Name: proton transfer in acids and bases
Uploaded: 2020-09-24T15:06:51.000Z
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Bronsted-Lowry Acids and Bases

Un acide d'Arrhenius est une substance qui produit un ion hydrogène lorsqu'il est dissous dans l'eau et une base d'Arrhenius est une substance qui produit un OH⁻ou un ion hydroxyde. L'acide chlorhydrique est un acide d'Arrhenius comme il se dissocie en un ion d'hydrogène et un ion de chlorure lorsqu'il est dissous dans l'eau. L'hydroxyde de sodium est une base d'Arrhenius puisqu'il se dissocie en un ion de sodium et un ion d'hydroxyde lorsqu'il est dissous dans l'eau.Cependant, cette définition ne peut être utilisée pour décrire les acides et des bases qui ne sont pas dans une solution aqueuse ou des bases qui ne contiennent pas d'ions d'hydroxyde. Selon une définition plus large de Brønsted et Lowry, un acide est un ion d'hydrogène ou un donneur de proton, tandis qu'une base est un accepteur de proton. Lorsque l'acide chlorhydrique est dissous dans l'eau, il agit comme un acide en donnant un proton à l'eau, produisant un ion hydronium et un ion de chlorure.Lorsque l'ammoniac est dissous dans l'eau, il agit comme une base et accepte un proton de l'eau, produisant un ion d'ammonium et un ion d'hydroxyde. Un acide Brønsted-Lowry réagira toujours avec une base Brønsted-Lowry et vice versa. Lorsqu'un acide, par exemple l'acide acétique, donne son proton, l'eau sert de base et accepte le proton.Acide acétique est converti en une base conjuguée, acétate, et l'eau est convertie en un acide conjugué, un ion d'hydronium. Les acides et les bases qui diffèrent les uns des autres par le transfert d'un proton sont appelés paires acide-base conjuguées. Dans la réaction inverse, l'acide conjugué, l'hydronium, agit comme un donneur de protons et la base conjuguée, acétate, acceptera un proton.La force d'un acide est déterminée par sa capacité de donner un proton alors que la force d'une base est déterminée par sa capacité à accepter un proton. Un acide plus fort est plus susceptible de donner un proton qu'un acide plus faible. De même, une base plus forte est plus susceptible d'accepter un proton qu'une base plus faible.La force d'un acide et de sa base conjuguée est inversement liée. Un acide fort se dissocie complètement en solution et la base conjuguée résultante est trop faible pour accepter un proton. Il en va de même dans le cas d'une base solide et son acide conjugué.D'autre part, un acide faible se dissocie partiellement en solution. La base conjuguée d'un acide faible est également relativement faible;par conséquent, un mélange de l'acide faible non dissocié et sa base conjuguée faible sera présente en équilibre. Le même phénomène se produit dans le cas d'une base faible et son acide conjugué faible.

<ol>
	<li>Story, David A. « Examen du laboratoire au chevet du patient : une brève histoire de l’acide-base clinique. » Soins intensifs 8, n° 4 (2004) : 253.</li>
</ol>

acides et bases de bronsted-lowry

La catégorie des réactions acido-basiques a été étudiée depuis un certain temps. En 1680, Robert Boyle a exposé des traits des solutions acides qui incluent leur capacité à dissoudre de nombreuses substances, à changer les couleurs de certains colorants naturels et à perdre ces traits après avoir été en contact avec des solutions alcalines (basiques). Au XVIIIe siècle, il a été reconnu que les acides ont un goût aigre, qu'ils réagissent avec le calcaire pour libérer une substance gazeuse (on sait maintenant que c'est du CO2) et interagissent avec les alcalis pour former des substances neutres. En 1815, Humphry Davy a grandement contribué au développement du concept acido-basique moderne en démontrant que l'hydrogène est le constituant essentiel des acides. À peu près à la même époque, Joseph Louis Gay-Lussac a conclu que les acides sont des substances qui peuvent neutraliser les bases et que ces deux catégories de substances ne peuvent être définies qu'en termes l'une de l'autre. L'importance de l'hydrogène a été soulignée en 1884 lorsque Svante Arrhénius a défini un acide comme un composé qui se dissout dans l'eau pour produire des cations hydrogène (maintenant reconnus comme étant des ions hydronium) et une base comme un composé qui se dissout dans l'eau pour produire des anions hydroxyde. 
 Acides et bases de Brønsted-Lowry 
 Johannes Brønsted et Thomas Lowry ont proposé en 1923 une description plus générale dans laquelle les acides et les bases sont définis en termes de transfert d'ions hydrogène, H+ (notez que ces ions hydrogène sont souvent appelés simplement des protons, puisque cette particule subatomique est la seule composante des cations dérivés de l'isotope d'hydrogène le plus abondant, 1H). Un composé qui donne un proton à un autre composé est appelé un acide de Brønsted-Lowry, et un composé qui accepte un proton est appelé une base de Brønsted-Lowry. Une réaction acido-basique est donc le transfert d'un proton d'un donneur (acide) à un accepteur (base). 
 Le concept des couples conjugués est utile pour décrire les réactions acido-basiques de Brønsted-Lowry (ainsi que d'autres réactions réversibles). Lorsqu'un acide donne H+, l'espèce qui reste est appelée la base conjuguée de l'acide parce qu'elle réagit comme un accepteur de proton dans la réaction inverse. De même, lorsqu'une base accepte H+, elle est transformée en son acide conjugué. La réaction entre l'eau et l'ammoniac illustre cette idée comme indiqué ci-dessous. 
  <img alt="Eq1" src="/files/ftp_upload/11394/11394_Equation_1.png" style="height: 50px;" />
 Dans le sens direct, l'eau agit comme un acide en donnant un proton à l'ammoniac et en devenant par la suite un ion hydroxyde, OH−, la base conjuguée de l'eau. L'ammoniac sert de base pour accepter ce proton, devenant un ion ammonium, NH4+, l'acide conjugué de l'ammoniac. Dans le sens inverse, un ion hydroxyde sert de base pour accepter un proton de l'ion ammonium, qui agit comme un acide. 
 Les acides forts et les bases fortes se dissocient complètement dans une solution. Leurs bases et leurs acides conjugués sont extrêmement faibles et ne peuvent pas donner ou accepter les protons, respectivement, pour effectuer la réaction inverse ; par conséquent, les réactions impliquant des acides forts et des bases fortes sont essentiellement terminées dans une solution aqueuse. D'autre part, les acides et les bases faibles se dissocient partiellement en solutions et produisent respectivement des bases et des acides conjugués faibles. Ces acides ou bases conjugués faibles peuvent effectuer la réaction inverse, et donc les réactions d'acide et de base faibles atteignent un équilibre en fonction des forces relatives des acide et base faibles. En résumé, un acide plus fort produira la base conjuguée qui est d'autant plus faible, alors qu'une base plus forte produira un acide conjugué d'autant plus faible et vice versa. Le tableau 1 illustre la relation entre les différents couples acides/bases conjugués. 
 <table style="margin-left: auto; margin-right: auto;">
 <tbody>
 <tr>
 <td style="color: black; border: 1px solid black; text-align: center;">Acide fort </td>
 <td style="color: black; border: 1px solid black; text-align: center;">Base conjuguée très faible </td>
 </tr>
 <tr>
 <td style="color: black; border: 1px solid black; text-align: center;">HCl </td>
 <td style="color: black; border: 1px solid black; text-align: center;">Cl−</td>
 </tr>
 <tr>
 <td style="color: black; border: 1px solid black; text-align: center;">HNO3</td>
 <td style="color: black; border: 1px solid black; text-align: center;">NO3− </td>
 </tr>
 <tr>
 <td colspan="2"></td>
 </tr>
 <tr>
 <td style="color: black; border: 1px solid black; text-align: center;">Acide faible </td>
 <td style="color: black; border: 1px solid black; text-align: center;">Base conjuguée faible </td>
 </tr>
 <tr>
 <td style="color: black; border: 1px solid black; text-align: center;">HF </td>
 <td style="color: black; border: 1px solid black; text-align: center;">F− </td>
 </tr>
 <tr>
 <td style="color: black; border: 1px solid black; text-align: center;">NH4+ </td>
 <td style="color: black; border: 1px solid black; text-align: center;">NH3</td>
 </tr>
 <tr>
 <td colspan="2"></td>
 </tr>
 <tr>
 <td style="color: black; border: 1px solid black; text-align: center;">Acide très faible </td>
 <td style="color: black; border: 1px solid black; text-align: center;">Base conjuguée forte </td>
 </tr>
 <tr>
 <td style="color: black; border: 1px solid black; text-align: center;">OH− </td>
 <td style="color: black; border: 1px solid black; text-align: center;">O2−</td>
 </tr>
 <tr>
 <td style="color: black; border: 1px solid black; text-align: center;">CH4</td>
 <td style="color: black; border: 1px solid black; text-align: center;">CH3− </td>
 </tr>
 </tbody>
 </table>
 Tableau 1 : force relative de quelques couples acide/base conjugués. 
 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 14.4 Acide et base de Brønsted-Lowry</a>.

Acides et bases de Bronsted-Lowry

La classe des réactions acido-basiques est étudiée depuis un certain temps. En 1680, Robert Boyle a rapporté des caractéristiques des solutions acides qui comprenaient leur capacité à ...

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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 bases. In 1884, Svante Arrhenius defined acids as compounds that produce hydrogen cations in water and bases as compounds that produce hydroxide anions.

Brønsted and Lowry gave a broader definition in 1923. A Brønsted-Lowry acid donates a proton, and a Brønsted-Lowry base accepts a proton. An acid-base reaction is the transfer of that proton from the donor to the acceptor. The hydrogen ion, H+, is often called a proton because it is the only particle in the most common hydrogen isotope.

Conjugate pairs help describe these reactions. After an acid donates H+, the species left behind is its conjugate base. After a base accepts H+, it becomes its conjugate acid. Water and ammonia show this clearly. In the forward direction, water donates a proton to ammonia, so water acts as an acid and becomes hydroxide, OH−, while ammonia acts as a base and becomes ammonium, NH4+.

The reverse reaction also fits the same pattern. Hydroxide can accept a proton, so it acts as a base. Ammonium can donate a proton, so it acts as an acid. Strong acids and strong bases dissociate completely in solution, and their conjugate acids and bases are extremely weak. That is why reactions with strong acids and bases in water usually go to completion.

Weak acids and weak bases behave differently. They only partially dissociate in solution and form weak conjugate bases or weak conjugate acids. These conjugate species can take part in the reverse reaction, so weak acid-base reactions reach equilibrium. In general, a stronger acid gives a weaker conjugate base, and a stronger base gives a weaker conjugate acid.

Proton Transfer in Acids and Bases

bronsted-lowry 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...

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Brønsted-Lowry acid-base chemistry is based on proton transfer. That idea helps show how the strength of an acid is linked to the strength of its conjugate base, and vice versa. Acid and base strength is measured with ionization constants, Ka and Kb, which tell how far an ionization reaction goes. For the conjugate pair HA and A−, the acid ionizes in water and the base reaction can be written for the partner species. When the two reactions are added, they give the autoionization of water. The...

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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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Electron-pair reactions explain Lewis acid-base chemistry. In 1923, G. N. Lewis described acids and bases by how they accept or donate a pair of electrons. When that electron pair forms a coordinate covalent bond, one atom supplies both bonding electrons. This bond is also called a dative bond. A simple example is the reaction of water with a hydrogen ion to make a hydronium ion. Ammonia can also combine with a hydrogen ion to form an ammonium ion. In both cases, the reaction creates a Lewis...

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Learn how Brønsted-Lowry acids and bases work through proton transfer, conjugate pairs, and the difference between strong and weak acid-base reactions.

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Proton Transfer in Acids and Bases

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