Chemistry, 03.07.2020 23:01 mariposa91
In the laboratory, a general chemistry student measured the pH of a 0.592 M aqueous solution of triethanolamine, C6H15O3N to be 10.781. Use the information she obtained to determine the Kb for this base. Kb(experiment) =
Answers: 3
![pOH=-log([OH^-])](/tpl/images/0700/9022/4105a.png)
![[OH^-]=10^{-pOH}=10^{-3.219}=6.04x10^{-4}M](/tpl/images/0700/9022/a7a1d.png)
![Kb=\frac{[OH^-][C6H14O2N^+]}{[C6H15O3N ]}](/tpl/images/0700/9022/e215d.png)
equals the concentration of hydroxyl ions that was previously, computed, therefore, we have:
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In the laboratory, a general chemistry student measured the pH of a 0.592 M aqueous solution of trie...
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