Calculate the value of the equilibrium constant, K., for the reactionAgBr(s) + 2 NH, (aq) =[Ag(NH;),]* (aq) + Br (aq)K. = ?The solubility product constant, Kgp, for AgBr is 5.35 x 10-13, and the formation constant, K¢ (B2), for [Ag(NH,),I* is1.6 x 107.K. =

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Calculate the value of the equilibrium constant, K., for the reaction AgBr(s) + 2 NH, (aq) = [Ag(NH,),1* (aq) + Br¯(aq) K. = ? The solubility product constant, K,p, for AgBr is 5.35 x 10-13, and the formation constant, K, (B2), for [Ag(NH,),J* is 1.6 x 107. K.

Calculate the value of the equilibrium constant, K., for the reaction AgBr(s) + 2 NH, (aq) = [Ag(NH,),1* (aq) + Br¯(aq) K. = ? The solubility product constant, K,p, for AgBr is 5.35 x 10-13, and the formation constant, K, (B2), for [Ag(NH,),J* is 1.6 x 107. K.

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 80AP

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Question

Calculate the value of the equilibrium constant, K., for the reaction
AgBr(s) + 2 NH, (aq) =[Ag(NH;),]* (aq) + Br (aq)
K. = ?
The solubility product constant, Kgp, for AgBr is 5.35 x 10-13, and the formation constant, K¢ (B2), for [Ag(NH,),I* is
1.6 x 107.
K. =

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