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Chapter sixteen - C hapter sixteen Acid-base titration and...

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Chapter sixteen Acid-base titration and ph Self-ionization of water- two water molecules produce a hydronium ion and a hydroxide ion by transfer of a proton H 2 O(l) + H 2 O(l) H 3 O + (aq) + OH - (aq) In brackets, [H 3 O + ] means “hydronium concentration in moles per liter” In brackets, [OH - ] means “hydroxide concentration in moles per liter” Neutral- hydronium ion and hydroxide ion concentrations are equal Acidic- concentration in which [H 3 O + ] > [OH - ] Basic- concentration in which [OH - ] > [H 3 O + ] pH- the negative of the common logarithm of the hydronium ion concentration pH = -log [H 3 O + ] a neutral solution at 25°C has a [H 3 O + ] of 1x10 -7 M and has a pH of 7 pOH- negative of the common logarithm of the hydroxide ion concentration pOH = -log [OH - ] a neutral solution at 25°C has a [OH - ] of 1x10 -7 M and has a pOH of 7 at 25°C, pH + pOH = 14 if either the [H 3 O + ] or the pH of a solution is known, the other can be calculated the number to the LEFT of the decimal determines significant figures
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