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You create a 0.578 M solution of acetic acid (HC2H3O2, Ka = 1.8*10-5). Which of the...

You create a 0.578 M solution of acetic acid (HC2H3O2, Ka = 1.8*10-5). Which of the following represents the correct Ka expression for this reaction?

1.Ka = [HC2H3O2]/([H+][C2H3O2-])

2.Ka = [H+][C2H3O2-]/[HC2H3O2]

3.Ka = [H+][OH-]

Solve for x: you will get two possible values. After, plug both x values back into the original ICE table to determine the appropriate x value.

What is the [H+] in molarity at equilibrium?

What is the percent ionization for this reaction?

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