What is the percent ionization of an acetic acid solution at the following concentrations? a. 1.00 M b. 0.500 M c. 0.100 M d. 0.0500 M

Verified step by step guidance

1. <insert step 1: Write the chemical equation for the ionization of acetic acid (CH3COOH) in water: CH3COOH (aq) ⇌ CH3COO^- (aq) + H^+ (aq).>
2. <insert step 2: Write the expression for the acid dissociation constant (Ka) for acetic acid: Ka = [CH3COO^-][H^+]/[CH3COOH].>
3. <insert step 3: Use the given concentration of acetic acid to set up an ICE (Initial, Change, Equilibrium) table to determine the equilibrium concentrations of the species involved.>
4. <insert step 4: Assume that the change in concentration of CH3COOH is x, and express the equilibrium concentrations in terms of x.>
5. <insert step 5: Solve for x using the Ka value for acetic acid (1.8 x 10^-5) and calculate the percent ionization using the formula: Percent Ionization = (x/initial concentration) * 100.>