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Beryllium hydroxide
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<h2 id="reactions">Reactions</h2> <p>Beryllium hydroxide is difficult to dissolve in water. With alkalis it dissolves to form the tetrahydroxoberyllate (also known as tetrahydroxidoberyllate) anion, [Be(OH)4]2−.<a class="footnote-ref" id="fnref:6" href="#fn:6"><sup>6</sup></a> With <a href="/facts/Sodium_hydroxide/xjtdYtq7">sodium hydroxide</a> solution: </p> 2 NaOH(aq) + Be(OH)2(s) → Na2[Be(OH)4](aq) <p>With acids, beryllium salts are formed.<a class="footnote-ref" id="fnref:7" href="#fn:7"><sup>7</sup></a> For example, with <a href="/facts/Sulfuric_acid/Wom6fymJ">sulfuric acid</a>, H2SO4, <a href="/facts/Beryllium_sulfate/8pgGhaBn">beryllium sulfate</a> is formed: </p> Be(OH)2 + H2SO4 → BeSO4 + 2 H2O <p>Beryllium hydroxide dehydrates at 400 °C to form the soluble white powder, <a href="/facts/Beryllium_oxide/o3VnG96d">beryllium oxide</a>:<a class="footnote-ref" id="fnref:8" href="#fn:8"><sup>8</sup></a> </p> Be(OH)2 → BeO + H2O <p>Further heating at higher temperature produces acid insoluble BeO.<a class="footnote-ref" id="fnref:9" href="#fn:9"><sup>9</sup></a> </p> <h2 id="references">References</h2> <ol> <li id="fn:1"><p>Jessica Elzea Kogel, Nikhil C. Trivedi, James M. Barker and Stanley T. Krukowski, 2006, Industrial Minerals & Rocks: Commodities, Markets, and Uses, 7th edition, SME, ISBN 0-87335-233-5 <a href="/wiki/ISBN_(identifier)" target="_blank">/wiki/ISBN_(identifier)</a> <a href="#fnref:1" class="footnote-back-ref">↩</a></p></li> <li id="fn:2"><p>Mindat, http://www.mindat.org/min-603.html <a href="http://www.mindat.org/min-603.html" target="_blank">http://www.mindat.org/min-603.html</a> <a href="#fnref:2" class="footnote-back-ref">↩</a></p></li> <li id="fn:3"><p>Mindat, http://www.mindat.org/min-1066.html <a href="http://www.mindat.org/min-1066.html" target="_blank">http://www.mindat.org/min-1066.html</a> <a href="#fnref:3" class="footnote-back-ref">↩</a></p></li> <li id="fn:4"><p>Mary Eagleson, 1994, Concise encyclopedia chemistry, Walter de Gruyter, ISBN 3-11-011451-8 <a href="/wiki/ISBN_(identifier)" target="_blank">/wiki/ISBN_(identifier)</a> <a href="#fnref:4" class="footnote-back-ref">↩</a></p></li> <li id="fn:5"><p>Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8. <a href="978-0-08-037941-8" target="_blank">978-0-08-037941-8</a> <a href="#fnref:5" class="footnote-back-ref">↩</a></p></li> <li id="fn:6"><p>Egon Wiberg, Arnold Frederick Holleman (2001) Inorganic Chemistry, Elsevier ISBN 0-12-352651-5 <a href="/wiki/ISBN_(identifier)" target="_blank">/wiki/ISBN_(identifier)</a> <a href="#fnref:6" class="footnote-back-ref">↩</a></p></li> <li id="fn:7"><p>Egon Wiberg, Arnold Frederick Holleman (2001) Inorganic Chemistry, Elsevier ISBN 0-12-352651-5 <a href="/wiki/ISBN_(identifier)" target="_blank">/wiki/ISBN_(identifier)</a> <a href="#fnref:7" class="footnote-back-ref">↩</a></p></li> <li id="fn:8"><p>Egon Wiberg, Arnold Frederick Holleman (2001) Inorganic Chemistry, Elsevier ISBN 0-12-352651-5 <a href="/wiki/ISBN_(identifier)" target="_blank">/wiki/ISBN_(identifier)</a> <a href="#fnref:8" class="footnote-back-ref">↩</a></p></li> <li id="fn:9"><p>Egon Wiberg, Arnold Frederick Holleman (2001) Inorganic Chemistry, Elsevier ISBN 0-12-352651-5 <a href="/wiki/ISBN_(identifier)" target="_blank">/wiki/ISBN_(identifier)</a> <a href="#fnref:9" class="footnote-back-ref">↩</a></p></li> </ol>