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How much AgBr would dissolve in 1 litre ...

How much AgBr would dissolve in 1 litre of 0.40 M` NH_3 ? K_(sp) (AgBr) = 5 xx 10^(-13), K_d [Ag(NH_3)_2^+] = 1 xx 10^(-8)`

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`2.83 xx 10^(-3) M`
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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) .

Calculated the minimum amount of Nh_(3) which must be added to 1.0L of solution in order to dissolve 0.1mol AgC1 by forming [Ag(NH_(3))_(2)]^(o+)? K_(sp) of AgC1 = 1 xx 10^(-10), K_(f) (NH_(3))_(2)^(o+) = 1 xx 10^(8) .

What is the molar solubility of AgCl(s) in 0.1 M NH_(3)(aq)?K_(sp)(AgCl)=1.8xx10^(-10), K_(f)[Ag(NH_(3))_(2)]^(+)=1.6xx10^(7).

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) .

What is the solubility of AgCl in 0.20 M NH_3 ? Given : K_(sp)(AgCl) = 1.7 xx 10^(-10) M^(2), K_(1)=[Ag(NH_(3))^(+)]//[Ag^(+)] [NH_(3)]=2.33 xx 10^(3) M^(-1) and K_(2)=[Ag(NH_(3))_(2)^(+)]//[Ag (NH_(3))^(+) [NH_(3)]=7.14 xx 10^(3) M^(-1)

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