Calculate the pH of a 1.0×10^-3 M strong acid solution.

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Multiple Choice

Calculate the pH of a 1.0×10^-3 M strong acid solution.

Explanation:
For a strong acid, it completely dissociates, so the hydrogen ion concentration equals the acid concentration. The pH is defined as the negative base-10 logarithm of [H+]. With [H+] = 1.0×10^-3 M, pH = -log(1.0×10^-3) = -(-3) = 3.0. So the solution has pH 3.0. The other pH values would correspond to different [H+]: pH 2.0 would need [H+] = 0.01 M, pH 0.0 would need [H+] = 1 M, and pH 4.0 would need [H+] = 0.0001 M, none of which matches the given concentration.

For a strong acid, it completely dissociates, so the hydrogen ion concentration equals the acid concentration. The pH is defined as the negative base-10 logarithm of [H+]. With [H+] = 1.0×10^-3 M, pH = -log(1.0×10^-3) = -(-3) = 3.0. So the solution has pH 3.0.

The other pH values would correspond to different [H+]: pH 2.0 would need [H+] = 0.01 M, pH 0.0 would need [H+] = 1 M, and pH 4.0 would need [H+] = 0.0001 M, none of which matches the given concentration.

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