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Chemistry · EQUILIBRIUM

हिन्दी

Which of the following conjugate bases is the strongest proton acceptor in aqueous solution?

  1. A
    \( \text{NO}_3^- \)
  2. B
    \( \text{Cl}^- \)
  3. C
    \( \text{NH}_2^- \)
  4. D
    \( \text{ClO}_4^- \)
View Answer & Solution

Correct answer · Option C

\( \text{NH}_2^- \)

Explanation

\( \text{NH}_3 \) is a very weak acid, so its conjugate base \( \text{NH}_2^- \) is an exceptionally strong base, far stronger than the conjugate bases of strong acids (\( \text{Cl}^-, \text{NO}_3^-, \text{ClO}_4^- \)).

Related questions

Given below are two statements:\n Statement I: Chemical equilibrium can be attained from either direction, whether starting with pure reactants or pure products.\n Statement II: The Law of Chemical Equilibrium and Law of Mass Action was proposed by Cato Maximillian Guldberg and Peter Waage in 1864. \nIn the light of the above statements, choose the most appropriate answer from the options given below:→For a 0.10 M aqueous solution of a diprotic acid \( \text{H}_2\text{X} \), the ionization constants are \( K_{a_1} = 4.0 \times 10^{-5} \) and \( K_{a_2} = 1.6 \times 10^{-11} \). The concentration of divalent anion \( [\text{X}^{2-}] \) at equilibrium is:→When \( \text{HCl} \) gas is passed through a saturated solution of \( \text{NaCl} \), pure \( \text{NaCl} \) precipitates out while impurities like \( \text{MgSO}_4 \) and \( \text{Na}_2\text{SO}_4 \) remain dissolved. The underlying reason for this phenomenon is:→In the equilibrium \( \text{Fe}^{3+}(\text{aq}) + \text{SCN}^-(\text{aq}) \rightleftharpoons [\text{Fe}(\text{SCN})]^{2+}(\text{aq}) \) (deep red), what happens to the red colour intensity upon the addition of oxalic acid \( (\text{H}_2\text{C}_2\text{O}_4) \) and why?→
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