running water, followed up with immediate medical attention. In the case of highly concentrated mineral acids such as sulfuric acid or nitric acid, the acid should first be wiped off, otherwise the exothermic mixing of the acid and the water could cause thermal burns. Particular acids may also be dangerous for reasons not related to their acidity. Material Safety Data Sheets (MSDS) can be consulted for detailed information on dangers and handling instructions.

## नामाकरण
क्लासिकल नामाकरणय् अम्लतेत इमिगु एनायन कथं नां बियातै। 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.

क्लासिकल नामाकरण:

## रसायनिक गुण
In water the following equilibrium occurs between a weak acid (HA) and water, which acts as a base:

HA(aq) + H2O  H3O+(aq) + A-(aq)

The acidity constant (or acid dissociation constant) is the equilibrium constant for the reaction of HA with water:

:K_a = \frac{[\mbox{H}_3\mbox{O}^+][\mbox{A}^-]}{[\mbox{HA}]}

Strong acids have large *K*a values (i.e. the reaction equilibrium lies far to the right; the acid is almost completely dissociated to H3O+ and A-). Strong acids include the heavier hydrohalic acids: hydrochloric acid (HCl), hydrobromic acid (HBr), and hydroiodic acid (HI). (However, hydrofluoric acid, HF, is relatively weak.) For example, the *K*a value for hydrochloric acid (HCl) is 107.

Weak acids have small *K*a values (i.e. at equilibrium significant amounts of HA and A− exist together in solution; modest levels of H3O+ are present; the acid is only partially dissociated). For example, the Ka value for acetic acid is 1.8 x 10-5. Most organic acids are weak acids. Oxoacids, which tend to contain central atoms in high oxidation states surrounded by oxygen may be quite strong or weak. Nitric acid, sulfuric acid, and perchloric acid are all strong acids, whereas nitrous acid, sulfurous acid and hypochlorous acid are all weak. 

Note on terms used:
* The terms "hydrogen ion" and "proton" are used interchangeably; both refer to H+.
* In aqueous solution, the water is protonated to form hydronium ion, H3O+(aq). This is often abbreviated as H+(aq) even though the symbol is not chemically correct.
* The strength of an acid is measured by its acid dissociation constant (*K*a) or equivalently its p*K*a (p*K*a= - log(*K*a)). 
* The pH of a solution is a measurement of the concentration of hydronium. This will depend on the concentration and nature of acids and bases in solution.

### मोनोप्रोटिक अम्ल
**मोनोप्रोटिक अम्ल** थन्यागु अम्ल ख गुकिलिं केमिकल डिसोसियसन (वा आयोनाइजेसन)य् छगू अम्ल प्रति मोलेक्युल दान यायेफु। दसु (HAया चिं दुगु अम्ल स्वयादिसँ):

:::::HA(aq) + H2O(l)  H3O+(aq) + A−(aq) &nbsp; &nbsp; &nbsp; &nbsp; *K*a

थ्व कथंया अम्लया साधारण दसुलि खनिज अम्ल (गुकिलि हाइड्रोक्लोरिक अम्ल (HCl) व नाइट्रिक अम्ल (HNO३) ला) ख। मेगु थासय् अर्‍ग्यानिक अम्लय् थ्व खँग्वः छगू कार्बोक्सिल पुचः दूगु अम्लया निंतिं छ्येलि गुकियात गबिलें-गबिलें **मोनोकार्बोक्सिलिक अम्ल**या नां नं बिइगु या। दसुया अर्‍ग्यानिक अम्लय् फर्मिक अम्ल (HCOOH), एसेटिक अम्ल (CH३COOH) व बेञ्जोइक अम्ल (C६H५COOH) ला।

### पोलिप्रोटिक अम्ल
Polyprotic 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) &nbsp; &nbsp; &nbsp; *K*a1

:::::HA−(aq) + H2O(l)  H3O+(aq) + A2−(aq)&nbsp; &nbsp; &nbsp;&nbsp; *K*a2

The first dissociation constant is typically greater than the second; i.e., *K*a1 > *K*a2 . For example, sulfuric acid (H2SO4) can donate one proton to form the bisulfate anion (HSO4−), for which *K*a1 is very large; then it can donate a second proton to form the sulfate anion (SO42−), wherein the *K*a2 is intermediate strength. The large *K*a1 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 (HCO3−) and lose a second to form carbonate anion (CO32−). Both *K*a values are small, but *K*a1 > *K*a2 .

A triprotic acid (H3A) can undergo one, two, or three dissociations and has three dissociation constants, where *K*a1 > *K*a2 > *K*a3 .

:::::H3A(aq) + H2O(l)  H3O+(aq) + H2A−(aq) &nbsp; &nbsp; &nbsp;&nbsp; *K*a1

:::::H2A−(aq) + H2O(l)  H3O+(aq) + HA2−(aq) &nbsp; &nbsp; &nbsp; *K*a2

:::::HA2−(aq) + H2O(l)  H3O+(aq) + A3−(aq) &nbsp; &nbsp;&nbsp;&nbsp;&nbsp;&nbsp; *K*a3

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 H2PO4−, then HPO42−, and finally PO43− , the orthophosphate ion, usually just called phosphate. An organic example of a triprotic acid is citric acid, which can successively lose three protons to finally form the citrate ion. Even though the positions of the protons on the original molecule may be equivalent, the successive *K*a values will differ since it is energetically less favorable to lose a proton if the conjugate base is more negatively charged.

### न्युट्रलाइजेसन
[thumb|[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.

### कमजोर अम्ल/कमजोर क्षार समीकरण

In order to lose a proton, it is necessary that the pH of the system rise above the p*K*a of the protonated 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, or to protonate its conjugate base (the deprotonated form).

Solutions of weak acids and salts of their conjugate bases form buffer solutions.

## अम्लया छ्य्‌ला

अम्ल यक्व थासय् छ्य्‌लेछिं। अम्लयात आपालं खतं व मेमेगु धातुया करोजन (corrosion) लिकायेत पिक्लिङ प्रकृयाय् छ्येलि। अम्लयात वेट सेल ब्याट्रीइ इलेक्ट्रोलाइटया कथं नं छ्येलिगु या, दसु स्ल्फ्युरिक अम्लयात कार ब्याट्रीइ छ्यलि।

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 catalysts; 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.

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.

## जैविक स्थिति
मनु व यक्व मेमेगु प्राणीइ हाइड्रोक्लोरिक अम्ल ग्यास्ट्रिक अम्लया छगू भागया रुपं प्वाथं प्रोटिन व पोलिस्याकेराइड पाचनया निंतिं पिकाइ। थुकिलिं इन्-एक्टिभ प्रो-इञ्जाइम पेप्सिनोजेनयात इञ्जाइम पेप्सिनय् हिलाछ्वइ। छुं प्राणीतेसं अम्लयात प्रतिकारया निंतिं पिकाइ, दसु इमुं फर्मिक अम्ल पिकाइ।

## साधारण अम्ल
### [[खनिज अम्ल]]
* हाइड्रोजन हेलाइडया सोलुसन, दसु हाइड्रोक्लोरिक अम्ल (HCl) व हाइड्रोब्रोमिक अम्ल (HBr)
* सल्फ्युरिक अम्ल (H2SO4)
* नाइट्रिक अम्ल (HNO3)
* फोस्फोरिक अम्ल (H3PO4)
* क्रोमिक अम्ल (H2CrO4)

### [[सल्फोनिक अम्ल]]
* मिथेनसल्फोनिक अम्ल (aka mesylic acid) (MeSO3H)
* इथेनसल्फोनिक अम्ल (aka esylic acid) (EtSO3H)
* बेञ्जिनसल्फोनिक अम्ल (aka besylic acid) (PhSO3H)
* टोलुइनसल्फोनिक अम्ल (aka tosylic acid, or (C6H4(CH3) (SO3H))

### [[कार्बोक्जिलिक अम्ल]]
* फर्मिक अम्ल
* एसेटिक अम्ल
* साइट्रिक अम्ल

### [[भिनिलोगस]] कार्बोक्सिलिक अम्ल
* एस्कर्बिक अम्ल
* मेल्ड्रमया अम्ल

## लिधंसा

* साधारण अम्ल व क्षारया धलः
* Zumdahl, Chemistry, 4th Edition.

## स्वयादिसँ

; रसायनशास्त्र
* अम्ल भ्यालु
* अम्ल लवण
* क्षार
* आधारभूत क्षार
* बाइनरी अम्ल
* भिट्रियोल
* अम्ल-क्षार एक्स्ट्र्याक्सन
; वातावरण

* अम्ल वा
* महासागर अम्लीकरण

## पिनेया स्वापू
* Science Aid: अम्ल व क्षार हाइस्कुलया विद्यार्थीतेगु निंतिं जानकारी
* कर्टिपोट: अम्ल-क्षार इक्विलिब्रिया किपा, pH ल्याखायेगु व टाइट्रेसन कर्भ स्टिमुलेसन व एनालाइसिस - फ्रिवेय्‌र
* अम्लया गुणया बारेय् प्राथमिक रसायनिक विद्यार्थीया निंतिं सार
* लङ्ग रेञ्ज ट्रान्सबाउण्डरी प्रदुषणया बारेय् UN ECE कन्भेन्सन


पुचः:अम्ल-क्षार रसायनशास्त्र
पुचः:विज्ञान