What is the concentration of `Ag^(+) ion` in a `1 L` solution containing `0.02 mol` of `AgNO_(3)` and `0.14 mol` of `NH_(3)` ? For `[Ag(NH_(3))_(2)]^(+), K_(I nstab)=10^(8)`

What will be the Ag^(+) ion concentration in a solution of 0.2 M solution of [Ag(NH_(3))_(2)^(+)] ? Ag (NH_(3))_(2)^(+) hArr Ag^(+) +2NH_(3) , " " K_("dis")= 6.8 xx10^(-8)

What will be the Ag^(+) ion concentration in a solution of 0.2 M solution of [Ag(NH_(3))_(2)^(+)] ? Ag (NH_(3))_(2)^(+) hArr Ag^(+) +2NH_(3) , " " K_("dis")= 6.8 xx10^(-8)

a. Calculate [Ag^(o+)] in a solution of [Ag^(o+)] in a solution of [Ag(NH_(3))_(2)^(o+)] prepared by adding 1.0 xx 10^(-3)mol AgNO_(3) to 1.0L of 1.0M NH_(3) solution K_(f) Ag(NH_(3))_(2)^(o+) = 10^(8) . b. Calculate [Ag^(o+)] which is in equilibrium with 0.15M [Ag(NH_(3))_(2)]^(o+) and 1.5 NH_(3) .

Calculate the concentration of free silver ion [Ag^(+) ] in an aqueous solution that is prepared as 0.1 M AgNO_3 and 3.0 M NH_3 ,Ag^(+) (aq) +2 NH_3 (aq) hArr [Ag(NH_3) _2]^(+) (aq) K_(f) = 1.6 xx 10^(7) . If answer is x xx 10^(-10) M then x= ______?

What is [NH_(4)^(+)] in a solution that contain 0.02 M NH_(3)(K_(b)=1.8xx10^(-5)) and 0.01 M KOH?

What is [NH_(4)^(+)] in a solution that contain 0.02 M NH_(3)(K_(b)=1.8xx10^(-5)) and 0.01 M KOH?

What is [NH_(4)^(+)] in a solution that contain 0.02 M NH_(3)(K_(b)=1.8xx10^(-5)) and 0.01 M KOH?