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To find the pH of 0.050 M diethylamine we must use the Kb of diethylamine.The Kb value of diethylamine is as follows:Kb=1.3X10^-3Kb = [(C2H5)2NH2+][OH-]/[(C2H5)2NH] as diethylamine dissolves, some will react with water forming diethylammonium ion and hydroxide, which is not accounted for in the Kb equation. Because of this, we don't know the concentration of each ion, but we do know they will be the same. We'll call them x. The diethylamine concentration will then be 0.050 - x.Kb = x^2/(0.050 - x)1.3x10^-3 = x^2/(0.050 - x)since 1.3 x 10^-3 is not much smaller compared to 0.050, x will be significant so we cannot ignore it. Rearrange the equation and use the quadratic formula to solve for x..000065 - .0013x = x^20 = x^2 + 0.013x - .000065x = [OH]pOH = -log([OH])14 - pOH = pH

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5mo ago

The pH of a solution of 0.050 M diethylamine would be around 12.3. Diethylamine is a weak base with a Kb value of 1.4 x 10^-3. This means that it will partially ionize in solution to produce hydroxide ions, resulting in a basic pH.

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Q: What is the pH of 0.050 M diethylamine?
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