Chemistry, 14.07.2020 02:01 hubbabubba0715
Calculate the pH of a 0.0255 M solution of ammonium bromide (NH4Br). The Kb of ammonia is 1.76 x 10-5
Answers: 3
![[H_3O^{+} ]= \sqrt{K_a \times C_a } = \sqrt{5.68 \times 10^{-10} \times 0.0255 } = 3.81 \times 10^{-6}M](/tpl/images/0705/0989/d386c.png)
![pH = -log [H_3O^{+} ] = -log (3.81 \times 10^{-6}) = 5.42](/tpl/images/0705/0989/96bbf.png)
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Calculate the pH of a 0.0255 M solution of ammonium bromide (NH4Br). The Kb of ammonia is 1.76 x 10-...
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