The aqueous silver ion [Ag"] and ammonia [NH3] form the complex ion [Ag(NH,)2] Determine the molar solubility of AgBr in 2.45 M NH3. The Kfvalue for [Ag(NH3)2] is Ke = 1.7x 10. The K, value for [AgBr] is K, = 5.0x 10 Type your answer in the space below using scientific notation. (example: 0.012 = 1.2 10^-2).
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![The aqueous silver ion \([Ag^+]\) and ammonia \([NH_3]\) form the complex ion \([Ag(NH_3)_2^+]\).
Determine the **molar solubility** of AgBr in 2.45 M \(NH_3\).
The \(K_f\) value for \([Ag(NH_3)_2^+]\) is \(K_f = 1.7 \times 10^7\).
The \(K_{sp}\) value for \([AgBr]\) is \(K_{sp} = 5.0 \times 10^{-13}\).
Type your answer in the space below using **scientific notation**.
(example: 0.012 = 1.2*10^-2).](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F40daf55f-9b36-4034-9111-c8b1fc526fc5%2F48886652-50b7-43f8-9856-4d5d66aeef8c%2Flf9j6cr_processed.jpeg&w=3840&q=75)
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