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**Problem**: Consider a solution of an unknown salt having the general formula BHCl, where B is one of the weak bases in the following table. A 0.10-M solution of the unknown salt has a pH of 5.82. What is the actual formula of the salt?

###### FREE Expert Solution

###### FREE Expert Solution

Step 1

Step 2

$\overline{)\mathbf{\left[}{\mathbf{H}}_{\mathbf{3}}{\mathbf{O}}^{\mathbf{+}}\mathbf{\right]}{\mathbf{}}{\mathbf{=}}{\mathbf{}}{{\mathbf{10}}}^{\mathbf{-}\mathbf{pH}}}\phantom{\rule{0ex}{0ex}}\mathbf{\left[}{\mathbf{H}}_{\mathbf{3}}{\mathbf{O}}^{\mathbf{+}}\mathbf{\right]}\mathbf{}\mathbf{=}\mathbf{}{\mathbf{10}}^{\mathbf{-}\mathbf{5}\mathbf{.}\mathbf{82}}$

**[H _{3}O^{+}] = x = 1.5136x10^{-6} M**

Step 3

[BH^{+}] = 0.180 M - 1.5136x10^{-6} M = 0.180 M

[B] = [H_{3}O^{+}] = 1.5136x10^{-6} M

###### Problem Details

Consider a solution of an unknown salt having the general formula BHCl, where B is one of the weak bases in the following table. A 0.10-M solution of the unknown salt has a pH of 5.82. What is the actual formula of the salt?

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Our tutors have indicated that to solve this problem you will need to apply the Weak Bases concept. If you need more Weak Bases practice, you can also practice Weak Bases practice problems .

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Our expert Chemistry tutor, Rae-Anne took 9 minutes to solve this problem. You can follow their steps in the video explanation above.

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