Multiple Choice
A 16.4 mL aliquot of 0.182 M H3PO4 is to be titrated with 0.267 M NaOH. What volume (in mL) of the base will it take to reach the equivalence point?
17. Acid and Base Equilibrium
Acids Introduction
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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+
Verified step by step guidance1
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+).
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+).
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.
Write the ionic equation for the reaction. The equation should reflect the dissociation of acetic acid and the formation of hydronium ions:
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.
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