a) Calculate the concentration of Zn+2 in a 0.01 M solution of Zn(NO3)2 and containing an added NH3 concentration of 3.2x10-2 M. We have the complex ion formation constants of: Zn(NH3) k1 = 151, Zn(NH3)2*2 ; k2 = 178, +2 %3D %3D

Appl Of Ms Excel In Analytical Chemistry
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Chapter9: Complexometric And Precipitation Titrations
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a) Calculate the concentration of Zn+2 in a
0.01 M solution of Zn(NO3)2 and containing
an added NH3 concentration of 3.2x102 M.
We have the complex ion formation constants
of: Zn(NH3)+2 kl = 151, Zn(NH3)2+2; k2 = 178,
Zn(NH3)3*2; k3 = 204, Zn(NH3)4+2 ; k4 = 91.2
+2.
b) If 1.2 x 10-10 M of Sulfide ions (S<) are
added to the previous solution, will the ZnS
precipitate? (for SnS Kps = 1 x 10-24)
Transcribed Image Text:a) Calculate the concentration of Zn+2 in a 0.01 M solution of Zn(NO3)2 and containing an added NH3 concentration of 3.2x102 M. We have the complex ion formation constants of: Zn(NH3)+2 kl = 151, Zn(NH3)2+2; k2 = 178, Zn(NH3)3*2; k3 = 204, Zn(NH3)4+2 ; k4 = 91.2 +2. b) If 1.2 x 10-10 M of Sulfide ions (S<) are added to the previous solution, will the ZnS precipitate? (for SnS Kps = 1 x 10-24)
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