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Determine the relative acid strengths of NH4 + and HCN by comparing their ionization constants. The ionization constant of HCN is given in Appendix H as 4.9 × 10−10. The ionization constant of NH4 + is not listed, but the ionization constant of its conjugate base, NH3, is listed as 1.8 × 10−5.

Respuesta :

Answer:

[tex]NH_{4}^{+}[/tex] is stronger acid than HCN

Explanation:

For a acid-conjugate base or base-conjugate acid pair-

                            [tex]K_{a}\times K_{b}=1\times 10^{-14}[/tex]

Where, [tex]K_{a}[/tex] is acid dissociation constant of acid or conjugate acid and [tex]K_{b}[/tex] is base dissociation constant of base or conjugate base

So, [tex]K_{a}(NH_{4}^{+})=\frac{1\times 10^{-14}}{1.8\times 10^{-5}}=5.6\times 10^{-10}[/tex]

As higher the [tex]K_{a}[/tex] value of an acid , higher will be the dissociation of the acid and hence more stronger will be the acid.

As [tex]K_{a}[/tex] value of [tex]NH_{4}^{+}[/tex] is higher than [tex]K_{a}[/tex] value of HCN therefore [tex]NH_{4}^{+}[/tex] is stronger acid than HCN

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