ChemistryLesson 2 of 3

Acids, Bases, pH & Buffer Solutions

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pH determines the acidity or basicity of an aqueous solution based on hydrogen ion activity.

pH Definition: \text{pH}=−\log₁₀[H⁺] \quad \text{and} \quad \text{pOH}=−\log₁₀[OH^-]

Water Ion Product: K_w = [H^+][OH^-] = 1.0 \times 10^{-14} \text{ at } 25^\circ\text{C} \implies \text{pH} + \text{pOH} = 14.
Strong Monoprotic Acid (e.g. HCl, HNO3): Complete dissociation \implies [H^+] = C_a.
Weak Monoprotic Acid (e.g. CH3COOH): Incomplete dissociation \implies [H^+] = \sqrt{K_a \cdot C_a}.
Buffer Solution (Henderson-Hasselbalch): \text{pH} = pK_a + \log_{10}\left(\frac{[A^-]}{[HA]}\right).

Determine if the acid/base is strong (100% ionization) or weak (equilibrium with Ka/Kb).
Calculate hydrogen ion concentration [H+].
Take the negative base-10 logarithm to find pH.

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