**Question:**Determine the pH of a 0.461 M C₆H₅CO₂H solution if the Kₐ of C₆H₅CO₂H is 6.5 × 10⁻⁵.**Options:**- ○ 4.52- ○ 11.74- ○ 9.48- ○ 2.26- ○ 5.48*Explanation:*To solve for the pH of the solution, use the formula for calculating pH from the equilibrium constant (Kₐ) and the concentration of the acid (C₆H₅CO₂H).1. Write the ionization equilibrium expression for the acid: \[ \text{C₆H₅CO₂H} \rightleftharpoons \text{C₆H₅CO₂⁻} + \text{H⁺} \]2. Set up the expression for the acid dissociation constant ($Kₐ$): \[ Kₐ = \frac{[\text{C₆H₅CO₂⁻}][\text{H⁺}]}{[\text{C₆H₅CO₂H}]} \]3. Assume $x$ is the amount dissociated at equilibrium, then: \[ Kₐ = \frac{x \cdot x}{0.461 - x} \approx \frac{x^2}{0.461} \]4. Solve for $x$ using the given $Kₐ$: \[ x^2 = 6.5 \times 10^{-5} \cdot 0.461 \] \[ x = \sqrt{(6.5 \times 10^{-5}) \cdot 0.461} \]5. Calculate the pH: \[ \text{pH} = -\log[\text{H⁺}] = -\log(x) \]

pH is commonly known power of hydrogen, it measures the concentration of hydrogen ion in the…

Answered: Determine the pH of a 0.461 M C3H5CO,H…

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Chemistry

Determine the pH of a 0.461 M C3H5CO,H M solution if the K, of C6H5CO2H is 6.5 x 105. 4.52 11.74 9.48 2.26 5.48

Chemistry

10th Edition

ISBN:9781305957404

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

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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