Question

Pyruvic acid, \(\mathrm{CH}_{3} \mathrm{COCOOH},\) is produced during aerobic respiration. Write a balanced chemical equation to represent why an aqueous solution of pyruvic acid is acidic.

Short answer

Pyruvic acid ionizes in water to form pyruvate and hydronium ions, creating an acidic solution.

Step-by-step solution

Write the Chemical Formula for Pyruvic Acid

The chemical formula for pyruvic acid is \(\mathrm{CH}_3\mathrm{COCOOH}\). This formula shows that pyruvic acid contains a carboxyl group \(\mathrm{COOH}\), which is key to its acidic nature.

Ionization in Aqueous Solution

In an aqueous solution, pyruvic acid can donate a hydrogen ion (proton), \(\mathrm{H}^+\), from its carboxyl group to the water. This process is called ionization and it increases the concentration of hydrogen ions in the solution.

Write the Ionization Equation

When pyruvic acid ionizes in water, it forms pyruvate ions \(\mathrm{CH}_3\mathrm{COCOO}^-\) and hydronium ions \(\mathrm{H}_3\mathrm{O}^+\). The balanced chemical equation for this reaction is: \[\mathrm{CH}_3\mathrm{COCOOH} + \mathrm{H}_2\mathrm{O} \rightleftharpoons \mathrm{CH}_3\mathrm{COCOO}^- + \mathrm{H}_3\mathrm{O}^+\].

Explanation of Acidity

Pyruvic acid is considered acidic because it increases the concentration of hydronium ions \(\mathrm{H}_3\mathrm{O}^+\) in the solution due to the ionization of its carboxyl group. The presence of more \(\mathrm{H}_3\mathrm{O}^+\) ions in the solution is characteristic of acidic solutions.

Key concepts

Pyruvic Acid in Respiration

Pyruvic acid, chemically denoted as \( \mathrm{CH}_3\mathrm{COCOOH} \), serves an important role in metabolism, particularly during aerobic respiration. It is one of the key intermediates that cells use to produce energy. Let's break down a few essential points:

• Pyruvic acid originates from glucose breakdown during glycolysis.
• It contains a carboxyl group \( \mathrm{COOH} \), which imparts its acidic characteristics.
• This molecule is crucial for the aerobic conversion of glucose to energy, acting as a bridge to the Krebs cycle.

Without the presence of pyruvic acid in aerobic conditions, efficient energy production in cells would not be possible.
Understanding its dual nature as both a metabolic intermediate and an acidic compound is crucial for grasping basic cellular chemistry.

Ionization of Pyruvic Acid

When discussing pyruvic acid and its acidity, the concept of ionization becomes essential. Ionization is a process where molecules dissociate into ions when in solution, particularly in water. Here’s how it works with pyruvic acid:

• In water, pyruvic acid can release a proton (\( \mathrm{H}^+ \)) from its carboxyl group.
• This release increases the concentration of hydronium ions (\( \mathrm{H}_3\mathrm{O}^+ \)) in the solution.
• As a result, the solution becomes more acidic.

Pyruvic acid's ability to donate protons is integral to its behavior in biological and chemical systems. This proton donation, or ionization, transforms pyruvic acid into its conjugate base, known as pyruvate. The carboxyl group's ionization is a clear demonstration of why the acid can affect the solution's pH, confirming its acid-like properties.

Balancing Chemical Equations for Ionization

In chemistry, writing a balanced equation is crucial to accurately represent the molecules and ions involved in a reaction. For the ionization of pyruvic acid, such a balanced chemical equation highlights the complete process. The equation for pyruvic acid in water is:

\[\mathrm{CH}_3\mathrm{COCOOH} + \mathrm{H}_2\mathrm{O} \rightleftharpoons \mathrm{CH}_3\mathrm{COCOO}^- + \mathrm{H}_3\mathrm{O}^+\]

This equation provides a step-by-step look at what happens when pyruvic acid ionizes:

• The forward arrow indicates the release of \( \mathrm{H}^+ \) from the acid to become \( \mathrm{CH}_3\mathrm{COCOO}^- \) (pyruvate).
• The reversibility (\(\rightleftharpoons\)) signifies that this process can go back and forth under the right conditions.
• The addition of hydronium ions (\( \mathrm{H}_3\mathrm{O}^+ \)) shows the result of this ionization.

Writing chemical equations like these helps visualize and understand how acids behave in solutions, crucial for grasping their roles in both biological systems and chemical reactions.