Calculate the concentration of an aqueous HBr solution that has \(\mathrm{pH}=4.25 . \mathrm{HBr}\) is a strong acid.

Short Answer

Expert verified
The concentration of the aqueous HBr solution is approximately \(5.62 \times 10^{-5} \ \text{M}\).

Step by step solution

01

Understand the relationship between pH and H+ concentration.

The pH of a solution is defined as: \[pH = -\log_{10}[H^+]\] where [H⁺] is the concentration of hydrogen ions in the solution. Since we are given the pH, we can solve for [H⁺].
02

Calculate the concentration of H⁺ ions.

To find the concentration of H⁺ ions, we rearrange the formula from step 1 and plug in the given pH value (4.25): \[[H^+] = 10^{-pH} = 10^{-4.25}\] Calculate the concentration of H⁺ ions: \[[H^+] = 10^{-4.25} \approx 5.62 \times 10^{-5} \ \text{M}\]
03

Determine the concentration of HBr.

Since HBr is a strong acid and ionizes completely, the concentration of HBr in the solution is equal to the concentration of H⁺ ions. Therefore, the concentration of the aqueous HBr solution is approximately \(5.62 \times 10^{-5} \ \text{M}\).

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