Name: water as an amphiprotic substance
Uploaded: 2020-09-24T15:06:51.000Z
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Water: A Bronsted-Lowry Acid and Base

Une molécule amphotère est capable de réagir à la fois comme un acide et comme une base. L'eau est un exemple de molécule amphotère. Dans une solution aqueuse d'ammoniac, l'eau peut agir comme un acide en donnant un proton à l'ammoniac, une base.En revanche, l'eau agit comme une base dans une solution aqueuse d'acide chlorhydrique en acceptant un proton de l'acide. Parce qu'elle est amphotère, l'eau peut subir une auto-ionisation. Dans ce processus, une molécule d'eau agit comme l'acide en donnant un proton à une autre molécule d'eau qui agit comme une base en acceptant ce proton.Cela se traduit par la production d'un ion hydronium et un ion hydroxyde. La constante d'équilibre pour l'auto-ionisation de l'eau, Kᴡ, également connue sous le nom de constante ion-produit pour l'eau, peut être exprimée en Kᴡ et a une valeur de 1 10⁻¹⁴. Son expression à l'équilibre est écrite comme la concentration des ions hydronium multipliés par la concentration des ions hydroxyde, sans dénominateur car les deux réactifs sont des liquides.Dans de l'eau pure à 25 degrés Celsius, les concentrations des ions hydronium et hydroxyde sont égales soit 1 10⁻⁷ M.Le Kᴡ peut être utilisé pour calculer la concentration des ions hydronium et hydroxyde dans une solution et pour déterminer si une solution est acide ou basique. Si une solution est acide, la concentration des ions hydronium sera plus élevée que les ions hydroxyde. En revanche, si une solution est basique, la concentration des ions hydroxyde sera plus élevé que les ions hydronium.Si la concentration d'ions hydronium en solution est 5 10⁻⁷ M, la concentration en ions hydroxyde peut être déterminée en utilisant Kᴡ.Comme les valeurs de Kᴡ et des ions hydronium sont connues, la concentration d'ions hydroxyde peut être calculée comme étant 2 10⁻⁸ molaire. En tant que concentration en ions hydronium, 5 10⁻⁷ molaire, est supérieure à la concentration en ions hydroxyde, 2 10⁻⁸ molaire, la solution est acide.

l'eau : un acide et une base selon bronsted-lowry

La réaction entre un acide de Brønsted-Lowry et l'eau est appelée une ionisation de l'acide. Par exemple, lorsque le fluorure d'hydrogène se dissout dans l'eau et s'ionise, les protons sont transférés des molécules de fluorure d'hydrogène aux molécules d'eau, ce qui donne des ions hydronium et des ions fluorure : 
  <img alt="Image1" src="/files/ftp_upload/11396/11396_Image_1.svg" style="height: 125px;" />
 L'ionisation de la base d'une espèce se produit lorsqu'elle accepte des protons provenant de molécules d'eau. Dans l'exemple ci-dessous, les molécules de pyridine, C5NH5, subissent l'ionisation de la base lorsqu'elles sont dissoutes dans l'eau, produisant des ions d'hydroxyde et pyridinium : 
  <img alt="Image2" src="/files/ftp_upload/11396/11396_image 2v2.svg" style="height: 190px;" />
 Les réactions d'ionisation précédentes suggèrent que l'eau peut fonctionner à la fois comme une base (comme dans sa réaction avec le fluorure d'hydrogène) et comme un acide (comme dans sa réaction avec l'ammoniac). On dit que les espèces capables de donner ou d'accepter des protons sont amphiprotiques, ou plus généralement, amphotères, un terme qui peut être utilisé pour les acides et les bases selon des définitions autres que celle de Brønsted-Lowry. Les équations ci-dessous montrent les deux réactions acido-basiques possibles pour deux espèces amphiprotiques, l'ion bicarbonate et l'eau : 
  <img alt="Equation1" src="/files/ftp_upload/11396/11396_Equation_1.png" style="height: 95px;" />
 La première équation représente la réaction du bicarbonate en tant qu'acide avec de l'eau comme base, tandis que la seconde représente la réaction du bicarbonate en tant que base avec de l'eau comme acide. Lorsque du bicarbonate est ajouté à l'eau, ces équilibres sont établis simultanément et la composition de la solution obtenue peut être déterminée par des calculs d'équilibre appropriés. À l'état liquide, les molécules d'une substance amphiprotique peuvent réagir les unes avec les autres, comme illustré pour l'eau dans les équations ci-dessous : 
  <img alt="Image3" src="/files/ftp_upload/11396/11396_image_3.svg" style="height: 125px;" />
 Le processus dans lequel des molécules semblables réagissent pour donner des ions est appelé auto-ionisation. L'eau liquide subit une auto-ionisation de façon très légère ; à 25 °C, environ deux molécules d'eau sur un milliard sont ionisées. L'ampleur du processus d'auto-ionisation de l'eau se reflète dans la valeur de sa constante d'équilibre, la constante du produit ionique pour l'eau, KE : 
  <img alt="Equation2" src="/files/ftp_upload/11396/11396_Equation_2.png" style="height: 50px;" />
 La légère ionisation de l'eau pure se reflète dans la faible valeur de la constante d'équilibre ; à 25 °C, KE a une valeur de 1,0 × 10−14. 
  <img alt="Equation3" src="/files/ftp_upload/11396/11396_Equation_3.png" style="height: 50px;" />
 Le processus est endothermique, et donc l'importance de l'ionisation et les concentrations résultantes d'ion hydronium et d'ion hydroxyde augmentent avec la température. Par exemple, à 100 °C, la valeur de KE est d'environ 5,6 × 10−13, soit environ 50 fois plus que la valeur de 25 °C. 
 L'auto-ionisation de l'eau donne le même nombre d'ions hydronium et hydroxyde. Par conséquent, dans l'eau pure à 25 °C : 
  <img alt="Equation4" src="/files/ftp_upload/11396/11396_Equation_4.png" style="height: 50px;" />
 Les concentrations de ces ions dans une solution sont souvent des déterminants critiques des propriétés de la solution et des comportements chimiques de ses autres solutés, et un vocabulaire spécifique a été développé pour décrire ces concentrations en termes relatifs. Une solution est neutre si elle contient des concentrations égales d'ions hydronium et hydroxyde ; acide si elle contient une plus grande concentration d'ions hydronium que d'ions hydroxyde ; et basique si elle contient une concentration moindre d'ions hydronium que d'ions hydroxyde. 
 Résumé des relations pour les solutions acides, basiques et neutres 
 <table style="margin-left: auto; margin-right: auto;">
 <tbody>
 <tr>
 <td style="color: black; border: 1px solid black; text-align: center;">Classification </td>
 <td style="color: black; border: 1px solid black; text-align: center;">Concentrations ioniques relatives </td>
 <td style="color: black; border: 1px solid black; text-align: center;">pH à 25 °C </td>
 </tr>
 <tr>
 <td style="color: black; border: 1px solid black; text-align: center;">acide </td>
 <td style="color: black; border: 1px solid black; text-align: center;">[H3O+] > [OH−] </td>
 <td style="color: black; border: 1px solid black; text-align: center;">pH < 7 </td>
 </tr>
 <tr>
 <td style="color: black; border: 1px solid black; text-align: center;">neutre </td>
 <td style="color: black; border: 1px solid black; text-align: center;">[H3O+] = [OH−] </td>
 <td style="color: black; border: 1px solid black; text-align: center;">pH = 7 </td>
 </tr>
 <tr>
 <td style="color: black; border: 1px solid black; text-align: center;">basique </td>
 <td style="color: black; border: 1px solid black; text-align: center;">[H3O+] < [OH−] </td>
 <td style="color: black; border: 1px solid black; text-align: center;">pH > 7 </td>
 </tr>
 </tbody>
 </table>
 Ce texte est adapté de<a href="https://openstax.org/books/chemistry-2e/pages/14-1-bronsted-lowry-acids-and-bases"> Openstax, Chimie 2e, Section 14.1 : Acides et bases de Brønsted-Lowry</a>, et <a href="https://openstax.org/books/chemistry-2e/pages/14-2-ph-and-poh"> Section 14.2 : pH et pOH</a>.

L'eau : un acide et une base selon Bronsted-Lowry

La réaction entre un acide de Brønsted-Lowry et l’eau est appelée ionisation acide. Par exemple, lorsque le fluorure d’hydrogène se dissout dans l’eau et s’ionise, ...

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water as an amphiprotic substance

Water can act as both a Brønsted-Lowry acid and a Brønsted-Lowry base. When hydrogen fluoride dissolves in water, it donates protons to water. This is acid ionization. The products are hydronium ions and fluoride ions.

Water can also accept protons from another substance. When pyridine dissolves in water, it accepts a proton from water molecules. This is base ionization. The products are hydroxide ions and pyridinium ions.

These reactions show that water can play either role. A substance that can donate or accept protons is called amphiprotic. The broader term amphoteric is also used for substances that can act as acids or bases under different definitions. Bicarbonate ion is another amphiprotic species. It can react with water as an acid or as a base, and both equilibria can be present at the same time in solution.

Liquid water can also react with itself. This process is called autoionization. It happens only to a very small extent. At 25 °C, about two out of every billion water molecules are ionized. The equilibrium constant for this process is the ion-product constant for water, K_w, and its value is 1.0 × 10^-14 at 25 °C.

Autoionization is endothermic, so more ionization occurs as temperature rises. At 100 °C, K_w is about 5.6 × 10^-13, which is roughly 50 times larger than at 25 °C. Pure water always produces equal amounts of hydronium and hydroxide ions through this process. A solution is neutral when these ion concentrations are equal. It is acidic when hydronium ion concentration is greater than hydroxide ion concentration, and basic when hydroxide ion concentration is greater. At 25 °C, acidic solutions have pH below 7, neutral solutions have pH 7, and basic solutions have pH above 7.

Water as an Amphiprotic Substance

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Proton Transfer in Acids and Bases

Acids and bases can be understood through proton transfer. Early scientists described acids by their sour taste, their effect on dyes, and their reaction with limestone, which releases carbon dioxide. Robert Boyle also noted that acid solutions can lose these properties after contact with alkali, or base, solutions. The modern view developed step by step. Humphry Davy showed that hydrogen is the essential part of acids. Joseph Louis Gay-Lussac then described acids as substances that neutralize...

water: a bronsted-lowry acid and base

Water can act as both a Brønsted-Lowry acid and a Brønsted-Lowry base. When hydrogen fluoride dissolves in water, it donates protons to water. This is acid ionization. The products are hydronium ions and fluoride ions. Water can also accept protons from another substance. When pyridine dissolves in water, it accepts a proton from water molecules. This is base ionization. The products are hydroxide ions and pyridinium ions. These reactions show that water can play either role. A substance that...

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Salt hydrolysis explains why some salt solutions are acidic, basic, or neutral. Salts are ionic compounds made of cations and anions. In water, either ion may react with water through an acid or base ionization reaction. The pH of the solution depends on the relative acid-base strength of the ions in the salt. Ammonium chloride is a good example of an acidic salt. When it dissolves, it separates into ammonium ions and chloride ions. The ammonium ion is the conjugate acid of ammonia, so it can...

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Acid and base strength in water depends on how much a substance ionizes after it dissolves. If ionization is nearly complete, the substance is called strong. If only a small amount ionizes, it is called weak. Weak acids and weak bases are much more common than strong ones. The most common strong acids are HClO4, HCl, HBr, HI, HNO3, and H2SO4. The most common strong bases are LiOH, NaOH, KOH, Ca(OH)2, Sr(OH)2, and Ba(OH)2. These strong acids and bases ionize essentially completely in water. <br...

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Learn how water can act as both an acid and a base, why it is amphiprotic, and how autoionization affects hydronium, hydroxide, and pH.

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Water as an Amphiprotic Substance

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