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1.2 Arrhenius Theory of Acids & Bases

  • Page ID
    32052
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    Although the properties of acids and bases had been recognized for a long time, it was Svante Arrhenius in the 1880's who determined that:

    • the properties of acids were due to the presence of hydrogen ions, H+, and
    • the properties of bases were due to the presence of hydroxide ions, OH-.
    This became known as the
    Arrhenius Theory
    of Acids and Bases
    ACIDS
    hydrochloric acid, \(\ce{HCl}\)
    sulfuric acid, \(\ce{H2SO4}\)
    nitric acid, \(\ce{HNO3}\)
    acetic acid, \(\ce{HC2H3O2}\) (vinegar)
    carbonic acid, \(\ce{H2CO3}\)
    formic acid, \(\ce{HCOOH}\)
    acetylsalicylic acid,
    \(\ce{C6H4(OCOCH3)CO2H}\)
    BASES
    sodium hydroxide, \(\ce{NaOH}\)
    potassium hydroxide, \(\ce{KOH}\)
    magnesium hydroxide, \(\ce{Mg(OH)2}\)
    calcium hydroxide, \(\ce{Ca(OH)2}\)
    ammonia, \(\ce{NH3}\) - oops! Where's the OH-?

    An important aspect of that theory is that these compounds only become acid or bases when in solution. \(\ce{HCl}\), hydrogen chloride, for example is not an acid when in its gaseous phase (according to the Arrhenius Theory). Add it to water, however, and we have a very strong acid. We need to examine what happens when we add them to water that suddenly produces either acidic or basic properties.


    1.2 Arrhenius Theory of Acids & Bases is shared under a CC BY-NC-SA 4.0 license and was authored, remixed, and/or curated by LibreTexts.

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