pH & Acid-Base Equilibria

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Flashcards for pH & Acid-Base Equilibria equations.

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10 Terms

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pH of strong acids

pH = − log10[H+]

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Hydrogen ion concentration from pH

[H+] = 10¬pH

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pOH

pOH = — log10[OH-]

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Relationship between pH and pOH

pH+ pOH = 14 (at 25C)

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Kw - Ionic product of water

K₂ = [H+][OH¯] = 1.0 × 10−14 mol²dm−6

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pKw

pKw = — log10 K = 14 (at 25C)

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Ka - Acid dissociation constant

Ka = [H+][A¯] / [HA]

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pKa

pKa = − log10 Ka or Ka = 10-pka

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pH of weak acids (simplified)

pH = − log10 (√√K[HA])

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pH of buffer solutions

pH = pKa + log10 ([A-]/[HA])