concentration NH3 solution one liter 0.10 mol AgCl

concentration NH3 solution one liter 0.10 mol AgCl

난용성염 AgCl과 착이온 [Ag(NH3)2]^+

 

 

1 L당 0.10 mol AgCl을 용해시킬 수 있는 NH3 용액의 농도는?

 

 

The concentration of NH3 solution

whose one litre can dissolve 0.10 mole AgCl is:

 

Ksp of AgCl = 1.0×10^(-10)

Kf of [Ag(NH3)2]^+ = 1.6×10^7

 

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AgCl(s) ⇌ Ag^+(aq) + Cl^-(aq)

Ksp = [Ag^+] [Cl^-]

 

 

 

Ag^+(aq) + 2NH3(aq) ⇌ [Ag(NH3)2]^+(aq)

Kf = [[Ag(NH3)2]^+] / [Ag^+] [NH3]^2

 

 

 

Ksp × Kf

= ([Ag^+] [Cl^-]) × ([[Ag(NH3)2]^+] / [Ag^+] [NH3]^2)

= [[Ag(NH3)2]^+] [Cl^-] / [NH3]^2

( 참고 https://ywpop.tistory.com/4154 )

 

 

 

 

AgCl(s) + 2NH3(aq) ⇌ [Ag(NH3)2]^+(aq) + Cl^-(aq)

K = [[Ag(NH3)2]^+] [Cl^-] / [NH3]^2

= Ksp × Kf

= (1.0×10^(-10)) × (1.6×10^7)

= 0.0016

 

 

 

AgCl(s) 중 용해된 AgCl(aq)가

[AgCl] = 0.10 mol / 1 L = 0.10 M 이므로,

[[Ag(NH3)2]^+] = [Cl^-] = 0.10 M

 

 

 

[NH3] = [(0.10) (0.10) / (0.0016)]^(1/2) = 2.5 M

 

 

 

답: [NH3] = 2.5 M

 

 

 

 

[키워드] 난용성염 AgCl과 착이온 [Ag(NH3)2]^+ 기준문서, AgCl과 [Ag(NH3)2]^+ 기준문서, 난용성염과 착이온 기준문서