Tellurous acid

<h2 id="properties">Properties</h2>
<p>In contrast to the analogous compound <a href="/facts/Selenous_acid/0jtCQBIB">selenous acid</a>, tellurous acid is only metastable. Most tellurite salts contain the TeO2−3 ion. Oxidation of its aqueous solution with hydrogen peroxide gives the <a href="/facts/Tellurate/jnAvMCss">tellurate</a> ion. It is usually prepared as an aqueous solution where it acts as a weak acid.<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>
</p>
H2TeO3 + H2O ⇌ H3O+ + HTeO−3 <i>K</i>a1 = 2×10−3
HTeO−3 + H2O ⇌ H3O+ + TeO2−3 <i>K</i>a2 = 1×10−8

<h2 id="references">References</h2>

<ol>
<li id="fn:1"><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:1" class="footnote-back-ref">↩</a></p></li>
<li id="fn:2"><p>Catherine E. Housecroft; Alan G. Sharpe (2008). "Chapter 16: The group 16 elements". Inorganic Chemistry (3rd ed.). Pearson. p. 524. ISBN 978-0-13-175553-6. <a href="978-0-13-175553-6" target="_blank">978-0-13-175553-6</a> <a href="#fnref:2" class="footnote-back-ref">↩</a></p></li>
<li id="fn:3"><p>"Ionization Constants for Weak Acids". www.austincc.edu. Archived from the original on 2014-10-20.
 <a href="https://web.archive.org/web/20141020041236/http://www.austincc.edu/chemlab/weakacid" target="_blank">https://web.archive.org/web/20141020041236/http://www.austincc.edu/chemlab/weakacid</a> <a href="#fnref:3" class="footnote-back-ref">↩</a></p></li>
</ol>

Tellurous acid open-in-new

Tellurous acid