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Chemistry Question on Equilibrium

Ag+ +NH3⇌[Ag(NH3)]+;K1=3.5×10−3Ag^+ \, + NH_3 \rightleftharpoons [ Ag ( NH_3 ) ]^+ ; K_1 = 3.5 \times 10^{ - 3 } [Ag(NH3)]+ +NH3⇌[Ag(NH3)2]+;K2=1.7×10−3[ Ag ( NH_3 )]^+ \, + NH_3 \rightleftharpoons [ Ag (NH_3 )_2 ]^+ ; K_2 = 1.7 \times 10^{ - 3 } then the formation constant of [Ag(NH3)2]+[ Ag (NH_3)_2]^+ is...

A

6.08×10−66.08 \times 10^{ - 6 }

B

6.08×1066.08 \times 10^6

C

6.08×10−96.08 \times 10^{ - 9 }

D

5.95×10−65.95 \times 10^{ - 6 }

Answer

5.95×10−65.95 \times 10^{ - 6 }

Explanation

Solution

Ag+NH3⇌[Ag(NH3)+]Ag^+ NH_3 \rightleftharpoons [ Ag (NH_3)^+ ] \hspace20mm K1=3.5×10−3K_1 = 3.5 \times 10^{ - 3 }
[Ag(NH3)+]+NH3⇌[Ag(NH3)2+] K2=1.7×10−3Adding:Ag+ +2NH3⇌[Ag(NH3)2+]\frac{ [ Ag ( NH_3 )^+ ] + NH_3 \rightleftharpoons [ Ag ( NH_3 )_2^+ ] \, K_2 = 1.7 \times 10^{ - 3 }}{ Adding : Ag^+ \, + 2NH_3 \rightleftharpoons [ Ag ( NH_3)_2^+ ] }
K=K1×K2=5.95×10−6K = K_1 \times K_2 = 5.95 \times 10^{ - 6 }