Based on these molecular views, determine whether each pictured acid is weak or strong.

Verified step by step guidance

1. Identify the species present in the solution: HCOOH (formic acid), HCOO- (formate ion), and H3O+ (hydronium ion).
2. Understand that a strong acid completely dissociates in water, while a weak acid only partially dissociates.
3. Observe the molecular view: there are both HCOOH molecules and HCOO- ions present, indicating that not all HCOOH has dissociated.
4. Note the presence of H3O+ ions, which are produced when an acid donates a proton to water.
5. Conclude that since both the undissociated form (HCOOH) and the dissociated form (HCOO-) are present, formic acid is a weak acid.

Key Concepts

Acid Strength

Acid strength refers to the ability of an acid to donate protons (H+) in a solution. Strong acids completely dissociate in water, releasing all their protons, while weak acids only partially dissociate. This distinction is crucial for understanding the behavior of acids in chemical reactions and their impact on pH levels.

Dissociation Equilibrium

Dissociation equilibrium describes the balance between the undissociated acid and its ions in solution. For weak acids, this equilibrium lies to the left, meaning that only a fraction of the acid molecules dissociate into ions. The presence of both the undissociated acid and its ions, as shown in the image, indicates that formic acid is a weak acid.

Conjugate Base

The conjugate base of an acid is the species that remains after the acid donates a proton. In the case of formic acid (HCOOH), its conjugate base is the formate ion (HCOO-). Understanding the relationship between an acid and its conjugate base is essential for predicting the behavior of acids in solution and their relative strengths.