What is the hydrogen ion concentration of an acetate buffer having a pH of 4.24?

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Study for the Bishop Clinical Chemistry Test. Engage with flashcards and multiple choice questions with hints and explanations to prepare thoroughly for your exam!

Multiple Choice

What is the hydrogen ion concentration of an acetate buffer having a pH of 4.24?

Explanation:
pH is the negative logarithm of the hydrogen ion concentration: pH = -log10[H+]. So [H+] = 10^(-pH). For pH 4.24, [H+] = 10^(-4.24) = 10^(-4) × 10^(-0.24) ≈ 1.0×10^-4 × 0.575 ≈ 5.75×10^-5 M. That matches the option 5.75 × 10^-5. The other values correspond to far different pH levels (much more acidic or basic), so they don’t fit a pH of 4.24.

pH is the negative logarithm of the hydrogen ion concentration: pH = -log10[H+]. So [H+] = 10^(-pH). For pH 4.24, [H+] = 10^(-4.24) = 10^(-4) × 10^(-0.24) ≈ 1.0×10^-4 × 0.575 ≈ 5.75×10^-5 M. That matches the option 5.75 × 10^-5. The other values correspond to far different pH levels (much more acidic or basic), so they don’t fit a pH of 4.24.

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