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<Mastering Ch. 17 Module V + pH of a Strong Acid and a Strong Base pH is a logarithmic scale used to indicate the hydrogen ion concentration, H+), of a solution: pH = -log[H+] Due to the autoionization of water, in any aqueous solution, the hydrogen ion concentration and the hydroxide ion concentration, [OH-], are related to each other by the K of water: K[H][OH-] = 1.00 x 10-4 where 1.00 x 10-14 is the value at approximately 297 K. Based on this relation, the pH and pOH are also related to each other as 14.00 = pH +POH
+ pH of a Strong Acid and a Strong Base # pH is a logarithmic scale used to indicate the hydrogen ion concentration, H), of a solution: -log[H+] pH = - Due to the autolonization of water, in any aqueous solution, the hydrogen ion concentration and the hydroxide ion concentration. [OH-], are related to each other by the K, of water: K=[H][OH-] = 1.00 x 10-¹ where 1.00 x 10-14 is the value at approximately 297 K. Based on this relation, the pH and pOH are also related to each other as 14.00 pH+pOH
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