Please answer very soon Calculate the [NH3] in a solution of 0.350M ammoniumcyanide (NH,CN). Hint: Use the Ka of HCN (4.9 × 10¬10)and the Kb of NH3 (1.8 × 10-5) to calculate Kc for thereactionNH,*(aq) + CN¯(aq)= NH3(aq) + HCN(aq).

Equilibrium constant is defined as ratio of concentration of reactant to the Concentration of…

Calculate the [NH3] in a solution of 0.350M ammonium cyanide (NH,CN). Hint: Use the Ka of HCN (4.9 × 10¬1º) and the Kb of NH3 (1.8 × 10-5) to calculate Kc for the reaction NH,*(aq) + CN¯(aq)= NH3(aq) + HCN(aq).

Calculate the [NH3] in a solution of 0.350M ammonium cyanide (NH,CN). Hint: Use the Ka of HCN (4.9 × 10¬1º) and the Kb of NH3 (1.8 × 10-5) to calculate Kc for the reaction NH,*(aq) + CN¯(aq)= NH3(aq) + HCN(aq).

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

Chapter15: Acid–base Equilibria

Section: Chapter Questions

Problem 55P

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Please answer very soon

Calculate the [NH3] in a solution of 0.350M ammonium
cyanide (NH,CN). Hint: Use the Ka of HCN (4.9 × 10¬10)
and the Kb of NH3 (1.8 × 10-5) to calculate Kc for the
reaction
NH,*(aq) + CN¯(aq)= NH3(aq) + HCN(aq).

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