![\rm K_{\text{b}} = \dfrac{\text{[BH}^{+}]\text{[OH}^{-}]}{\text{[B]}} = 1.8 \times 10^{-5}\\\\\dfrac{x^{2}}{0.335 - x} = 1.8 \times 10^{-5}](/tpl/images/0685/0322/975fe.png)
![\dfrac{x^{2}}{0.335} = 1.8 \times 10^{-5}\\\\x^{2} = 0.335 \times 1.8 \times 10^{-5}\\x^{2} = 6.03 \times 10^{-6}\\x = \sqrt{6.03 \times 10^{-6}}\\x = \text{[OH]}^{-} = \mathbf{2.46 \times 10^{-3}} \textbf{ mol/L}](/tpl/images/0685/0322/0aa42.png)
![\text{pOH} = -\log \text{[OH}^{-}] = -\log(2.46 \times 10^{-3}) = 2.61](/tpl/images/0685/0322/acbc3.png)
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Ammonia (NH3) is an example of a Brønsted-Lowry Base.
-Define the...
Chemistry, 13.06.2020 09:57 hmskevinjacobo5471
I NEED HELP PLEASE, THANKS!
Ammonia (NH3) is an example of a Brønsted-Lowry Base.
-Define the Brønsted-Lowry acid-base theory.
-What is the pH of an ammonia solution that has a concentration of 0.335 M? The Kb of ammonia is 1.8 × 10^–5.
Answers: 3
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