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Chemistry · Ionic equilibrium: Weak and strong electrolytes, ionization of electrolytes

Aqueous solutions of and of identical concentrations are provided. The pair(s) o

Aqueous solutions of \( \boldsymbol{H} \boldsymbol{N} \boldsymbol{O}_{3}, \boldsymbol{K} \boldsymbol{O} \boldsymbol{H}, \boldsymbol{C} \boldsymbol{H}_{3} \boldsymbol{C O O H} \) and \( \boldsymbol{C H}_{3} \boldsymbol{C O O N a} \) of identical concentrations are provided. The pair(s) of solutions which form a buffer upon mixing are: This question has multiple correct options

  • A. \( \mathrm{HNO}_{3} \) and \( \mathrm{CH}_{3} \mathrm{COOH} \)
  • B. кОН апа СНзСООNa
  • C. \( \mathrm{HNO}_{3} \) and \( \mathrm{CH}_{3} \mathrm{COONa} \)
  • D. \( \mathrm{CH}_{3} \mathrm{COOH} \) and \( \mathrm{CH}_{3} \mathrm{COONa} \)

Step-by-step solution

A buffer requires a weak acid and its conjugate base. CH3COOH is a weak acid, and CH3COONa provides its conjugate base (CH3COO−). Options A (two acids) and B (strong base and salt) do not form buffers. Option C can produce a buffer only if HNO3 is limiting, but with equal concentrations and equal volumes, no buffer forms. Therefore, D is the unambiguous choice.
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