If `Ag^(+)+2NH_3iff[Ag(NH_3)_2]^(+)`
`K_1=1.8xx10^7`
`Ag^(+)+Cl^(-)iffAgCl`
`K_2=5.6xx10^9`
Then for `AgCl+2NH_3iff[Ag(NH_3)_2]^(+)+Cl^-`
What will be value of equilibrium constant?

If Ag + 2NH_3 iff [Ag(NH_3)_2] K_1 = 1.8 xx 10^7 Ag^+ +Cl^- iff AgCl K_2 = 5.6 xx 10^9 Then for AgCl + 2NH_3 iff [Ag(NH_3)_2]^+ + Cl^- What will be the value of equilibrium constant?

Oxidation state of Cr in [Cr(NH_3)_4Cl_2]^+

Consider the following equilibria along with the respective stability constants : Ag^(+)+NH_(3)hArr [Ag(NH_(2))]^(+),K_(1)=3.5xx10^(3) [Ag(NH_(3))]^(+)+NH_(3)hArr [Ag(NH_(3))_(2)]^(+), K_(2)=1.7xx10^(3) Calculate the overal formiation constant of [Ag(NH_(3))_(2)]^(+) .

Give the IUPAC name of the complex: [Ag(NH_3)_2]Cl .

K_b for NH_3=1.8xx10^(-5) at 25^(@) C. What is the value of K_a for NH_4^(+) ion at the same temperature ?

For the reaction, 2NH_3(g) iff N_2(g) + 3H_2(g) the units of K_p will be

The following concentrations were obtained for the formation of NH_3 from N_2 and H_2 at equilibrium at 500K. [N_2] = 1.5 xx 10^-2M. [H_2] = 3.0 xx10^-2 M and [NH_3] =1.2 xx 10^-2 M . Calculate equilibrium constant.

What is the IUPAC name of [Ni(NH_(3))_(6)]Cl_(2) ?

The stability (or formation) constant (K_(f)) for [Ag(NH_(3))_(2)]^(+) is 1.6xx10^(7) . Calculate the ratio of the concentrations of [Ag(NH_(3))_(2)]^(+) and Ag^(+) in 0.12M NH_(3) solution.