What is the pH of a solution with [H+] = 1.0×10−4 M?

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Multiple Choice

What is the pH of a solution with [H+] = 1.0×10−4 M?

Explanation:
pH is defined as the negative base-10 logarithm of the hydrogen ion concentration: pH = -log10[H+]. If [H+] = 1.0×10^-4 M, then log10[H+] = log10(1.0×10^-4) = -4, so pH = -(-4) = 4.0. This value sits in the acidic range (below 7), and matches the idea that each tenfold decrease in [H+] increases pH by 1.

pH is defined as the negative base-10 logarithm of the hydrogen ion concentration: pH = -log10[H+]. If [H+] = 1.0×10^-4 M, then log10[H+] = log10(1.0×10^-4) = -4, so pH = -(-4) = 4.0. This value sits in the acidic range (below 7), and matches the idea that each tenfold decrease in [H+] increases pH by 1.

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