Chapter 15: Problem 15

In the presence of water, the bicarbonate ion, \(\mathrm{HCO}_{3}^{-}\), can be either a BronstedLowry acid or a Bronsted-I.owry base. Write both equilibrium equations.

Short Answer

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The bicarbonate ion (HCO₃⁻) can act as a Bronsted-Lowry acid or base in the presence of water. As an acid, the equilibrium equation is \( HCO_{3}^{-} + H_{2}O \rightleftharpoons H_{3}O^{+} + CO_{3}^{2-} \). As a base, the equilibrium equation is \( HCO_{3}^{-} + H_{2}O \rightleftharpoons OH^{-} + H_{2}CO_{3} \).

Step by step solution

Understand Bronsted-Lowry Acid-Base Definition

A Bronsted-Lowry acid is a substance that can donate a proton (H⁺), while a Bronsted-Lowry base is a substance that can accept a proton (H⁺). In this case, we are given that the bicarbonate ion (HCO₃⁻) can act as both an acid and a base when dissolved in water.

Write the Acid Equilibrium Equation

When the bicarbonate ion (HCO₃⁻) acts as an acid, it donates a proton (H⁺) to a water molecule and forms hydronium ions (H₃O⁺) and carbonate ions (CO₃²⁻). The acid equilibrium equation can be written as: \[ HCO_{3}^{-} + H_{2}O \rightleftharpoons H_{3}O^{+} + CO_{3}^{2-} \]

Write the Base Equilibrium Equation

When the bicarbonate ion (HCO₃⁻) acts as a base, it accepts a proton (H⁺) from a water molecule and forms hydroxide ions (OH⁻) and carbonic acid (H₂CO₃). The base equilibrium equation can be written as: \[ HCO_{3}^{-} + H_{2}O \rightleftharpoons OH^{-} + H_{2}CO_{3} \] So, the two equilibrium equations representing bicarbonate ion (HCO₃⁻) as a Bronsted-Lowry acid and as a Bronsted-Lowry base in the presence of water are: \[ HCO_{3}^{-} + H_{2}O \rightleftharpoons H_{3}O^{+} + CO_{3}^{2-} \] \[ HCO_{3}^{-} + H_{2}O \rightleftharpoons OH^{-} + H_{2}CO_{3} \]

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In the presence of water, the bicarbonate ion, \(\mathrm{HCO}_{3}^{-}\), can be either a BronstedLowry acid or a Bronsted-I.owry base. Write both equilibrium equations.

Short Answer

Step by step solution

Understand Bronsted-Lowry Acid-Base Definition

Write the Acid Equilibrium Equation

Write the Base Equilibrium Equation

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