https://glossary.ametsoc.org/w/index.php?title=Ph&feed=atom&action=historyPh - Revision history2024-03-28T15:31:58ZRevision history for this page on the wikiMediaWiki 1.39.5https://glossary.ametsoc.org/w/index.php?title=Ph&diff=5070&oldid=prevUnknown user at 00:35, 26 April 20122012-04-26T00:35:52Z<p></p>
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<tr><td class="diff-marker"></td><td style="background-color: #f8f9fa; color: #202122; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #eaecf0; vertical-align: top; white-space: pre-wrap;"><br/></td><td class="diff-marker"></td><td style="background-color: #f8f9fa; color: #202122; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #eaecf0; vertical-align: top; white-space: pre-wrap;"><br/></td></tr>
<tr><td class="diff-marker" data-marker="−"></td><td style="color: #202122; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #ffe49c; vertical-align: top; white-space: pre-wrap;"><div><div class="definition"><div class="short_definition">In aqueous solution, the [[logarithm]] (base 10) of the inverse of the concentration of [[hydrogen]] ions expressed in moles per liter; a measure of solution acidity. Thus, <div class="inline-formula">[[File:ams2001glos-Pex04.gif|link=|ams2001glos-Pex04]]</div>.</div><br/> <div class="paragraph">The pH of neutral water is 7, since it contains 10<sup>-7</sup> moles hydrogen ions and 10<sup>-7</sup> moles hydroxyl [[ions]] per liter. Lower pH values correspond to more acidic solution. The pH of natural waters in the [[atmosphere]] is 5.5 or less, due to the dissolution of acidic gases such as [[carbon dioxide]] and [[sulfur dioxide]]. In polluted continental areas the pH can drop to as low as 3.0, a condition known as [[acid rain]], due to the production of sulfuric and nitric acids from [[anthropogenic]] activity.</div><br/> </div></div></td><td class="diff-marker" data-marker="+"></td><td style="color: #202122; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #a3d3ff; vertical-align: top; white-space: pre-wrap;"><div><div class="definition"><div class="short_definition">In aqueous solution, the [[logarithm]] (base 10) of the inverse of the concentration of [[hydrogen]] ions expressed in moles per liter; a measure of solution acidity. Thus, <div class="inline-formula">[[File:ams2001glos-Pex04.gif|link=|ams2001glos-Pex04]]</div>.</div><br/> <div class="paragraph">The pH of neutral water is 7, since it contains 10<sup>-7</sup> moles hydrogen ions and 10<sup>-7</sup> moles hydroxyl [[ions]] per liter. Lower pH values correspond to more acidic solution. The pH of natural waters in the [[atmosphere]] is 5.5 or less, due to the dissolution of acidic gases such as [[<ins style="font-weight: bold; text-decoration: none;">carbon dioxide|</ins>carbon dioxide]] and [[sulfur dioxide]]. In polluted continental areas the pH can drop to as low as 3.0, a condition known as [[acid rain]], due to the production of sulfuric and nitric acids from [[anthropogenic]] activity.</div><br/> </div></div></td></tr>
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</table>Unknown userhttps://glossary.ametsoc.org/w/index.php?title=Ph&diff=5069&oldid=prevUnknown user at 22:50, 20 February 20122012-02-20T22:50:13Z<p></p>
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<td colspan="2" style="background-color: #fff; color: #202122; text-align: center;">Revision as of 15:50, 20 February 2012</td>
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<tr><td class="diff-marker"></td><td style="background-color: #f8f9fa; color: #202122; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #eaecf0; vertical-align: top; white-space: pre-wrap;"><br/></td><td class="diff-marker"></td><td style="background-color: #f8f9fa; color: #202122; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #eaecf0; vertical-align: top; white-space: pre-wrap;"><br/></td></tr>
<tr><td class="diff-marker" data-marker="−"></td><td style="color: #202122; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #ffe49c; vertical-align: top; white-space: pre-wrap;"><div><div class="definition"><div class="short_definition">In aqueous solution, the [[logarithm]] (base 10) of the inverse of the concentration of [[hydrogen]] ions expressed in moles per liter; a measure of solution acidity. Thus, <div class="inline-formula">[[File:ams2001glos-Pex04.gif|link=|ams2001glos-Pex04]]</div>.</div><br/> <div class="paragraph">The pH of neutral water is 7, since it contains 10<sup><del style="font-weight: bold; text-decoration: none;">&minus;</del>7</sup> moles hydrogen ions and 10<sup><del style="font-weight: bold; text-decoration: none;">&minus;</del>7</sup> moles hydroxyl [[ions]] per liter. Lower pH values correspond to more acidic solution. The pH of natural waters in the [[atmosphere]] is 5.5 or less, due to the dissolution of acidic gases such as [[carbon dioxide]] and [[sulfur dioxide]]. In polluted continental areas the pH can drop to as low as 3.0, a condition known as [[acid rain]], due to the production of sulfuric and nitric acids from [[anthropogenic]] activity.</div><br/> </div></div></td><td class="diff-marker" data-marker="+"></td><td style="color: #202122; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #a3d3ff; vertical-align: top; white-space: pre-wrap;"><div><div class="definition"><div class="short_definition">In aqueous solution, the [[logarithm]] (base 10) of the inverse of the concentration of [[hydrogen]] ions expressed in moles per liter; a measure of solution acidity. Thus, <div class="inline-formula">[[File:ams2001glos-Pex04.gif|link=|ams2001glos-Pex04]]</div>.</div><br/> <div class="paragraph">The pH of neutral water is 7, since it contains 10<sup><ins style="font-weight: bold; text-decoration: none;">-</ins>7</sup> moles hydrogen ions and 10<sup><ins style="font-weight: bold; text-decoration: none;">-</ins>7</sup> moles hydroxyl [[ions]] per liter. Lower pH values correspond to more acidic solution. The pH of natural waters in the [[atmosphere]] is 5.5 or less, due to the dissolution of acidic gases such as [[carbon dioxide]] and [[sulfur dioxide]]. In polluted continental areas the pH can drop to as low as 3.0, a condition known as [[acid rain]], due to the production of sulfuric and nitric acids from [[anthropogenic]] activity.</div><br/> </div></div></td></tr>
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</table>Unknown userhttps://glossary.ametsoc.org/w/index.php?title=Ph&diff=5068&oldid=prevUnknown user: Created page with " {{TermHeader}} {{TermSearch}} <div class="termentry"> <div class="term"> == pH == </div> <div class="definition"><div class="short_definition">In aqueous solution, the..."2012-01-27T01:41:16Z<p>Created page with " {{TermHeader}} {{TermSearch}} <div class="termentry"> <div class="term"> == pH == </div> <div class="definition"><div class="short_definition">In aqueous solution, the..."</p>
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== pH ==<br />
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<div class="definition"><div class="short_definition">In aqueous solution, the [[logarithm]] (base 10) of the inverse of the concentration of [[hydrogen]] ions expressed in moles per liter; a measure of solution acidity. Thus, <div class="inline-formula">[[File:ams2001glos-Pex04.gif|link=|ams2001glos-Pex04]]</div>.</div><br/> <div class="paragraph">The pH of neutral water is 7, since it contains 10<sup>&minus;7</sup> moles hydrogen ions and 10<sup>&minus;7</sup> moles hydroxyl [[ions]] per liter. Lower pH values correspond to more acidic solution. The pH of natural waters in the [[atmosphere]] is 5.5 or less, due to the dissolution of acidic gases such as [[carbon dioxide]] and [[sulfur dioxide]]. In polluted continental areas the pH can drop to as low as 3.0, a condition known as [[acid rain]], due to the production of sulfuric and nitric acids from [[anthropogenic]] activity.</div><br/> </div><br />
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[[Category:Terms_P]]</div>Unknown user