I don’t understand how to do this question **Title: Calculating the pH of an Aqueous Solution of Benzoic Acid****Instruction:**Use the references to access important values if needed for this question.**Problem Statement:**Calculate the pH of a 0.528 M aqueous solution of benzoic acid (C₆H₅COOH). The acid dissociation constant (Kₐ) for benzoic acid is given as 6.3 x 10⁻⁵.**Formula to Calculate pH:**The formula to determine the pH of an acidic solution is:\[ \text{pH} = -\log[\text{H}^+] \]Where \([\text{H}^+]\) is the concentration of hydrogen ions in the solution.**Task:**Determine the concentration of hydrogen ions \([\text{H}^+]\) using the provided concentration of the acid and the acid dissociation constant, and then calculate the pH using the above formula.**Additional Notes:**- Use the quadratic formula if needed to solve for hydrogen ion concentration.- For weak acids like benzoic acid, assume that \([\text{H}^+]\) is much smaller than the initial concentration of the acid. **Answer Box:**pH = [Enter your answer here]

concentration of Benzoic acid (C6H5COOH) = 0.528 M Ka of Benzoic acid = 6.3 x 10−5

Answered: Calculate the pH of a 0.528 M aqueous…

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Calculate the pH of a 0.528 M aqueous solution of benzoic acid (C,H3COOH, K, = 6.3x10). %3D pH =

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ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

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Question

I don’t understand how to do this question

**Title: Calculating the pH of an Aqueous Solution of Benzoic Acid**

**Instruction:**

Use the references to access important values if needed for this question.

**Problem Statement:**

Calculate the pH of a 0.528 M aqueous solution of benzoic acid (C₆H₅COOH). The acid dissociation constant (Kₐ) for benzoic acid is given as 6.3 x 10⁻⁵.

**Formula to Calculate pH:**

The formula to determine the pH of an acidic solution is:

\[ \text{pH} = -\log[\text{H}^+] \]

Where \([\text{H}^+]\) is the concentration of hydrogen ions in the solution.

**Task:**

Determine the concentration of hydrogen ions \([\text{H}^+]\) using the provided concentration of the acid and the acid dissociation constant, and then calculate the pH using the above formula.

**Additional Notes:**

- Use the quadratic formula if needed to solve for hydrogen ion concentration.
- For weak acids like benzoic acid, assume that \([\text{H}^+]\) is much smaller than the initial concentration of the acid.

**Answer Box:**

pH = [Enter your answer here]

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