If [OH−] = 1.0×10−4 M, what is the pH of the solution?

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Multiple Choice

If [OH−] = 1.0×10−4 M, what is the pH of the solution?

Explanation:
Understanding how pH relates to hydroxide concentration is key here. At 25°C, pH and pOH add up to 14, so first find pOH from the given [OH−]: pOH = −log(1.0 × 10−4) = 4. Then pH = 14 − pOH = 10.0, indicating a basic solution. You can also use [H+] = Kw/[OH−] with Kw ≈ 1.0 × 10−14: [H+] = 1.0 × 10−14 / 1.0 × 10−4 = 1.0 × 10−10 M, and pH = −log(1.0 × 10−10) = 10.0.

Understanding how pH relates to hydroxide concentration is key here. At 25°C, pH and pOH add up to 14, so first find pOH from the given [OH−]: pOH = −log(1.0 × 10−4) = 4. Then pH = 14 − pOH = 10.0, indicating a basic solution.

You can also use [H+] = Kw/[OH−] with Kw ≈ 1.0 × 10−14: [H+] = 1.0 × 10−14 / 1.0 × 10−4 = 1.0 × 10−10 M, and pH = −log(1.0 × 10−10) = 10.0.

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