comparison and contrast on arrhenius, bronsted-lowry, and lewis concepts of acids-bases
...nd [OH-] is equal to the Kw (Ion product constant for water). The Kw is equal to 1x10-4 at 25°C. As acid or base is added to the water, this relationship will still hold true. When the concentrations of the hydrogren or hydroxide ion concentrations are know, they can be used to determine the ph of the acid or base being tested. The ph is equal to –log of the hydronium ion concentration. The poh for that matter is equal to –log of the hydroxide ion concentration. When either is known, the sum of both must equal 14. When the ph is figured, it can be put on a scale to measure the whether the concentration is in fact an acid, or a base. The ph scale along with the direct relationship to the hydronium ion and hydroxide ion concentrations is as follows: PH [H3O+] [OH-] pOH Basic 14 10-14 1 0 Neutral 7 10-7 10-7 7 Acidic 0 1 10-14 14 Now that we understand what an acid and a base are and how they are measured in relationship to their concentrations, we can take a look at the theories developed by Arrhenius, Bronsted-Lowry and Lewis with reg...