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

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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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