Arrhenius
Definition
Arrhenius acids are substances that increase the concentration of $H^+$ ions in aqueous solutions, while Arrhenius bases increase the concentration of $OH^-$ ions. This definition is fundamental to understanding acid-base reactions in water.
5 Must Know Facts For Your Next Test
- An Arrhenius acid dissociates in water to produce $H^+$ ions.
- An Arrhenius base dissociates in water to produce $OH^-$ ions.
- The strength of an Arrhenius acid or base depends on its degree of ionization in water.
- Common examples of Arrhenius acids include HCl and HNO3.
- Common examples of Arrhenius bases include NaOH and KOH.
Review Questions
- What ion does an Arrhenius acid release in water?
- Give an example of a common Arrhenius base.
- How does the strength of an Arrhenius acid relate to its ionization?
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Related terms
Brønsted-Lowry Acid: A substance that donates a proton ($H^+$) to another substance.
Brønsted-Lowry Base: A substance that accepts a proton ($H^+$) from another substance.
pH: A measure of the hydrogen ion concentration in a solution, indicating its acidity or basicity.
