Predict the products of the following acid–base reactions.
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Identify the acid and base in the reaction. In this case, (CH3)3NH+ is the acid because it can donate a proton (H+), and -OH is the base because it can accept a proton.

Consider the acid-base reaction mechanism. The base (-OH) will accept a proton from the acid ((CH3)3NH+), leading to the formation of water (H2O) and the conjugate base of the acid.

Write the chemical equation for the proton transfer. The acid (CH3)3NH+ will lose a proton, forming (CH3)3N, and the base (-OH) will gain a proton, forming H2O.

Use MathML to represent the chemical equation:

{({CH 3}_{3} N)}_{H} + + - OH ⇌ {({CH 3}_{3} N)}_{+} + H O_{2}

Recognize the equilibrium nature of the reaction. The double arrow (⇌) indicates that the reaction can proceed in both directions, forming products and reactants until equilibrium is reached.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Acid-Base Reactions

Acid-base reactions involve the transfer of protons (H+) between reactants. In this context, the acid donates a proton to the base. The reaction between (CH3)3NH+ (a protonated amine) and -OH (a hydroxide ion) is a classic example where the base (OH-) will accept a proton from the acid (CH3)3NH+.

Conjugate Acid-Base Pairs

In an acid-base reaction, the acid and base react to form their conjugate base and conjugate acid, respectively. For (CH3)3NH+, the conjugate base is (CH3)3N, and for -OH, the conjugate acid is H2O. Understanding these pairs helps predict the products of the reaction.

Equilibrium in Acid-Base Reactions

Acid-base reactions can reach an equilibrium where the forward and reverse reactions occur at the same rate. The position of equilibrium depends on the relative strengths of the acids and bases involved. In this reaction, equilibrium will favor the formation of the weaker acid and base, which are (CH3)3N and H2O.

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