Calculate how much `AgBR` could dissolves in `1.0L of 0.4M NH_(3). K_(f) Ag(NH_(3))_(2)^(o+) = 1.0 xx 10^(8)`.

How much AgBr could dissolve in 1.0L of 0.4M NH_(3) ? Assume that Ag(NH_(3))_(2)^(o+) is the only complex formed. Given: the dissociation constant for Ag(NH_(3))_(2)^(o+) hArr Ag^(o+) xx 2NH_(3) , K_(d) = 6.0 xx 10^(-8) and K_(sp)(AgBr) =5.0 xx 10^(-13) .

How much AgBr could dissolve in 1.0L of 0.4M NH_(3) ? Assume that Ag(NH_(3))_(2)^(o+) is the only complex formed. Given: the dissociation constant for Ag(NH_(3))_(2)^(o+) hArr Ag^(o+) + 2NH_(3) , K_(d) = 6.0 xx 10^(-8) and K_(sp)(AgBr) =5.0 xx 10^(-13) .

Determine the concentration of NH_(3) solution whose one litre can dissolve 0.10 mole AgCI. K_(SP) of AgCI and K_(f) of Ag(NH_(3))_(2)^(+) are 1.0xx10^(-10)M^(2) and 1.6xx10^(7)M^(-2) respectively.

Determine the concentration of NH_(3) solution whose one litre can dissolve 0.10 mole AgCl. K_(sp) of AgCl and K_(f) of Ag(NH_(3))_(2)^(+) are 1.0xx10^(-10)M^(2) and 1.6xx10^(7)M^(-2) respectively.

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) .

a. Calculate [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) .

How many moles of NH_(3) must be added to 1.0L of 0.75M AgNO_(3) in order to reduce the [Ag^(o+)] to 5.0 xx 10^(-8)M. K_(f) Ag (NH_(3))_(2)^(o+) = 1 xx 10^(8) .

How many moles of NH_(3) must be added to 1.0L of 0.75M AgNO_(3) in order to reduce the [Ag^(o+)] to 5.0 xx 10^(-8)M. K_(f) Ag (NH_(3))_(2)^(o+) = 1 xx 10^(8) .