0.1 mole of acetic acid has been dissolved per dm3 of the solution, the percentage ionization of acetic acid will be
Correct answer: C. 1.3
- A. 13
- B. 15
- C. 1.3
- D. 0.1
Explanation
A, B and D are incorrect because these are not correct percentage ionization valuesC is correct since The solution is given as CH3COOH dissociates to a small extent:CH3COOH ↔ CH3COO- + H+Calculate [H+] from the Ka equation.Ka = [H+] [[CH3COO-] / [CH3COOH]Because [H+] =[CH3COO-] and dissociation is very small, we can write the equation asKa = [H+]² / 0.1Ka = 1.8*10-51.8*10-5 = [H+]² / 0.1[H+]² = (1.8*10-5)* 0.1[H+]² = 1.8*10-6[H+] = 0.0013M% dissociation = 0.0013/0.1*100 = 1.34%
This question appeared on the UHS MDCAT 2010 paper, which you can sit online with every answer explained.
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About pH and pOH
pH measures hydrogen ion concentration and pOH measures hydroxide ion concentration on a logarithmic scale. Calculations use pH = minus log of hydrogen ion concentration, pOH = minus log of hydroxide ion concentration and pH plus pOH equals pKw, with separate treatment of strong and weak acids and bases.
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