Name: acid and base strength in water
Uploaded: 2025-10-30T13:58:47.000Z
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Acid/Base Strengths and Dissociation Constants

Säuren und Basen können danach kategorisiert werden, ob es sich um eine starke Säure, eine starke Base, eine schwache Säure oder eine schwache Base handelt. Es gibt nur sehr wenige starke Säuren und Basen, so dass die meisten Säuren und Basen schwach sind.
Eine starke Säure, wie Salzsäure, dissoziiert vollständig in Wasserstoffionen und Chloridionen, wenn sie in Wasser gelöst wird. Eine starke Base dissoziiert wie Natriumhydroxid vollständig in Natriumionen und Hydroxidionen.
Schwache Säuren und Basen dissoziieren teilweise und liegen sowohl in ionisierter als auch in unionisierter Form vor. Zum Beispiel finden sich sowohl Essigsäure als auch ihre schwache konjugierte Base, Acetat, in einer wässrigen Lösung.
Der Dissoziationsgrad einer schwachen Säure oder Base kann anhand ihrer Gleichgewichtskonstante gemessen werden. Die Gleichgewichtskonstante für schwache Säuren hat einen besonderen Namen, die Säuredissoziationskonstante oder Ka.
Für eine generische schwache Säure HA kann Ka bei einer gegebenen Temperatur durch eine Gleichgewichtsgleichung berechnet werden, bei der die Konzentration der Produkte A-Ion und Hydronium-Ion durch die Konzentration der Reaktanten HA und Wasser dividiert wird.
Da Wasser flüssig ist und seine Konzentration in der Reaktion nahezu unverändert bleibt, wird es aus der Gleichung ausgeschlossen.
Je höher das Ka, desto stärker die Säure. Salpetrige Säure ist stärker als Essigsäure, da das Ka der salpetrigen Säure größer ist als das Ka der Essigsäure. 
Die Gleichgewichtskonstante für schwache Basen, die Basendissoziationskonstante oder Kb, verhält sich ähnlich wie Ka. Für eine generische schwache Base B kann Kb bei einer gegebenen Temperatur bestimmt werden, indem die Konzentration der Produkte BH-Ion und Hydroxid-Ion durch die Konzentration des Reaktanten B dividiert wird.
Wie bei Säuren ist auch die Stärke der Basen direkt proportional zum Kb. Zum Beispiel ist Ethylamin relativ stärker als Harnstoff, da das Kb von Ethylamin größer ist als das Kb von Harnstoff. 
Die Stärke einer Säure kann auch in Prozent der Ionisation ausgedrückt werden. Die prozentuale Ionisation einer Säure kann berechnet werden, indem die Hydroniumionenkonzentration im Gleichgewicht durch die anfängliche Säurekonzentration dividiert und mit hundert multipliziert wird. 
In ähnlicher Weise kann die prozentuale Ionisation für Basen berechnet werden, indem die Hydroxidionenkonzentration im Gleichgewicht durch die Anfangskonzentration der Base dividiert und mit hundert multipliziert wird. Je höher die prozentuale Ionisation, desto stärker die Säure oder Base.

säure-/basestärken und dissoziationskonstanten

Die relative Stärke einer Säure oder Base ist das Ausmaß, in dem sie ionisiert, wenn sie in Wasser gelöst wird. Wenn die Ionisierungsreaktion im Wesentlichen abgeschlossen ist, wird die Säure oder Base als stark bezeichnet; Wenn relativ wenig Ionisierung auftritt, ist die Säure oder Base schwach. Es gibt viel mehr schwache Säuren und Basen als starke. Die häufigsten starken Säuren und Basen sind unten aufgeführt: <table style="margin-left: auto; margin-right: auto;"> <tbody> <tr> <td style="color: black; border: 1px solid black; text-align: center;">Strong Acids</td> <td style="color: black; border: 1px solid black; text-align: center;">Strong Bases</td> </tr> <tr> <td style="color: black; border: 1px solid black; text-align: center;">HClO4</td> <td style="color: black; border: 1px solid black; text-align: center;">LiOH</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;">NaOH</td> </tr> <tr> <td style="color: black; border: 1px solid black; text-align: center;">HBr</td> <td style="color: black; border: 1px solid black; text-align: center;">KOH</td> </tr> <tr> <td style="color: black; border: 1px solid black; text-align: center;">HI</td> <td style="color: black; border: 1px solid black; text-align: center;">Ca(OH)2</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;">Sr(OH)2</td> </tr> <tr> <td style="color: black; border: 1px solid black; text-align: center;">H2SO4</td> <td style="color: black; border: 1px solid black; text-align: center;">Ba(OH)2</td> </tr> </tbody> </table> Die relativen Stärken von Säuren können durch Messung ihrer Gleichgewichtskonstanten in wässrigen Lösungen quantifiziert werden. In Lösungen gleicher Konzentration ionisieren stärkere Säuren stärker und liefern daher höhere Konzentrationen an Hydroniumionen als schwächere Säuren. Die Gleichgewichtskonstante einer Säure wird Säureionisationskonstante Ka genannt. Für die Reaktion einer Säure HA: <img alt="Eq1" src="/files/ftp_upload/11395/11395eq1.png" style="text-align: center; height: 50px;"> Die Säureionisationskonstante wird geschrieben als  <img alt="Eq2" src="/files/ftp_upload/11395/11395eq2.png" style="text-align: center; height: 90px;"> 

 wobei die Konzentrationen diejenigen im Gleichgewicht sind. Obwohl Wasser ein Reaktant in der Reaktion ist, ist es auch das Lösungsmittel, daher beziehen wir [H2O] nicht in die Gleichung ein. Je größer der Ka einer Säure, desto größer ist die Konzentration von H3O+ und A− im Verhältnis zur Konzentration der nichtionisierten Säure HA in einer Gleichgewichtsmischung und desto stärker ist die Säure. Eine Säure wird als „stark“ klassifiziert, wenn sie vollständig ionisiert ist. In diesem Fall ist die HA-Konzentration Null und die Ionisationskonstante der Säure ist unermesslich groß (Ka ≈ ∞). Teilweise ionisierte Säuren werden als „schwach“ bezeichnet und ihre Säureionisationskonstanten können experimentell gemessen werden. 

 Um diese Idee zu veranschaulichen, werden unten drei Säureionisationsgleichungen und Ka-Werte gezeigt. Die Ionisationskonstanten nehmen von der ersten zur letzten der aufgeführten Gleichungen zu, was darauf hinweist, dass die relative Säurestärke in der Reihenfolge CH3CO2H < HNO2 < HSO4− zunimmt. 

 <img alt="Eq3-5" src="/files/ftp_upload/11395/11395eq3-5.png" style="text-align: center; height: 135px;"> 

 Ein weiteres Maß für die Stärke einer Säure ist der Ionisierungsgrad. Der Prozentsatz der Ionisierung einer schwachen Säure wird anhand der Zusammensetzung einer Gleichgewichtsmischung definiert:  

 <img alt="Eq6" src="/files/ftp_upload/11395/11395eq6.png" style="text-align: center; height: 90px;"> wobei der Zähler der Konzentration der konjugierten Base der Säure entspricht (per Stöchiometrie, [A−] = [H3O+]). Im Gegensatz zum Ka-Wert variiert der Prozentsatz der Ionisierung einer schwachen Säure mit der anfänglichen Säurekonzentration und nimmt typischerweise mit zunehmender Konzentration ab. Wie bei Säuren spiegelt sich die relative Stärke einer Base in der Größe ihrer Basenionisationskonstante (Kb) in wässrigen Lösungen wider. In Lösungen gleicher Konzentration ionisieren stärkere Basen stärker und liefern daher höhere Hydroxidionenkonzentrationen als schwächere Basen. Eine stärkere Base hat eine größere Ionisationskonstante als eine schwächere Base. Für die Reaktion einer Base, B:  <img alt="Eq7" src="/files/ftp_upload/11395/11395eq7.png" style="text-align: center; height: 50px;"> Die Ionisationskonstante wird geschrieben als  <img alt="Eq8" src="/files/ftp_upload/11395/11395eq8.png" style="text-align: center; height: 90px;"> Die Betrachtung der unten dargestellten Daten für drei schwache Basen zeigt, dass die Basenstärke in der Reihenfolge NO2− < CH2 CO2− < NH3 zunimmt. <img alt="Eq9-11" src="/files/ftp_upload/11395/11395eq9-11.png" style="text-align: center; height: 135px;"> Wie bei Säuren spiegelt sich die relative Stärke einer Base auch in ihrem prozentualen Ionisierungsgrad wider, der wie folgt berechnet wird: <img alt="Eq12" src="/files/ftp_upload/11395/11395eq12.png" style="text-align: center; height: 90px;"> variiert jedoch abhängig von der Basisionisationskonstante und der Anfangskonzentration der Lösung. Dieser Text ist adaptiert von <a href="https://openstax.org/books/chemistry-2e/pages/14-3-relative-strengths-of-acids-and-bases">Openstax, Chemistry 2e, Section 14.3: Relative Strengths of Acids and Bases.</a>

Säure-/Basestärken und Dissoziationskonstanten

Die relative Stärke einer Säure oder Base ist das Ausmaß, in dem sie ionisiert, wenn sie in Wasser gelöst wird. Ist die Ionisationsreaktion im Wesentlichen abgeschlossen, ...

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acid and base strength in water

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.

Acid strength can be measured with the acid-ionization constant, Ka. For an acid HA in water, Ka compares the concentrations of the products and the nonionized acid at equilibrium. Water is a reactant in the reaction, but it is not included in the equation because it is the solvent. A larger Ka means more H3O+ and A− relative to HA, so the acid is stronger.

A strong acid is considered completely ionized. In that case, the concentration of HA is zero, and Ka is immeasurably large, or approximately infinite. Weak acids ionize only partially, so their Ka values can be measured in the lab. The relative acid strengths in the examples increase in the order CH3CO2H &lt; HNO2 &lt; HSO4−.

Percent ionization is another way to describe weak acid strength. It is based on the amount of acid that ionizes at equilibrium. For a weak acid, the percent ionization changes with the starting concentration and usually gets smaller as the concentration gets higher. This makes percent ionization different from Ka.

Base strength is measured in a similar way with the base-ionization constant, Kb. For a base B in water, a larger Kb means the base ionizes more and produces a higher hydroxide ion concentration. A stronger base has a larger ionization constant than a weaker base.

The examples of weak bases show the strength order NO2− &lt; CH2CO2− &lt; NH3. Base strength can also be described with percent ionization. As with weak acids, this value depends on both the base-ionization constant and the initial concentration of the solution.

Acid and Base Strength in Water

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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...

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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...

strong acid and base solutions

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acid/base strengths and dissociation constants

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 acid and base strength in water depends on ionization, Ka, Kb, and percent ionization, with examples of strong and weak acids and bases.

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Acids and Bases: Percent Dissociation and pH

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Acid and Base Strength in Water

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