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Betts electrolytic process
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<h2 id="process-description-for-lead">Process description for lead</h2> <p>The <a href="/facts/Electrolyte/4YE8bIVa">electrolyte</a> for this process is a mixture of lead fluorosilicate ("PbSiF6") and <a href="/facts/Hexafluorosilicic_acid/J35wRTRh">hexafluorosilicic acid</a> (H2SiF6) operating at 45 °C (113 °F). Cathodes are thin sheets of pure lead and anodes are cast from the impure lead to be purified. A potential of 0.5 volts is applied. At the anode, lead dissolves, as do metal impurities that are less noble than lead. Impurities that are more noble than lead, such as silver, gold, and bismuth, flake from the anode as it dissolves and settle to the bottom of the vessel as "anode mud." Pure metallic lead plates onto the cathode, with the less noble metals remaining in solution. Because of its high cost, electrolysis is used only when very pure lead is needed. Otherwise pyrometallurgical methods are preferred, such as the <a href="/facts/Parkes_process/NASalU7Q">Parkes process</a> followed by the <a href="/facts/Betterton-Kroll_process/KVFmY9Nt">Betterton-Kroll process</a>.<a class="footnote-ref" id="fnref:2" href="#fn:2"><sup>2</sup></a><a class="footnote-ref" id="fnref:3" href="#fn:3"><sup>3</sup></a><a class="footnote-ref" id="fnref:4" href="#fn:4"><sup>4</sup></a> </p> <h2 id="history">History</h2> <p>The process is named for its inventor Anson Gardner Betts who filed several patents for this method starting in 1901.<a class="footnote-ref" id="fnref:5" href="#fn:5"><sup>5</sup></a><a class="footnote-ref" id="fnref:6" href="#fn:6"><sup>6</sup></a> </p> <h2 id="see-also">See also</h2> <ul><li><a href="/facts/Lead/EYljasJN">Processing lead from ore</a></li> <li><a href="/facts/Lead_smelter/PLrBJ7EK">Lead smelter</a></li> <li><a href="/facts/Electrochemical_engineering/QcHfW5RE">Electrochemical engineering</a></li></ul> <h2 id="external-links">External links</h2> <ul><li><a href="https://web.archive.org/web/20061006210829/http://www.epa.gov/epaoswer/other/mining/minedock/id/id4-bis.pdf">Bismuth</a></li></ul> <h2 id="references">References</h2> <ol> <li id="fn:1"><p>Charles A. Sutherland, Edward F. Milner, Robert C. Kerby, Herbert Teindl, Albert Melin Hermann M. Bolt "Lead" in Ullmann's Encyclopedia of Industrial Chemistry, 2005, Wiley-VCH, Weinheim. doi:10.1002/14356007.a15_193.pub2 <a href="/wiki/Doi_(identifier)" target="_blank">/wiki/Doi_(identifier)</a> <a href="#fnref:1" class="footnote-back-ref">↩</a></p></li> <li id="fn:2"><p>Samans, Carl H. Engineering Metals and their Alloys, 1949 MacMillan <a href="#fnref:2" class="footnote-back-ref">↩</a></p></li> <li id="fn:3"><p>Ojebuoboh, Funsho K. (1992). "Bismuth—Production, properties, and applications". JOM. 44 (4): 46–49. Bibcode:1992JOM....44d..46O. doi:10.1007/BF03222821. S2CID 52993615. <a href="/wiki/Bibcode_(identifier)" target="_blank">/wiki/Bibcode_(identifier)</a> <a href="#fnref:3" class="footnote-back-ref">↩</a></p></li> <li id="fn:4"><p>Betts, Anson Gardner (May 2008). Lead Refining by Electrolysis. Read Books. ISBN 9781409730156. <a href="9781409730156" target="_blank">9781409730156</a> <a href="#fnref:4" class="footnote-back-ref">↩</a></p></li> <li id="fn:5"><p>us 679824 <a href="https://worldwide.espacenet.com/textdoc?DB=EPODOC&IDX=us679824" target="_blank">https://worldwide.espacenet.com/textdoc?DB=EPODOC&IDX=us679824</a> <a href="#fnref:5" class="footnote-back-ref">↩</a></p></li> <li id="fn:6"><p>us 713278 <a href="https://worldwide.espacenet.com/textdoc?DB=EPODOC&IDX=us713278" target="_blank">https://worldwide.espacenet.com/textdoc?DB=EPODOC&IDX=us713278</a> <a href="#fnref:6" class="footnote-back-ref">↩</a></p></li> </ol>