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+ + pH = log [H3O ] or log [H ] using the shorthand notation + 14 Remember that in pure water Kw = [H3O ][OH ] = 10 10 Since both the hydronium ion and hydroxide ions are formed in equal amounts, the Kw expression can be expressed as:

where j is the reaction index For a gas-phase reaction Eq (1338) takes the form:

If the equilibrium mixture is an ideal gas,

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For r independent reactions there are r separate equations of this kind, and the yi's can be eliminated by Eq (137) in favor of the r reaction coordinates E; The set of equations is then solved simultaneously for the r reaction coordinates, as illustrated in the following examples

[H3O+ ]2 = 10 10 14 Solving for [H3O+] gives us [H3O+] = 10 10 7 If you then calculate the pH of pure water: pH = log[H3O+ ] = log [1 0 10 7 ] = ( 7 00) = 7 00 The pH of pure water is 700 On the pH scale this is called neutral A solution whose [H3O+] is greater than in pure water will have a pH less than 700 and is called acidic A + solution whose [H3O ] is less than in pure water will have a pH greater than 700 and is called basic Figure 152 shows the pH scale and the pH values of some common substances

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