Consider the following equilibrium reaction for hydrocyanic acid, HCN. HCNHH* +CN- At 25°C the concentrations are found to be [HCN] = 0.0160 M and [H+] = [CN-] = 2.0 x 10-6 M. What is the value of the equilibrium constant at 25°C? (Show your work.)

Consider the following equilibrium reaction for hydrocyanic acid, HCN. HCNHH* +CN- At 25°C the concentrations are found to be [HCN] = 0.0160 M and [H+] = [CN-] = 2.0 x 10-6 M. What is the value of the equilibrium constant at 25°C? (Show your work.)

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 7QRT

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Question

Consider the following equilibrium reaction for hydrocyanic acid, HCN.
HCNH+ + CN
At 25°C the concentrations are found to be [HCN] = 0.0160 M and [H+] = [CN-] = 2.0 x 10-6 M. What is the value of the
equilibrium constant at 25°C? (Show your work.)

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