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Chapter 1: QCYL (page 9)

We can 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 脳 10鈭�10. The ionization constant of NH4+ is not listed, but the ionization constant of its conjugate base, NH3, is listed as 1.8 脳 10鈭�5. Determine the ionization constant of NH4+, and decide which is the stronger acid, HCN or NH4+.

Short Answer

Expert verified

An acid dissociation constant can be explained as numerical measure of strength of acids in the solution. It is given by formulae.

\(\begin{aligned}{}HA \rightleftharpoons \;\;\;\;H\; + \;{A^ - }\\Ka\; = \;\frac{{\left[ {{A^ - }} \right]\;\left[ {{H^ + }} \right]\;}}{{\left[ {HA} \right]}}\end{aligned}\)

Step by step solution

01

calculating Ka

Ka value of ammonia is calculated as follows

\(\begin{array}{l}{K_a} of HCN = 4.9 \times 1{0^{ - 10}}\;\\{K_b}(N{H_3}) = 1.8 \times 1{0^{ - 5}}\\{K_a}(N{H_4}^ + ) = 5.6 \times 1{0^{ - 10}}\end{array}\)

As Ka of \(N{H_4}^ + \) is greater than \(HCN\). hence \(N{H_4}^ + \) is strong acid

02

Final answer

NH4+ is strong acid

Thus, ammonium ion is considered as strong acid

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