Final answer:
To find the concentration of OH- in a solution of ethylamine, we can use the equation for Kb, which is the equilibrium constant for the reaction of ethylamine with water. Given the concentration of ethylamine and the value of Kb, you can calculate the hydroxide ion concentration using the equation [OH-] = (Kb x [C2H5NH2]) / [C2H5NH3+]. In this case, the concentration of OH- in the ethylamine solution is zero.
Step-by-step explanation:
To find the hydroxide ion concentration in a solution of ethylamine, we can use the equation for Kb, which is the equilibrium constant for the reaction of ethylamine with water:
Kb = [OH-][C2H5NH2] / [C2H5NH3+]
We are given the concentration of ethylamine (0.380 M) and the value of Kb (5.6x10^-4). Since [C2H5NH3+] is negligible compared to [C2H5NH2], we can assume that [C2H5NH3+] is equal to zero.
Using this information, we can rearrange the equation to solve for [OH-]:
[OH-] = (Kb x [C2H5NH2]) / [C2H5NH3+]
Substituting the given values, we get:
[OH-] = (5.6x10^-4 x 0.380) / 0
However, we cannot divide by zero, so we conclude that the concentration of OH- in the ethylamine solution is zero.