Im neutralen Milieu ist die Konzentration der Oxonium-Ionen (H3O+) genauso groß wie die der Hydroxid-Ionen (OH-). In sauren Lösungen ist die Option Oxonium-Ionen-Konzentration größer, in alkalischen kleiner als die der Hydroxid-Ionen-Konzentration.

Nach Brönsted gehen bei einer Säure-Base-Reaktion immer Protonen (H+) von einer Säure- zu einem Base-Molekül über.

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Somit sind Säuren Protonendonatoren und Basen Protonenakzeptoren.

Gibt eine Säure ihr Proton ab, entsteht aus ihr die korrespondierende Base, nimmt eine Base ein Proton auf, entsteht aus ihr die korrespondierende Säure.

Moleküle die sowohl als Säure als auch als Base reagieren können, nennt man Ampholyte. Zu ihnen zählen z.B. Wasser und Ammoniak.

Reagiert eine Säure mit einer Base so neutralisieren sich die beiden Moleküle. Es entsteht ein Salz und MEIST auch Wasser.

Die Neutralisation verläuft exotherm, die freiwerdende Energie nennt man neutralisations Energie.

Säure + Base --> Salz + Wasser + Energie

Um messen zu können, ob eine Lösung sauer, alkalisch oder neutral reagiert, berechnet man den pH-Wert.

Der pH-Wert ist laut Definition der negative dekadische Logarithmus des Zahlenwertes der Oxonium-Ionen-Konzentration. Der pOH-Wert ist laut Definition der negative dekadische Logarithmus des Zahlenwertes der Hydroxid-Ionen-Konzentration. pH und pOH-Wert ergeben in der Summe immer 14. pH = -lg c(H3O+)

Auf einer Skala von 0 bis 14 bedeutet ein pH-Wert von 7 neutral, ein pH-Wert kleiner 7 sauer und größer 7 alkalisch.

Salzsäure ist eine wässrige Lösung von HCl; Natronlauge bzw. Kalilauge sind wässrige Lösungen von NaOH bzw. KOH; Kalkwasser bzw. Barytwasser sind wässrige Lösungen von Ca(OH)2 bzw. Na(OH)2.

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