[xshadow]

Hi!!
I don't know how  to calculate pH of a solution :

10^-2M AgNO₃
10^-1M NH₃

...because i have to   consider  also this reaction:
Ag⁺ + NH3  >>> Ag(NH₃)⁺    with β₁ = K₁

Usually in order to calculate pH (without AgNO₃) i have to write the charge (or protonic) balance...
In the balance charge i substitute the equlibrium concentration [ i ] with  α_i*C_NH3 for all the species involved in C.B (where C_NH3 is the initial concentration of ammonia)

For example for a solution of (ONLY) NH3 (considered  the  correspondng acid reaction = K_a  ) i have:

α_NH4+≡α₀= [H⁺]/ k_a +[H⁺]
α_NH3 ≡ α₁ =  k_a/ k_a+[H⁺]

1)Now my QUESTION is:
IF i have also AgNO3 ( = NH3 can complex Ag⁺) the α_i in the  charge balance are the same or they are changed??

2) And now in the charge balance C_NH3 is always equal to   C_NH3= [NH₄+ [NH₃] or is C_NH3= [NH₄+ [NH₃] + [AgNH3⁺]

Please help me !!
Thanks

[AWK]

1. Calculate stoichiometry of full complex formation reaction
2. For the rest of ammonia calculate pH.

An excess of ammonia will reduce concentration of Ag(NH₃)⁺ to a neglegible value.

[xshadow]

1. Calculate stoichiometry of full complex formation reaction
2. For the rest of ammonia calculate pH.

An excess of ammonia will reduce concentration of Ag(NH₃)⁺ to a neglegible value.

Understand!!

So I calculate all the complex species (the  concentration []) using the complexiometric equilibrium  formula,then  I can find the exact value of NH3 "free" ....on this NH3 free I calculate the pH

Thanksss