Name: water as an amphiprotic substance
Uploaded: 2020-09-24T15:06:51.000Z
Duration: 2 min 30 s
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Water: A Bronsted-Lowry Acid and Base

Ein amphoteres Molekül ist in der Lage, sowohl als Säure als auch als Base zu wirken. Wasser ist ein Beispiel für ein amphoteres Molekül.
In einer wässrigen Lösung von Ammoniak kann Wasser als Säure wirken, indem es ein Proton an Ammoniak, eine Base, abgibt. Im Gegensatz dazu wirkt Wasser als Base in einer wässrigen Salzsäurelösung, indem es ein Proton aus der Säure aufnimmt.
Da es amphoter ist, kann Wasser einer Autoionisation unterzogen werden. Bei diesem Prozess fungiert ein Wassermolekül als Säure, indem es ein Proton an ein anderes Wassermolekül abgibt, das als Base fungiert, indem es dieses Proton aufnimmt.
Dabei entstehen ein Hydronium-Ion und ein Hydroxid-Ion.
Die Gleichgewichtskonstante für die Autoionisation von Wasser, KW, auch Ionenproduktkonstante für Wasser genannt, hat einen Wert von 1 × 10−14. Sein Gleichgewichtsausdruck wird als die Konzentration der Hydroniumionen multipliziert mit der Konzentration der Hydroxidionen geschrieben, ohne Nenner, da beide Reaktanten Flüssigkeiten sind. 
In reinem Wasser bei 25 °C sind die Konzentrationen von Hydronium- und Hydroxidionen gleich, d. h. 1 × 10−7 M. 
KW kann verwendet werden, um die Konzentration von Hydronium- und Hydroxidionen in einer Lösung zu berechnen und um zu bestimmen, ob eine Lösung sauer oder basisch ist.
Wenn eine Lösung sauer ist, ist die Konzentration der Hydronium-Ionen höher als die der Hydroxid-Ionen. Wenn eine Lösung dagegen basisch ist, ist die Konzentration der Hydroxidionen höher als die der Hydroniumionen.
Wenn die Konzentration von Hydroniumionen in Lösung 5 × 10−7 M beträgt, kann die Hydroxidionenkonzentration mit KW bestimmt werden.
Da die Werte von KW und Hydroniumionen bekannt sind, kann die Konzentration von Hydroxidionen auf 2 × 10−8 M berechnet werden.
Da die Hydroniumionenkonzentration von 5 × 10−7 M höher ist als die Hydroxidionenkonzentration von 2 × 10−8 M, ist die Lösung sauer.

wasser: eine bronsted-lowry-säure und base

Die Reaktion zwischen einer Brønsted-Lowry-Säure und Wasser wird Säureionisierung genannt. Wenn sich beispielsweise Fluorwasserstoff in Wasser löst und ionisiert, werden Protonen von Fluorwasserstoffmolekülen auf Wassermoleküle übertragen, wodurch Hydroniumionen und Fluoridionen entstehen:  <img alt="Image1" src="/files/ftp_upload/11396/11396_Image_1.svg" style="height: 125px;"> Die Basionisierung einer Spezies erfolgt, wenn sie Protonen von Wassermolekülen aufnimmt. Im folgenden Beispiel unterliegen Pyridinmoleküle, C5NH5, einer Basenionisierung, wenn sie in Wasser gelöst werden, wodurch Hydroxid- und Pyridiniumionen entstehen:  <img alt="Image2" src="/files/ftp_upload/11396/11396_image 2v2.svg" style="height: 190px;"> Die vorangegangenen Ionisierungsreaktionen legen nahe, dass Wasser sowohl als Base (wie bei seiner Reaktion mit Fluorwasserstoff) als auch als Säure (wie bei seiner Reaktion mit Ammoniak) fungieren kann. Spezies, die in der Lage sind, Protonen entweder abzugeben oder aufzunehmen, werden als amphiprotisch oder allgemeiner als amphoter bezeichnet. Dieser Begriff kann für Säuren und Basen gemäß anderen Definitionen als der von Brønsted-Lowry verwendet werden. Die folgenden Gleichungen zeigen die beiden möglichen Säure-Base-Reaktionen für zwei amphiprotische Spezies, Bicarbonat-Ion und Wasser:  <img alt="Equation1" src="/files/ftp_upload/11396/11396_Equation_1.png" style="height: 95px;"> Die erste Gleichung stellt die Reaktion von Bicarbonat als Säure mit Wasser als Base dar, während die zweite die Reaktion von Bicarbonat als Base mit Wasser als Säure darstellt. Bei der Zugabe von Bicarbonat zu Wasser stellen sich beide Gleichgewichte gleichzeitig ein und die Zusammensetzung der resultierenden Lösung kann durch entsprechende Gleichgewichtsberechnungen bestimmt werden. Im flüssigen Zustand können Moleküle einer amphiprotischen Substanz miteinander reagieren, wie die folgenden Gleichungen für Wasser zeigen:  <img alt="Image3" src="/files/ftp_upload/11396/11396_image_3.svg" style="height: 125px;"> Der Prozess, bei dem gleichartige Moleküle unter Bildung von Ionen reagieren, wird Autoionisierung genannt. Flüssiges Wasser erfährt in sehr geringem Maße eine Autoionisierung; Bei 25 °C sind etwa zwei von einer Milliarde Wassermoleküle ionisiert. Das Ausmaß des Autoionisierungsprozesses von Wasser spiegelt sich im Wert seiner Gleichgewichtskonstante, der Ionenproduktkonstante für Wasser, KW, wider:  <img alt="Equation2" src="/files/ftp_upload/11396/11396_Equation_2.png" style="height: 50px;"> Die leichte Ionisierung von reinem Wasser spiegelt sich im kleinen Wert der Gleichgewichtskonstante wider; Bei 25 °C hat KW einen Wert von 1,0 × 10−14.  <img alt="Equation3" src="/files/ftp_upload/11396/11396_Equation_3.png" style="height: 50px;"> Der Prozess ist endotherm, daher nehmen das Ausmaß der Ionisierung und die daraus resultierenden Konzentrationen an Hydroniumionen und Hydroxidionen mit der Temperatur zu. Bei 100 °C beträgt der Wert für KW beispielsweise etwa 5,6 × 10−13, etwa 50-mal größer als der Wert bei 25 °C. Die Autoionisierung von Wasser ergibt die gleiche Anzahl an Hydronium- und Hydroxidionen. Daher gilt in reinem Wasser bei 25 °C:  <img alt="Equation4" src="/files/ftp_upload/11396/11396_Equation_4.png" style="height: 50px;"> Die Konzentrationen dieser Ionen in einer Lösung sind oft entscheidende Faktoren für die Eigenschaften der Lösung und das chemische Verhalten ihrer anderen gelösten Stoffe, und es wurde ein spezielles Vokabular entwickelt, um diese Konzentrationen relativ zu beschreiben. Eine Lösung ist neutral, wenn sie gleiche Konzentrationen an Hydronium- und Hydroxidionen enthält; sauer, wenn es eine größere Konzentration an Hydroniumionen als Hydroxidionen enthält; und basisch, wenn es eine geringere Konzentration an Hydroniumionen als Hydroxidionen enthält. Zusammenfassung der Beziehungen für saure, basische und neutrale Lösungen <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;">Relative Ion Concentrations</td> <td style="color: black; border: 1px solid black; text-align: center;">pH at 25 °C</td> </tr> <tr> <td style="color: black; border: 1px solid black; text-align: center;">acidic</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;">neutral</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;">basic</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> Dieser Text ist adaptiert von<a href="https://openstax.org/books/chemistry-2e/pages/14-1-bronsted-lowry-acids-and-bases"> Openstax, Chemistry 2e, Section 14.1: Brønsted-Lowry Acids and Bases</a>, and <a href="https://openstax.org/books/chemistry-2e/pages/14-2-ph-and-poh">Section 14.2: pH and pOH</a>

Wasser: Eine Bronsted-Lowry-Säure und Base

Die Reaktion zwischen einer Brønsted-Lowry-Säure und Wasser wird als saure Ionisation bezeichnet. Wenn sich beispielsweise Fluorwasserstoff in Wasser löst und ionisiert, ...

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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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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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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 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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