Question

$A{g}^{+}+N{H}_3\rightleftharpoons \left[Ag\right(N{H}_3{)}^{+}];k_1=3.5\times {10}^{-3}$

$\left[Ag\right(N{H}_3){]}^{+}+N{H}_3\rightleftharpoons [Ag(N{H}_3{)}_2{]}^{+};k_2=1.7\times {10}^{-3}$

Then the formation constant of $\left[Ag\right(N{H}_3{)}_2{]}^{+}$ is:

• A. $5.95\times {10}^{-6}$
• B. $6.08\times {10}^6$
• C. $6.08\times {10}^{-6}$
• D. none of the above

Answer 1

The correct option is A $5.95\times {10}^{-6}$

$A{g}^{+}+N{H}_3\rightleftharpoons \left[Ag\right(N{H}_3{)}^{+}];k_1=3.5\times {10}^{-3}$

$\left[Ag\right(N{H}_3){]}^{+}+N{H}_3\rightleftharpoons [Ag(N{H}_3{)}_2{]}^{+};k_2=1.7\times {10}^{-3}$

Then the formation constant of $\left[Ag\right(N{H}_3{)}_2{]}^{+}$ is:

$k=k_1\times k_2=3.5\times {10}^{-3}\times 1.7\times {10}^{-3}=5.95\times {10}^{-6}$

Hence, the correct option is $\text{A}$