11th Class Chemistry Equilibrium Question Bank 11th CBSE Chemistry Ionic Equilibrium

  • question_answer lonization constants \[{{K}_{a}}\] for formic acid and acetic acid are \[17\cdot \,7\times {{10}^{-5}}\] and \[1\cdot 77\times {{10}^{-5}}\]. Which acid is stronger and how many times the other if equimolar concentrations of the two are taken?


                      \[{{K}_{a}}\] for \[HCOOH>{{K}_{a}}\] for \[C{{H}_{3}}COOH\]. Hence, formic acid is stronger. \[\text{Further,}\,\,\frac{\text{Strength}\,\text{of}\,\text{HCOOH}}{\text{Strength}\,\text{of}\,\text{C}{{\text{H}}_{\text{3}}}\text{COOH}}\]\[\,=\sqrt{\frac{{{\text{K}}_{\text{HCOOH}}}}{{{\text{K}}_{\text{C}{{\text{H}}_{\text{3}}}\text{COOH}}}}}\,=\sqrt{10}\,=3\cdot 16\,\text{times}.\]

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