What is the pH of a 0.01 M NaOH solution?

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Multiple Choice

What is the pH of a 0.01 M NaOH solution?

Explanation:
A strong base like NaOH dissociates completely in water, so the hydroxide ion concentration equals the base’s concentration: [OH−] = 0.01 M. The pOH is -log10(0.01) = 2. At 25 °C, pH and pOH add to 14, so pH = 14 − 2 = 12. This shows a highly basic solution. The other pH values would require different OH− concentrations (for example, pH 13 would imply [OH−] = 0.1 M, not 0.01 M), so they don’t match a 0.01 M NaOH solution. The pH is 12.

A strong base like NaOH dissociates completely in water, so the hydroxide ion concentration equals the base’s concentration: [OH−] = 0.01 M. The pOH is -log10(0.01) = 2. At 25 °C, pH and pOH add to 14, so pH = 14 − 2 = 12. This shows a highly basic solution. The other pH values would require different OH− concentrations (for example, pH 13 would imply [OH−] = 0.1 M, not 0.01 M), so they don’t match a 0.01 M NaOH solution. The pH is 12.

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