Answer:
The pH of this solution is 3.4.
Explanation:
Consider the definition of the pH of a solution:
[tex]\displaystyle \rm pH = \log{\frac{1}{[H_{3}O^{+}]}} = - \log{[H_3O}^{+}]}[/tex],
where
- [tex]\rm [H_3O}^{+}][/tex] is the hydronium ion concentration of the solution in moles per liter. Note that some textbooks write [tex]\rm [H_3O}^{+}][/tex] as [tex]\rm H^{+}[/tex].
The unit "M" here is the same as moles per liter.
On a scientific calculator, evaluate
[tex]\rm -\log{(3.8\times 10^{-4})}[/tex]
to find the pH of this solution.
[tex]\rm pH = -\log{(3.8\times 10^{-4})} \approx 3.4[/tex].
The pH of this solution is approximately 3.4.
