https://www.sciencemadness.org/smwiki/index.php?title=Sulfamic_acid&feed=atom&action=history
Sulfamic acid - Revision history
2024-03-29T15:42:40Z
Revision history for this page on the wiki
MediaWiki 1.25.1
https://www.sciencemadness.org/smwiki/index.php?title=Sulfamic_acid&diff=15389&oldid=prev
Mabus: /* Properties */
2023-11-18T12:58:33Z
<p><span dir="auto"><span class="autocomment">Properties</span></span></p>
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<td colspan='2' style="background-color: white; color:black; text-align: center;">← Older revision</td>
<td colspan='2' style="background-color: white; color:black; text-align: center;">Revision as of 12:58, 18 November 2023</td>
</tr><tr><td colspan="2" class="diff-lineno" id="L133" >Line 133:</td>
<td colspan="2" class="diff-lineno">Line 133:</td></tr>
<tr><td class='diff-marker'> </td><td style="background-color: #f9f9f9; color: #333333; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #e6e6e6; vertical-align: top; white-space: pre-wrap;"><div>Upon heating sulfamic acid will react with alcohols to form the corresponding organosulfates.</div></td><td class='diff-marker'> </td><td style="background-color: #f9f9f9; color: #333333; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #e6e6e6; vertical-align: top; white-space: pre-wrap;"><div>Upon heating sulfamic acid will react with alcohols to form the corresponding organosulfates.</div></td></tr>
<tr><td class='diff-marker'> </td><td style="background-color: #f9f9f9; color: #333333; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #e6e6e6; vertical-align: top; white-space: pre-wrap;"></td><td class='diff-marker'> </td><td style="background-color: #f9f9f9; color: #333333; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #e6e6e6; vertical-align: top; white-space: pre-wrap;"></td></tr>
<tr><td class='diff-marker'>−</td><td style="color:black; 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>Refluxing sulfamic acid with [[methanol]] will yield [[methylamine]].</div></td><td class='diff-marker'>+</td><td style="color:black; 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>Refluxing sulfamic acid with [[methanol]] will yield <ins class="diffchange diffchange-inline">ammonium methyl sulfate, which can be easily converted into </ins>[[methylamine]] <ins class="diffchange diffchange-inline">(sulfate) by heating it at high temperatures</ins>.<ins class="diffchange diffchange-inline"><ref>[https://www.youtube.com/watch?v=zU9qJRfISIk Making Ammonium Methyl Sulfate]</ref></ins></div></td></tr>
<tr><td class='diff-marker'> </td><td style="background-color: #f9f9f9; color: #333333; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #e6e6e6; vertical-align: top; white-space: pre-wrap;"></td><td class='diff-marker'> </td><td style="background-color: #f9f9f9; color: #333333; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #e6e6e6; vertical-align: top; white-space: pre-wrap;"></td></tr>
<tr><td class='diff-marker'> </td><td style="background-color: #f9f9f9; color: #333333; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #e6e6e6; vertical-align: top; white-space: pre-wrap;"><div>Sulfamic acid melts at 205 °C before decomposing at higher temperatures to [[water]], [[sulfur trioxide]], [[sulfur dioxide]] and [[nitrogen]].</div></td><td class='diff-marker'> </td><td style="background-color: #f9f9f9; color: #333333; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #e6e6e6; vertical-align: top; white-space: pre-wrap;"><div>Sulfamic acid melts at 205 °C before decomposing at higher temperatures to [[water]], [[sulfur trioxide]], [[sulfur dioxide]] and [[nitrogen]].</div></td></tr>
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Mabus
https://www.sciencemadness.org/smwiki/index.php?title=Sulfamic_acid&diff=13841&oldid=prev
Mabus at 20:09, 24 February 2021
2021-02-24T20:09:02Z
<p></p>
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<td colspan='2' style="background-color: white; color:black; text-align: center;">← Older revision</td>
<td colspan='2' style="background-color: white; color:black; text-align: center;">Revision as of 20:09, 24 February 2021</td>
</tr><tr><td colspan="2" class="diff-lineno" id="L128" >Line 128:</td>
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<tr><td class='diff-marker'> </td><td style="background-color: #f9f9f9; color: #333333; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #e6e6e6; vertical-align: top; white-space: pre-wrap;"><div>Sulfamic acid reacts with [[nitrous acid]] to give [[nitrogen]], while reaction with [[nitric acid]], it affords [[nitrous oxide]]:</div></td><td class='diff-marker'> </td><td style="background-color: #f9f9f9; color: #333333; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #e6e6e6; vertical-align: top; white-space: pre-wrap;"><div>Sulfamic acid reacts with [[nitrous acid]] to give [[nitrogen]], while reaction with [[nitric acid]], it affords [[nitrous oxide]]:</div></td></tr>
<tr><td class='diff-marker'> </td><td style="background-color: #f9f9f9; color: #333333; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #e6e6e6; vertical-align: top; white-space: pre-wrap;"></td><td class='diff-marker'> </td><td style="background-color: #f9f9f9; color: #333333; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #e6e6e6; vertical-align: top; white-space: pre-wrap;"></td></tr>
<tr><td class='diff-marker'>−</td><td style="color:black; 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>:HNO<sub>2</sub> + H<sub>3</sub>NSO<sub>3</sub> → H<sub>2</sub>SO<sub>4</sub> + N<sub>2</sub> + H<sub>2</sub>O</div></td><td class='diff-marker'>+</td><td style="color:black; 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>: HNO<sub>2</sub> + H<sub>3</sub>NSO<sub>3</sub> → H<sub>2</sub>SO<sub>4</sub> + N<sub>2</sub> + H<sub>2</sub>O</div></td></tr>
<tr><td class='diff-marker'>−</td><td style="color:black; 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>:HNO<sub>3</sub> + H<sub>3</sub>NSO<sub>3</sub> → H<sub>2</sub>SO<sub>4</sub> + N<sub>2</sub>O + H<sub>2</sub>O</div></td><td class='diff-marker'>+</td><td style="color:black; 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>: HNO<sub>3</sub> + H<sub>3</sub>NSO<sub>3</sub> → H<sub>2</sub>SO<sub>4</sub> + N<sub>2</sub>O + H<sub>2</sub>O</div></td></tr>
<tr><td class='diff-marker'> </td><td style="background-color: #f9f9f9; color: #333333; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #e6e6e6; vertical-align: top; white-space: pre-wrap;"></td><td class='diff-marker'> </td><td style="background-color: #f9f9f9; color: #333333; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #e6e6e6; vertical-align: top; white-space: pre-wrap;"></td></tr>
<tr><td class='diff-marker'> </td><td style="background-color: #f9f9f9; color: #333333; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #e6e6e6; vertical-align: top; white-space: pre-wrap;"><div>Upon heating sulfamic acid will react with alcohols to form the corresponding organosulfates.</div></td><td class='diff-marker'> </td><td style="background-color: #f9f9f9; color: #333333; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #e6e6e6; vertical-align: top; white-space: pre-wrap;"><div>Upon heating sulfamic acid will react with alcohols to form the corresponding organosulfates.</div></td></tr>
<tr><td colspan="2" class="diff-lineno" id="L153" >Line 153:</td>
<td colspan="2" class="diff-lineno">Line 153:</td></tr>
<tr><td class='diff-marker'> </td><td style="background-color: #f9f9f9; color: #333333; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #e6e6e6; vertical-align: top; white-space: pre-wrap;"><div>Hydrolysis of sulfamide will yield sulfamic acid.</div></td><td class='diff-marker'> </td><td style="background-color: #f9f9f9; color: #333333; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #e6e6e6; vertical-align: top; white-space: pre-wrap;"><div>Hydrolysis of sulfamide will yield sulfamic acid.</div></td></tr>
<tr><td class='diff-marker'> </td><td style="background-color: #f9f9f9; color: #333333; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #e6e6e6; vertical-align: top; white-space: pre-wrap;"></td><td class='diff-marker'> </td><td style="background-color: #f9f9f9; color: #333333; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #e6e6e6; vertical-align: top; white-space: pre-wrap;"></td></tr>
<tr><td class='diff-marker'>−</td><td style="color:black; 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>Preparation of sulfamic acid is not something any amateur chemist can do at home, due to the extreme conditions the preparation requires. As such, it's much more economical to simply purchase the compound, <del class="diffchange diffchange-inline">and </del>usually <del class="diffchange diffchange-inline">is </del>readily available.</div></td><td class='diff-marker'>+</td><td style="color:black; 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>Preparation of sulfamic acid is not something any amateur chemist can do at home, due to the extreme conditions the preparation requires. As such, it's much more economical to simply purchase the compound, <ins class="diffchange diffchange-inline">as </ins>usually <ins class="diffchange diffchange-inline">it's </ins>readily available.</div></td></tr>
<tr><td class='diff-marker'> </td><td style="background-color: #f9f9f9; color: #333333; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #e6e6e6; vertical-align: top; white-space: pre-wrap;"></td><td class='diff-marker'> </td><td style="background-color: #f9f9f9; color: #333333; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #e6e6e6; vertical-align: top; white-space: pre-wrap;"></td></tr>
<tr><td class='diff-marker'> </td><td style="background-color: #f9f9f9; color: #333333; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #e6e6e6; vertical-align: top; white-space: pre-wrap;"><div>==Projects==</div></td><td class='diff-marker'> </td><td style="background-color: #f9f9f9; color: #333333; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #e6e6e6; vertical-align: top; white-space: pre-wrap;"><div>==Projects==</div></td></tr>
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Mabus
https://www.sciencemadness.org/smwiki/index.php?title=Sulfamic_acid&diff=12841&oldid=prev
Mabus at 00:20, 29 March 2020
2020-03-29T00:20:10Z
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Mabus
https://www.sciencemadness.org/smwiki/index.php?title=Sulfamic_acid&diff=11347&oldid=prev
Mabus at 14:42, 5 June 2019
2019-06-05T14:42:26Z
<p></p>
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<td colspan='2' style="background-color: white; color:black; text-align: center;">Revision as of 14:42, 5 June 2019</td>
</tr><tr><td colspan="2" class="diff-lineno" id="L153" >Line 153:</td>
<td colspan="2" class="diff-lineno">Line 153:</td></tr>
<tr><td class='diff-marker'> </td><td style="background-color: #f9f9f9; color: #333333; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #e6e6e6; vertical-align: top; white-space: pre-wrap;"><div>Hydrolysis of sulfamide will yield sulfamic acid.</div></td><td class='diff-marker'> </td><td style="background-color: #f9f9f9; color: #333333; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #e6e6e6; vertical-align: top; white-space: pre-wrap;"><div>Hydrolysis of sulfamide will yield sulfamic acid.</div></td></tr>
<tr><td class='diff-marker'> </td><td style="background-color: #f9f9f9; color: #333333; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #e6e6e6; vertical-align: top; white-space: pre-wrap;"></td><td class='diff-marker'> </td><td style="background-color: #f9f9f9; color: #333333; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #e6e6e6; vertical-align: top; white-space: pre-wrap;"></td></tr>
<tr><td class='diff-marker'>−</td><td style="color:black; 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>Preparation of sulfamic acid is not something any amateur chemist can do at home, due to the extreme conditions the preparation requires. As such, it's much more economical to simply purchase the compound.</div></td><td class='diff-marker'>+</td><td style="color:black; 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>Preparation of sulfamic acid is not something any amateur chemist can do at home, due to the extreme conditions the preparation requires. As such, it's much more economical to simply purchase the compound<ins class="diffchange diffchange-inline">, and usually is readily available</ins>.</div></td></tr>
<tr><td class='diff-marker'> </td><td style="background-color: #f9f9f9; color: #333333; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #e6e6e6; vertical-align: top; white-space: pre-wrap;"></td><td class='diff-marker'> </td><td style="background-color: #f9f9f9; color: #333333; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #e6e6e6; vertical-align: top; white-space: pre-wrap;"></td></tr>
<tr><td class='diff-marker'> </td><td style="background-color: #f9f9f9; color: #333333; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #e6e6e6; vertical-align: top; white-space: pre-wrap;"><div>==Projects==</div></td><td class='diff-marker'> </td><td style="background-color: #f9f9f9; color: #333333; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #e6e6e6; vertical-align: top; white-space: pre-wrap;"><div>==Projects==</div></td></tr>
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Mabus
https://www.sciencemadness.org/smwiki/index.php?title=Sulfamic_acid&diff=11292&oldid=prev
Mabus at 22:13, 27 May 2019
2019-05-27T22:13:53Z
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<tr><td class='diff-marker'> </td><td style="background-color: #f9f9f9; color: #333333; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #e6e6e6; vertical-align: top; white-space: pre-wrap;"></td><td class='diff-marker'> </td><td style="background-color: #f9f9f9; color: #333333; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #e6e6e6; vertical-align: top; white-space: pre-wrap;"></td></tr>
<tr><td class='diff-marker'> </td><td style="background-color: #f9f9f9; color: #333333; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #e6e6e6; vertical-align: top; white-space: pre-wrap;"><div>===Physical===</div></td><td class='diff-marker'> </td><td style="background-color: #f9f9f9; color: #333333; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #e6e6e6; vertical-align: top; white-space: pre-wrap;"><div>===Physical===</div></td></tr>
<tr><td class='diff-marker'>−</td><td style="color:black; 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>Sulfamic acid is a colorless odorless solid acid, soluble in water, but insoluble in organic solvents. Sulfamic acid is not hygroscopic.</div></td><td class='diff-marker'>+</td><td style="color:black; 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>Sulfamic acid is a colorless odorless solid acid, soluble in water, but insoluble in organic solvents. Sulfamic acid is not hygroscopic<ins class="diffchange diffchange-inline">, though finely powdered form may appear "sticky", similar to wet snow in appearance</ins>.</div></td></tr>
<tr><td class='diff-marker'> </td><td style="background-color: #f9f9f9; color: #333333; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #e6e6e6; vertical-align: top; white-space: pre-wrap;"></td><td class='diff-marker'> </td><td style="background-color: #f9f9f9; color: #333333; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #e6e6e6; vertical-align: top; white-space: pre-wrap;"></td></tr>
<tr><td class='diff-marker'> </td><td style="background-color: #f9f9f9; color: #333333; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #e6e6e6; vertical-align: top; white-space: pre-wrap;"><div>==Availability==</div></td><td class='diff-marker'> </td><td style="background-color: #f9f9f9; color: #333333; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #e6e6e6; vertical-align: top; white-space: pre-wrap;"><div>==Availability==</div></td></tr>
</table>
Mabus
https://www.sciencemadness.org/smwiki/index.php?title=Sulfamic_acid&diff=10096&oldid=prev
Mabus at 13:51, 1 December 2018
2018-12-01T13:51:08Z
<p></p>
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<td colspan='2' style="background-color: white; color:black; text-align: center;">← Older revision</td>
<td colspan='2' style="background-color: white; color:black; text-align: center;">Revision as of 13:51, 1 December 2018</td>
</tr><tr><td colspan="2" class="diff-lineno" id="L7" >Line 7:</td>
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<tr><td class='diff-marker'> </td><td style="background-color: #f9f9f9; color: #333333; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #e6e6e6; vertical-align: top; white-space: pre-wrap;"><div>| OtherNames = Amidosulfonic acid<br>Amidosulfuric acid<br>Aminosulfonic acid<br>Imidosulfonic acid<br>Sulfamidic acid</div></td><td class='diff-marker'> </td><td style="background-color: #f9f9f9; color: #333333; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #e6e6e6; vertical-align: top; white-space: pre-wrap;"><div>| OtherNames = Amidosulfonic acid<br>Amidosulfuric acid<br>Aminosulfonic acid<br>Imidosulfonic acid<br>Sulfamidic acid</div></td></tr>
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Mabus
https://www.sciencemadness.org/smwiki/index.php?title=Sulfamic_acid&diff=9980&oldid=prev
Mabus: Created page with "{{Chembox | Name = Sulfamic acid | Reference = | IUPACName = Sulfamic acid | PIN = | SystematicName = Sulfamic acid | OtherNames = Amidosulfonic acid<br>Amidosulfuric acid<br>..."
2018-11-24T18:39:47Z
<p>Created page with "{{Chembox | Name = Sulfamic acid | Reference = | IUPACName = Sulfamic acid | PIN = | SystematicName = Sulfamic acid | OtherNames = Amidosulfonic acid<br>Amidosulfuric acid<br>..."</p>
<p><b>New page</b></p><div>{{Chembox<br />
| Name = Sulfamic acid<br />
| Reference =<br />
| IUPACName = Sulfamic acid<br />
| PIN =<br />
| SystematicName = Sulfamic acid<br />
| OtherNames = Amidosulfonic acid<br>Amidosulfuric acid<br>Aminosulfonic acid<br>Imidosulfonic acid<br>Sulfamidic acid<br />
<!-- Images --><br />
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<!-- Sections --><br />
| Section1 = {{Chembox Identifiers<br />
| 3DMet = <br />
| Abbreviations = <br />
| SMILES = <br />
}}<br />
| Section2 = {{Chembox Properties<br />
| AtmosphericOHRateConstant = <br />
| Appearance = Colorless solid<br />
| BoilingPt = <br />
| BoilingPtC = <br />
| BoilingPt_ref = <br />
| BoilingPt_notes = Decomposes<br />
| Density = 2.15 g/cm<sup>3</sup><br />
| Formula = H<sub>3</sub>NSO<sub>3</sub><br />
| HenryConstant = <br />
| LogP = 0.1<br />
| MolarMass = 97.10 g/mol<br />
| MeltingPt = <br />
| MeltingPtC = 205<br />
| MeltingPt_ref = <br />
| MeltingPt_notes = (decomposes)<br />
| Odor = Odorless<br />
| pKa = 1.0<br />
| pKb = <br />
| Solubility = 14.68 g/100 ml (0 °C)<br>18.56 g/100 ml (10 °C)<br>21.32 g/100 ml (20 °C)<br>26.09 g/100 ml (30 °C)<br>29.49 g/100 ml (40 °C)<br>32.82 g/100 ml (50 °C)<br>37.10 g/100 ml (60 °C)<br>41.91 g/100 ml (70 °C)<br>47.08 g/100 ml (80 °C)<br>Slow hydrolysis<br />
| SolubleOther = Moderately soluble in [[ammonia]], [[dimethylformamide|DMF]], [[formamide]]<br>Sparingly solubility in [[methanol]], [[sulfuric acid]]<br>Insoluble in [[acetone]], [[acetonitrile]], [[carbon disulfide]], [[carbon tetrachloride]], [[chloroform]], [[dichloromethane|DCM]], [[diethyl ether]], [[ethanol]], hydrocarbons<br />
| Solubility1 = 0.4 g/100 g<ref>Cupery, M. E.; Industrial and Engineering Chemistry; vol. 30; (1938); p. 627 - 631</ref><br />
| Solvent1 = acetone<br />
| Solubility2 = 0.009 g/100 g<br />
| Solvent2 = diethyl ether<br />
| Solubility3 = 20 g/100 g<br />
| Solvent3 = formamide<br />
| Solubility4 = 4.3 g/100 g<br />
| Solvent4 = methanol<br />
| Solubility5 = 2.38 g/100 g<br />
| Solvent5 = sulfuric acid<br />
| VaporPressure = ~0.06 mmHg (20 °C)<br />
}}<br />
| Section3 = {{Chembox Structure<br />
| Coordination = <br />
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}}<br />
| Section4 = {{Chembox Thermochemistry<br />
| DeltaGf = <br />
| DeltaHc = <br />
| DeltaHf = <br />
| Entropy = <br />
| HeatCapacity = 111.31 J·mol<sup>−1</sup>·K<sup>−1</sup><ref>Patron, M.; Ind. chim.; vol. 42; (1955); p. 237 - 243</ref><br />
}}<br />
| Section5 = {{Chembox Explosive<br />
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| Section6 = {{Chembox Hazards<br />
| AutoignitionPt = Non-flammable<br />
| ExploLimits = Non-flammable<br />
| ExternalMSDS = [https://www.docdroid.net/qExSBve/sulfamic-acid-sa.pdf Sigma-Aldrich]<br />
| FlashPt = Non-flammable<br />
| LD50 = 3,160 mg/kg (rat, oral)<br>1,312 mg/kg (mouse, oral)<br>1,050 mg/kg (guinea pig, oral)<br />
| LC50 = <br />
| MainHazards = Corrosive<br />
| NFPA-F = <br />
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| NFPA-R = <br />
| NFPA-S = <br />
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| Section7 = {{Chembox Related<br />
| OtherAnions = <br />
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| OtherFunction = <br />
| OtherFunction_label = <br />
| OtherCompounds = [[Sulfuric acid]]<br>[[Sulfamide]]<br />
}}<br />
}}<br />
'''Sulfamic acid''', also known as '''amidosulfonic acid''', '''aminosulfonic acid''' or '''sulfamidic acid''', is a chemical compound with the formula '''H<sub>3</sub>NSO<sub>3</sub>''' or '''H<sub>2</sub>NSO<sub>3</sub>H''', a solid strong acid at room.<br />
<br />
==Properties==<br />
===Chemical===<br />
Sulfamic acid is a moderately strong acid, Ka = 0.101 (pKa = 0.995).<br />
<br />
Aqueous solutions of sulfamic acid are unstable and slowly hydrolyze to [[ammonium bisulfate]], but the crystalline solid is indefinitely stable under ordinary storage conditions.<br />
<br />
Sulfamic acid reacts with [[nitrous acid]] to give [[nitrogen]], while reaction with [[nitric acid]], it affords [[nitrous oxide]]:<br />
<br />
:HNO<sub>2</sub> + H<sub>3</sub>NSO<sub>3</sub> → H<sub>2</sub>SO<sub>4</sub> + N<sub>2</sub> + H<sub>2</sub>O<br />
:HNO<sub>3</sub> + H<sub>3</sub>NSO<sub>3</sub> → H<sub>2</sub>SO<sub>4</sub> + N<sub>2</sub>O + H<sub>2</sub>O<br />
<br />
Upon heating sulfamic acid will react with alcohols to form the corresponding organosulfates.<br />
<br />
Refluxing sulfamic acid with [[methanol]] will yield [[methylamine]].<br />
<br />
Sulfamic acid melts at 205 °C before decomposing at higher temperatures to [[water]], [[sulfur trioxide]], [[sulfur dioxide]] and [[nitrogen]].<br />
<br />
: H<sub>3</sub>NSO<sub>3</sub> → H<sub>2</sub>O + SO<sub>3</sub> + SO<sub>2</sub> + N<sub>2</sub><br />
<br />
===Physical===<br />
Sulfamic acid is a colorless odorless solid acid, soluble in water, but insoluble in organic solvents. Sulfamic acid is not hygroscopic.<br />
<br />
==Availability==<br />
Sulfamic acid is readily available as solid acidic descaling agent, sold in many hardware stores. Sometimes it's sold as coffee machine cleaning powder, though always read the label, as many have producers have replaced it with [[citric acid]].<br />
<br />
==Preparation==<br />
Sulfamic acid is produced industrially by treating [[urea]] with a mixture of [[sulfur trioxide]] and [[sulfuric acid]] (or [[oleum]]). The conversion is conducted in two stages:<br />
<br />
: (NH<sub>2</sub>)<sub>2</sub>CO + SO<sub>3</sub> → OC(NH<sub>2</sub>)(NHSO<sub>3</sub>H)<br />
: OC(NH<sub>2</sub>)(NHSO<sub>3</sub>H) + H<sub>2</sub>SO<sub>4</sub> → CO<sub>2</sub> + 2 H<sub>3</sub>NSO<sub>3</sub><br />
<br />
Hydrolysis of sulfamide will yield sulfamic acid.<br />
<br />
Preparation of sulfamic acid is not something any amateur chemist can do at home, due to the extreme conditions the preparation requires. As such, it's much more economical to simply purchase the compound.<br />
<br />
==Projects==<br />
*Make nitrous oxide<br />
*Make [[methylamine]]<br />
*Make sodium cyclamate<br />
*Catalyst for esterification process<br />
*Make [[ammonium bisulfate]]<br />
*Make [[ammonium sulfamate]]<br />
*Make [[guanidinium sulfate]]<br />
*Make [[ammonium dinitramide]]<br />
*Coagulator for urea-formaldehyde resins<br />
*Silver polishing<br />
<br />
==Handling==<br />
===Safety===<br />
Sulfamic acid is irritant and should be handled with care.<br />
<br />
===Storage===<br />
Sulfamic acid is best stored in closed plastic bottles, away from ammonia and moisture.<br />
<br />
===Disposal===<br />
Can be neutralized with an aq. base, then poured down the drain.<br />
<br />
==References==<br />
<references/><br />
===Relevant Sciencemadness threads===<br />
*[http://www.sciencemadness.org/talk/viewthread.php?tid=73027 OTC sulfamic acid]<br />
*[http://www.sciencemadness.org/talk/viewthread.php?tid=63946 Sulfamic acid decomposition]<br />
*[http://www.sciencemadness.org/talk/viewthread.php?tid=31206 Reactions with Sulfamic acid]<br />
*[http://www.sciencemadness.org/talk/viewthread.php?tid=3477 Sulfamic acid]<br />
*[http://www.sciencemadness.org/talk/viewthread.php?tid=10928 Need help w/ Sulfamic synthesis]<br />
<br />
[[Category:Chemical compounds]]<br />
[[Category:Inorganic compounds]]<br />
[[Category:Sulfamates]]<br />
[[Category:Acids]]<br />
[[Category:Strong acids]]<br />
[[Category:Mineral acids]]<br />
[[Category:Oxoacids]]<br />
[[Category:Materials unstable in basic solution]]<br />
[[Category:Readily available chemicals]]<br />
[[Category:Essential reagents]]<br />
[[Category:Solids]]</div>
Mabus