An aqueous solution of HBrO 4 has a pH of 4.34. Find the molar concentration of HBrO 4 solution.

An aqueous solution of perbromic acid has a pH of 4.34. Find the molar concentration of perbromic acid. So, the key to this question is to realize that since this is a strong acid that the concentration of H+ion is equal to the molarity of your strong acid. So what we need to do here is we need to determine what our H+ion concentration will be. We can do that since we know the pH. You're going to say here that H+ion concentration is equal to 10 to the negative pH. So it's equal to 10 to the negative 4.34. When we punch this into our calculator we're going to get back 4.6 times 10 to the negative 5 molar. This would represent the molar concentration of our perbromic acid solution.

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17. Acid and Base Equilibrium

pH of Strong Acids and Bases

General Chemistry

17. Acid and Base Equilibrium

pH of Strong Acids and Bases

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Multiple Choice

An aqueous solution of HBrO₄ has a pH of 4.34. Find the molar concentration of HBrO₄ solution.

4.6 × 10⁻¹⁹ M

2.6 × 10⁻⁶ M

2.2 × 10⁻¹⁰ M

4.6 × 10⁻⁵ M

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Verified step by step guidance

Understand that the pH of a solution is related to the concentration of hydrogen ions (H⁺) in the solution. The pH is defined as the negative logarithm (base 10) of the hydrogen ion concentration: \( \text{pH} = -\log[\text{H}^+] \).

Given the pH of the solution is 4.34, use the pH formula to find the concentration of hydrogen ions: \( [\text{H}^+] = 10^{-\text{pH}} \). Substitute the given pH value into the equation: \( [\text{H}^+] = 10^{-4.34} \).

Calculate the hydrogen ion concentration using the expression from the previous step. This will give you the molarity of H⁺ ions in the solution.

Recognize that for a strong acid like HBrO4, which dissociates completely in water, the concentration of H⁺ ions is equal to the initial concentration of the acid. Therefore, the molarity of HBrO4 is the same as the calculated [H⁺].

Compare the calculated molarity of HBrO4 with the given options to identify the correct answer. The correct molarity should match one of the provided choices.