<?xml version='1.0' encoding='utf-8'?>
<oai_dc:dc xmlns:dc="http://purl.org/dc/elements/1.1/" xmlns:oai_dc="http://www.openarchives.org/OAI/2.0/oai_dc/" xmlns:xsi="http://www.w3.org/2001/XMLSchema-instance" xsi:schemaLocation="http://www.openarchives.org/OAI/2.0/oai_dc/ http://www.openarchives.org/OAI/2.0/oai_dc.xsd">
  <dc:creator>William Back</dc:creator>
  <dc:date>1963</dc:date>
  <dc:description>&lt;p&gt;&lt;span&gt;The departure of&amp;nbsp;&lt;/span&gt;&lt;span class="ScopusTermHighlight"&gt;ground&lt;/span&gt;&lt;span&gt;&amp;nbsp;&lt;/span&gt;&lt;span class="ScopusTermHighlight"&gt;water&lt;/span&gt;&lt;span&gt;&amp;nbsp;from equilibrium with calcite is being studied&amp;nbsp;&lt;/span&gt;&lt;span class="ScopusTermHighlight"&gt;in&lt;/span&gt;&lt;span&gt;&amp;nbsp;&lt;/span&gt;&lt;span class="ScopusTermHighlight"&gt;central&lt;/span&gt;&lt;span&gt;&amp;nbsp;&lt;/span&gt;&lt;span class="ScopusTermHighlight"&gt;Florida&lt;/span&gt;&lt;span&gt;. Measurements of pH, temperature, and concentration of bicarbonate made&amp;nbsp;&lt;/span&gt;&lt;span class="ScopusTermHighlight"&gt;in&lt;/span&gt;&lt;span&gt;&amp;nbsp;the field are used with standard laboratory analyses of&amp;nbsp;&lt;/span&gt;&lt;span class="ScopusTermHighlight"&gt;water&lt;/span&gt;&lt;span&gt;&amp;nbsp;samples to calculate an ion activity product (K) for&amp;nbsp;&lt;/span&gt;&lt;span class="ScopusTermHighlight"&gt;calcium&lt;/span&gt;&lt;span&gt;&amp;nbsp;&lt;/span&gt;&lt;span class="ScopusTermHighlight"&gt;carbonate&lt;/span&gt;&lt;span&gt;. The calculated Kiap is compared with the equilibrium constant (Keq) for calcite to determine the departure from equilibrium. The&amp;nbsp;&lt;/span&gt;&lt;span class="ScopusTermHighlight"&gt;calcium&lt;/span&gt;&lt;span&gt;&amp;nbsp;concentration is lowest&amp;nbsp;&lt;/span&gt;&lt;span class="ScopusTermHighlight"&gt;in&lt;/span&gt;&lt;span&gt;&amp;nbsp;the area of the highest piezometric surface. Some of the highest concentrations of bicarbonate are&amp;nbsp;&lt;/span&gt;&lt;span class="ScopusTermHighlight"&gt;in&lt;/span&gt;&lt;span&gt;&amp;nbsp;the area of low&amp;nbsp;&lt;/span&gt;&lt;span class="ScopusTermHighlight"&gt;calcium&lt;/span&gt;&lt;span&gt;.&amp;nbsp;&lt;/span&gt;&lt;span class="ScopusTermHighlight"&gt;In&lt;/span&gt;&lt;span&gt;&amp;nbsp;about half of the area of&amp;nbsp;&lt;/span&gt;&lt;span class="ScopusTermHighlight"&gt;study&lt;/span&gt;&lt;span&gt;, the&amp;nbsp;&lt;/span&gt;&lt;span class="ScopusTermHighlight"&gt;water&lt;/span&gt;&lt;span&gt;&amp;nbsp;is undersaturated with respect to calcite. This indicates that solution of limestone can occur several hundred feet below the&amp;nbsp;&lt;/span&gt;&lt;span class="ScopusTermHighlight"&gt;water&lt;/span&gt;&lt;span&gt;&amp;nbsp;table.&lt;/span&gt;&lt;/p&gt;</dc:description>
  <dc:format>application/pdf</dc:format>
  <dc:identifier>10.1080/02626666309493336</dc:identifier>
  <dc:language>en</dc:language>
  <dc:publisher>Taylor &amp; Francis</dc:publisher>
  <dc:title>Preliminary results of a study of calcium carbonate saturation of ground water in central Florida</dc:title>
  <dc:type>article</dc:type>
</oai_dc:dc>