What is the pH of a solution containing [H+] = 1.0e-3 M (a strong acid)?

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Multiple Choice

What is the pH of a solution containing [H+] = 1.0e-3 M (a strong acid)?

Explanation:
pH is the negative base-10 logarithm of the hydrogen ion concentration: pH = -log[H+]. For a strong acid, the acid fully dissociates, so [H+] equals the acid concentration. With [H+] = 1.0×10^-3 M, pH = -log10(1.0×10^-3) = -(-3) = 3. This places the solution in the acidic range (pH < 7). The log nature of pH means a tenfold change in [H+] changes pH by one unit; for example, [H+] = 1×10^-4 M gives pH 4, and [H+] = 1×10^-2 M gives pH 2. The other options correspond to different hydrogen ion levels: pH 9 would require [H+] = 1×10^-9 M, and pH 0 would require [H+] = 1 M.

pH is the negative base-10 logarithm of the hydrogen ion concentration: pH = -log[H+]. For a strong acid, the acid fully dissociates, so [H+] equals the acid concentration. With [H+] = 1.0×10^-3 M, pH = -log10(1.0×10^-3) = -(-3) = 3. This places the solution in the acidic range (pH < 7). The log nature of pH means a tenfold change in [H+] changes pH by one unit; for example, [H+] = 1×10^-4 M gives pH 4, and [H+] = 1×10^-2 M gives pH 2. The other options correspond to different hydrogen ion levels: pH 9 would require [H+] = 1×10^-9 M, and pH 0 would require [H+] = 1 M.

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