Amantadine, C10 H15 NH2, is a base used to treat Parkinson's...

Amantadine, $\mathrm{C}_{10} \mathrm{H}_{15} \mathrm{NH}_{2}$, is a base used to treat Parkinson's disease. Write a balanced chemical equation to represent why an aqueous solution of amantadine is basic.

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Key Concepts

Bronsted-Lowry Acid-Base Theory

This concept explains that acid-base reactions involve the transfer of a proton from an acid to a base. In the context of aqueous solutions, a base like an amine accepts a proton from water, which acts as the acid, producing its conjugate acid and hydroxide ions. This reaction is central to understanding why certain compounds create basic solutions when dissolved in water.

Amine Protonation Reaction

Amines contain a nitrogen atom with a lone pair of electrons, making them capable of accepting a proton from water. When an amine reacts with water, it forms a protonated amine (conjugate acid) and releases hydroxide ions, thereby increasing the basicity of the solution. This is a classic example of how organic bases behave in an aqueous environment.

Chemical Equilibrium in Aqueous Base Reactions

In aqueous solutions, many acid-base reactions are reversible and reach an equilibrium state. The reaction of an amine with water, which produces hydroxide ions, represents an equilibrium that defines the basicity of the solution. Understanding this equilibrium is key to predicting the pH and behavior of the solution.

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