What is the pH of a 0.025 M NaOH solution?

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Multiple Choice

What is the pH of a 0.025 M NaOH solution?

Explanation:
Strong bases dissociate completely in water, so the hydroxide concentration directly comes from the base’s molarity. For 0.025 M NaOH, [OH-] = 0.025 M. Compute pOH = -log10(0.025) ≈ 1.60, then pH = 14 - pOH ≈ 12.40 at 25°C. So the solution is highly basic with a pH about 12.40. To see why the other values don’t fit: a pH of 13.00 would require a much higher [OH-] (around 0.1 M). A pH of 11.80 corresponds to a smaller [OH-] (about 0.0063 M), and a pH of 12.00 corresponds to [OH-] ≈ 0.01 M. The given concentration yields pH ≈ 12.40.

Strong bases dissociate completely in water, so the hydroxide concentration directly comes from the base’s molarity. For 0.025 M NaOH, [OH-] = 0.025 M. Compute pOH = -log10(0.025) ≈ 1.60, then pH = 14 - pOH ≈ 12.40 at 25°C. So the solution is highly basic with a pH about 12.40.

To see why the other values don’t fit: a pH of 13.00 would require a much higher [OH-] (around 0.1 M). A pH of 11.80 corresponds to a smaller [OH-] (about 0.0063 M), and a pH of 12.00 corresponds to [OH-] ≈ 0.01 M. The given concentration yields pH ≈ 12.40.

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