AgCl(s), silver chloride, has a very low solubility: AgCl(s) ⇌ Ag +(aq) + Cl−(aq), Ksp = 1.6 × 10–10 . Adding ammonia significantly increases the solubility of AgCl because a complex ion is formed: Ag +(aq) + 2NH3 (aq) ⇌ Ag(NH3 )2 + (aq), Kf = 1.7 × 107 . What mass of NH3 is required to prepare 1.00 L of solution that will dissolve 2.00 g of AgCl by formation of Ag(NH3 )2 +?
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AgCl(s), silver chloride, has a very low solubility: AgCl(s) ⇌ Ag
+(aq) + Cl−(aq), Ksp = 1.6 × 10–10
.
Adding ammonia significantly increases the solubility of AgCl because a complex ion is formed:
Ag
+(aq) + 2NH3
(aq) ⇌ Ag(NH3
)2
+
(aq), Kf = 1.7 × 107
. What mass of NH3
is required to prepare 1.00
L of solution that will dissolve 2.00 g of AgCl by formation of Ag(NH3
)2
+?
The answer is supposedly 4.81, but I am not getting that. When I do a quadratic I get 0.0015, and that multipled by the molar mass of NH3 = 0.026, not 4.81. Where am I going wrong? May this equation be explained in great detail?
Thank you
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