Chemistry, 06.12.2020 19:00, alanflores40
The pH of a 0.15 M butylamine, C&H3NH2 solution is 12.0 at 25°C. Calculate the dissociation constant of the base.
Answers: 1
![\rm Kb=\dfrac{[L][OH^-]}{[LOH]}](/tpl/images/0954/6725/84d1f.png)
![\tt [OH^-]=\sqrt{Kb.M}](/tpl/images/0954/6725/ab388.png)
![\tt [OH^-]=10^{-pOH}\\\\(OH^-]=10^{-2}](/tpl/images/0954/6725/b2b50.png)
![\tt Kb=\dfrac{x^2}{0.15-x}\rightarrow x=[OH^-]\\\\Kb=\dfrac{10^{-4}}{0.15-10^{-2}}=7.14\times 10^{-4}](/tpl/images/0954/6725/69346.png)
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The pH of a 0.15 M butylamine, C&H3NH2 solution is 12.0 at 25°C. Calculate the dissociation
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