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Ionic Equilibrum question

2001 · Q119
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Ionic Equilibrum question

2001 · Q119

NEETChemistryIonic EquilibrumMCQ+4 / −1
Ionisation constant of CH3COOH is 1.7 ×\times× 10−-−5 and concentration of H+ ions is 3.4 ×\times× 10−-−4. Then find out initial concentration of CH3COOH molecules.
  1. A
    3.4 ×\times× 10−-−4
  2. B
    3.4 ×\times× 10−-−3
  3. C
    6.8 ×\times× 10−-−4
  4. D
    6.8 ×\times× 10−-−3
View written solutionFree

Correct answer: D

CH3COOH ⇌ CH3COO–

  • H+

    Kc = [CH3COO−][H+][CH3COOH]{{{\left[ {C{H_3}CO{O^ - }} \right]\left[ {{H^ + }} \right]} \over {\left[ {C{H_3}COOH} \right]}}}[CH3​COOH][CH3​COO−][H+]​

    ⇒\Rightarrow⇒ [CH3COOH] = 3.4×10−4×3.4×10−41.7×10−5{{{3.4 \times {{10}^{ - 4}} \times 3.4 \times {{10}^{ - 4}}} \over {1.7 \times {{10}^{ - 5}}}}}1.7×10−53.4×10−4×3.4×10−4​

    = 6.8 × 10–3
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