Which of the following represents the ionic equation when H+ is added to a solution of acetic acid (CH3COOH) in water?

• A. CH3COOH + H+ → CH3COOH + H+
• B. CH3COOH + H+ → CH3COO- + H3O+
• C. CH3COOH + H+ → CH3COO- + H2O
• D. CH3COOH + H+ → CH3COOH2+

Answer: (A)

Verified step by step guidance

1. Identify the nature of acetic acid (CH3COOH) in water. Acetic acid is a weak acid that partially dissociates in water to form acetate ions (CH3COO-) and hydronium ions (H3O+).
2. Understand the role of H+ ions in the solution. When H+ ions are added to the solution, they can interact with water molecules to form hydronium ions (H3O+).
3. Consider the possible reactions. The addition of H+ to acetic acid in water can lead to the formation of acetate ions (CH3COO-) and hydronium ions (H3O+), as acetic acid donates a proton to water.
4. Write the ionic equation for the reaction. The equation should reflect the dissociation of acetic acid and the formation of hydronium ions: ${\text{CH}}_3{\text{COOH}}_{+}$
5. Verify the equation by checking the conservation of mass and charge. Ensure that the number of atoms and the charge are balanced on both sides of the equation.