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Boric acid
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<h2 id="history">History</h2> <p>Orthoboric acid was first prepared by <a href="/facts/Wilhelm_Homberg/zyFNlCPL">Wilhelm Homberg</a> (1652–1715) from <a href="/facts/Borax/IQrXRJ3N">borax</a>, by the action of mineral acids, and was given the name <i>sal sedativum Hombergi</i> ("sedative salt of Homberg"). However, boric acid and <a href="/facts/Borate/5XwkBTv1">borates</a> have been used since the time of the <a href="/facts/Ancient_Greece/PTVBrWXq">ancient Greeks</a> for cleaning, preserving food, and other uses.<a class="footnote-ref" id="fnref:2" href="#fn:2"><sup>2</sup></a> </p> <h2 id="molecular-and-crystal-structure">Molecular and crystal structure</h2> <p>The three oxygen atoms form a <a href="/facts/Trigonal_planar_molecular_geometry/935Tdp3Y">trigonal planar geometry</a> around the boron. The B-O bond length is 136 pm, and the O-H is 97 pm. The <a href="/facts/Molecular_symmetry/BrDxAkTK">molecular point group</a> is <i>C</i>3h.<a class="footnote-ref" id="fnref:3" href="#fn:3"><sup>3</sup></a> </p><p>Two crystalline forms of orthoboric acid are known: <a href="/facts/Triclinic_crystal_system/Y6yEdqfN">triclinic</a> with <a href="/facts/Space_group/2XQx0J7M">space group</a> P1, and <a href="/facts/Hexagonal_crystal_system/sSSok8wo">trigonal</a> with space group P32. The former is the most common; the second, which is a bit more stable thermodynamically, can be obtained with a special preparation method.<a class="footnote-ref" id="fnref:4" href="#fn:4"><sup>4</sup></a> </p><p>The triclinic form of boric acid consists of layers of B(OH)3 molecules held together by hydrogen bonds with an O...O separation of 272 pm. The distance between two adjacent layers is 318 pm.<a class="footnote-ref" id="fnref:5" href="#fn:5"><sup>5</sup></a> While the layers of the triclinic phase are nearly trigonal with γ = 119.76°, <i>a</i> = 701.87 pm, and <i>b</i> = 703.5 pm (compared to <i>a</i> = 704.53(4) pm for the trigonal form), the stacking of the layers is somewhat offset in the triclinic phase, with α = 92.49° and β = 101.46°. The triclinic phase has <i>c</i> = 634.72 pm and the trigonal one has <i>a</i> = 956.08(7) pm.<a class="footnote-ref" id="fnref:6" href="#fn:6"><sup>6</sup></a><a class="footnote-ref" id="fnref:7" href="#fn:7"><sup>7</sup></a> </p> <table><tbody><tr><td></td><td></td></tr><tr><td>The <a href="/facts/Unit_cell/znygJqdx">unit cell</a> of boric acid</td><td><a href="/facts/Hydrogen_bond/85V86IIg">hydrogen bonding</a> (dashed lines)allows boric acid molecules to formparallel layers in the solid state</td></tr></tbody></table> <h2 id="preparation">Preparation</h2> <p>Boric acid may be prepared by reacting <a href="/facts/Borax/IQrXRJ3N">borax</a> (sodium tetraborate decahydrate) with a <a href="/facts/Mineral_acid/MaftYXr0">mineral acid</a>, such as <a href="/facts/Hydrochloric_acid/HqItJlUT">hydrochloric acid</a>: </p> Na2B4O7·10H2O + 2 HCl → 4 B(OH)3 + 2 NaCl + 5 H2O <p>It is also formed as a byproduct of hydrolysis of boron trihalides and <a href="/facts/Diborane/k7egwbPf">diborane</a>:<a class="footnote-ref" id="fnref:8" href="#fn:8"><sup>8</sup></a> </p> B2H6 + 6 H2O → 2 B(OH)3 + 6 H2 BX3 + 3 H2O → B(OH)3 + 3 HX (X = Cl, Br, I) <h2 id="reactions">Reactions</h2> <h3>Pyrolysis</h3> <p>When heated, orthoboric acid undergoes a three-step dehydration. The reported transition temperatures vary substantially from source to source. </p><p>When heated above 140 °C, orthoboric acid yields <a href="/facts/Metaboric_acid/G6qWQW2N">metaboric acid</a> (HBO2) with loss of one water molecule:<a class="footnote-ref" id="fnref:9" href="#fn:9"><sup>9</sup></a><a class="footnote-ref" id="fnref:10" href="#fn:10"><sup>10</sup></a> </p> B(OH)3 → HBO2 + H2O <p>Heating metaboric acid above about 180 °C eliminates another water molecule forming <a href="/facts/Tetraboric_acid/53nKyt9a">tetraboric acid</a>, also called pyroboric acid (H2B4O7):<a class="footnote-ref" id="fnref:11" href="#fn:11"><sup>11</sup></a><a class="footnote-ref" id="fnref:12" href="#fn:12"><sup>12</sup></a> </p> 4 HBO2 → H2B4O7 + H2O <p>Further heating (to about 530 °C) leads to <a href="/facts/Boron_trioxide/N9o3sNUJ">boron trioxide</a>:<a class="footnote-ref" id="fnref:13" href="#fn:13"><sup>13</sup></a><a class="footnote-ref" id="fnref:14" href="#fn:14"><sup>14</sup></a><a class="footnote-ref" id="fnref:15" href="#fn:15"><sup>15</sup></a> </p> H2B4O7 → 2 B2O3 + H2O <h3>Aqueous solution</h3> <p>When orthoboric acid is dissolved in water, it partially dissociates to give <a href="/facts/Metaboric_acid/G6qWQW2N">metaboric acid</a>: </p> B(OH)3 ⇌ HBO2 + H2O <p>The solution is mildly acidic due to the ionization of the acids: </p> B(OH)3 + H2O ⇌ [BO(OH)2]− + H3O+ HBO2 + H2O ⇌ [BO2]− + H3O+ <p>However, <a href="/facts/Raman_spectroscopy/XY063k29">Raman spectroscopy</a> of strongly alkaline solutions has shown the presence of <a href="/facts/Tetrahydroxyborate/VjSKKVgC">[B(OH)4]− ions</a>,<a class="footnote-ref" id="fnref:16" href="#fn:16"><sup>16</sup></a> leading some to conclude that the acidity is exclusively due to the abstraction of OH− from water:<a class="footnote-ref" id="fnref:17" href="#fn:17"><sup>17</sup></a> </p> B(OH)3 + HO− ⇌ B(OH)−4 <p>Equivalently, </p> B(OH)3 + H2O ⇌ B(OH)−4 + <a href="/facts/Hydron/pjypwafP">H+</a> (<i>K</i>a = 7.3×10−10; p<i>K</i>a = 9.14) <p>Or, more properly, </p> B(OH)3 + 2 H2O ⇌ B(OH)−4 + H3O+ <p>This reaction occurs in two steps, with the neutral complex aquatrihydroxyboron B(OH)3(OH2) as an intermediate:<a class="footnote-ref" id="fnref:18" href="#fn:18"><sup>18</sup></a> </p> B(OH)3 + H2O → B(OH)3(OH2) B(OH)3(OH2) + H2O → [B(OH)4]− + H3O+ <p>This reaction may be characterized as <a href="/facts/Lewis_acid/qlLqRvg2">Lewis acidity</a> of boron toward HO−, rather than as <a href="/facts/Br%25C3%25B8nsted_acid/bqxQnJoX">Brønsted acidity</a>.<a class="footnote-ref" id="fnref:19" href="#fn:19"><sup>19</sup></a><a class="footnote-ref" id="fnref:20" href="#fn:20"><sup>20</sup></a><a class="footnote-ref" id="fnref:21" href="#fn:21"><sup>21</sup></a> However, some of its behaviour towards some chemical reactions suggest it to be a tribasic acid in the Brønsted-Lowry sense as well. </p><p>Boric acid, mixed with <a href="/facts/Borax/IQrXRJ3N">borax</a> Na2B4O7·10H2O (more properly Na2B4O5(OH)4·8H2O) in the weight ratio of 4:5, is highly soluble in water, though they are not so soluble separately.<a class="footnote-ref" id="fnref:22" href="#fn:22"><sup>22</sup></a> </p> <h3>Sulfuric acid solution</h3> <p>Boric acid also dissolves in anhydrous sulfuric acid according to the equation:<a class="footnote-ref" id="fnref:23" href="#fn:23"><sup>23</sup></a> </p> B(OH)3 + 6 H2SO4 → [B(SO4H)4]− + 2 [HSO4]− + 3 H3O+ <p>The product is an extremely strong acid, even stronger than the original sulfuric acid.<a class="footnote-ref" id="fnref:24" href="#fn:24"><sup>24</sup></a> </p> <h3>Esterification</h3> <p>Boric acid reacts with alcohols to form <a href="/facts/Borate_ester/YjvR6GAH">borate esters</a>, B(OR)3 where R is <a href="/facts/Alkyl/vmEk8X4v">alkyl</a> or <a href="/facts/Aryl/M3z7QRXd">aryl</a>. The reaction is typically driven by a dehydrating agent, such as concentrated <a href="/facts/Sulfuric_acid/Wom6fymJ">sulfuric acid</a>:<a class="footnote-ref" id="fnref:25" href="#fn:25"><sup>25</sup></a> </p> B(OH)3 + 3 ROH → B(OR)3 + 3 H2O <h3>With vicinal diols</h3> <p>The acidity of boric acid solutions is considerably increased in the presence of <a href="/facts/Cis%25E2%2580%2593trans_isomerism/vqlchJly">cis</a>-<a href="/facts/Diol/pmaVtfKx">vicinal diols</a> (<a href="/facts/Organic_compound/gqCNaN45">organic compounds</a> containing similarly oriented <a href="/facts/Hydroxyl/1Hs2QAEv">hydroxyl</a> groups in adjacent <a href="/facts/Carbon/ukrgQexo">carbon</a> atoms, (R1,R2)=C(OH)−C(OH)=(R3,R4)) such as <a href="/facts/Glycerol/sRQ6NBQQ">glycerol</a> and <a href="/facts/Mannitol/CeHJsKMq">mannitol</a>.<a class="footnote-ref" id="fnref:26" href="#fn:26"><sup>26</sup></a><a class="footnote-ref" id="fnref:27" href="#fn:27"><sup>27</sup></a><a class="footnote-ref" id="fnref:28" href="#fn:28"><sup>28</sup></a><a class="footnote-ref" id="fnref:29" href="#fn:29"><sup>29</sup></a> </p><p>The tetrahydroxyborate anion formed in the dissolution spontaneously reacts with these diols to form relatively stable anion esters containing one or two five-member −B−O−C−C−O− rings. For example, the reaction with mannitol H(HCOH)6H, whose two middle hydroxyls are in <i>cis</i> orientation, can be written as: </p> B(OH)3 + H2O ⇌ [B(OH)4]− + H+ [B(OH)4]− + H(HCOH)6H ⇌ [B(OH)2(H(HCOH)2(HCO−)2(HCOH)2H)]− + 2 H2O [B(OH)2(H(HCOH)2(HCO−)2(HCOH)2H)]− + H(HCOH)6H ⇌ [B(H(HCOH)2(HCO−)2(HCOH)2H)2]− + 2 H2O <p>Giving the overall reaction: </p> B(OH)3 + 2 H(HCOH)6H ⇌ [B(H(HCOH)2(HCO−)2(HCOH)2H)2]− + 3 H2O + H+ <p>The stability of these mannitoborate ester anions shifts the equilibrium to the right, thereby increasing the solution's acidity by five orders of magnitude compared to that of pure boric oxide. This lowers the p<i>K</i>a from 9 to below 4 for a sufficient concentration of mannitol.<a class="footnote-ref" id="fnref:30" href="#fn:30"><sup>30</sup></a><a class="footnote-ref" id="fnref:31" href="#fn:31"><sup>31</sup></a><a class="footnote-ref" id="fnref:32" href="#fn:32"><sup>32</sup></a><a class="footnote-ref" id="fnref:33" href="#fn:33"><sup>33</sup></a> The resulting solution is referred to as mannitoboric acid. </p><p>The addition of mannitol to an initially neutral solution containing boric acid or simple borates lowers its <a href="/facts/PH/RnSv8D7y">pH</a> enough for it to be titrated by a strong base such as NaOH, including with an automated potentiometric <a href="/facts/Titrator/gGUfvQcW">titrator</a>. This property is used in analytical chemistry to determine the borate content of aqueous solutions, for example to monitor the depletion of boric acid by <a href="/facts/Neutron/oRCM1geb">neutrons</a> in the water of the primary circuit of <a href="/facts/Light-water_reactor/c330w1Wt">light-water reactor</a> when the compound is added as a <a href="/facts/Neutron_poison/bkruR3yz">neutron poison</a> during refueling operations.<a class="footnote-ref" id="fnref:34" href="#fn:34"><sup>34</sup></a> </p> <h2 id="toxicology">Toxicology</h2> <p>Based on mammalian <a href="/facts/Median_lethal_dose/PSTer8Wv">median lethal dose</a> (LD50) rating of 2,660 mg/kg body mass, boric acid is only poisonous if taken internally or inhaled in large quantities. The Fourteenth Edition of the <i><a href="/facts/Merck_Index/3X9mzhzx">Merck Index</a></i> indicates that the LD50 of boric acid is 5.14 g/kg for oral dosages given to rats, and that 5 to 20 g/kg has produced death in adult humans. For a 70 kg adult, at the lower 5 g/kg limit, 350 g could produce death in humans. For comparison's sake, the LD50 of <a href="/facts/Sodium_chloride/MWcXl3Mb">salt</a> is reported to be 3.75 g/kg in rats according to the <i>Merck Index</i>. According to the <a href="/facts/Agency_for_Toxic_Substances_and_Disease_Registry/jVG5SPBA">Agency for Toxic Substances and Disease Registry</a>, "The minimal lethal dose of ingested boron (as boric acid) was reported to be 2–3 g in infants, 5–6 g in children, and 15–20 g in adults. [...] However, a review of 784 human poisonings with boric acid (10–88 g) reported no fatalities, with 88% of cases being asymptomatic."<a class="footnote-ref" id="fnref:35" href="#fn:35"><sup>35</sup></a> Human studies in three borate exposure-rich comparison groups (U.S. Borax mine and production facility workers, Chinese boron workers, Turkish residents living near boron-rich regions) produced no indicators of developmental toxicity in blood and semen tests. The highest estimated exposure was 5 mg B/kg/day, likely due to eating in contaminated workplaces, more than 100 times the average daily exposure.<a class="footnote-ref" id="fnref:36" href="#fn:36"><sup>36</sup></a> </p><p>Long-term exposure to boric acid may be of more concern, causing kidney damage and eventually kidney failure (see links below). Although it does not appear to be <a href="/facts/Carcinogenic/soH8Y9CE">carcinogenic</a>, studies in dogs have reported <a href="/facts/Testicular_atrophy/mH1EKLzR">testicular atrophy</a> after exposure to 32 mg/(kg⋅day) for 90 days. This level, were it applicable to humans at like dose, would equate to a cumulative dose of 202 g over 90 days for a 70 kg adult, not far lower than the above LD50.<a class="footnote-ref" id="fnref:37" href="#fn:37"><sup>37</sup></a> </p><p>According to the CLH report for boric acid published by the Bureau for Chemical Substances Lodz, Poland, boric acid in high doses shows significant developmental toxicity and <a href="/facts/Teratogenicity/j4BN6lsB">teratogenicity</a> in rabbit, rat, and mouse fetuses, as well as cardiovascular defects, skeletal variations, and mild kidney lesions.<a class="footnote-ref" id="fnref:38" href="#fn:38"><sup>38</sup></a> As a consequence in the 30th ATP to EU directive 67/548/EEC of August 2008, the European Commission decided to amend its classification as <a href="/facts/Reprotoxic/t1NWkVr3">reprotoxic</a> category 2 and to apply the <a href="/facts/Risk_phrase/h0tkv79y">risk phrases</a> R60 (may impair fertility) and R61 (may cause harm to the unborn child).<a class="footnote-ref" id="fnref:39" href="#fn:39"><sup>39</sup></a><a class="footnote-ref" id="fnref:40" href="#fn:40"><sup>40</sup></a><a class="footnote-ref" id="fnref:41" href="#fn:41"><sup>41</sup></a><a class="footnote-ref" id="fnref:42" href="#fn:42"><sup>42</sup></a><a class="footnote-ref" id="fnref:43" href="#fn:43"><sup>43</sup></a> </p><p>At a 2010 European Diagnostics Manufacturing Association (EDMA) Meeting, several new additions to the <a href="/facts/Substance_of_very_high_concern/SPylhVqo">substance of very high concern</a> (SVHC) candidate list in relation to the <a href="/facts/Registration%2c_Evaluation%2c_Authorisation_and_Restriction_of_Chemicals/xzQp2nKs">Registration, Evaluation, Authorisation and Restriction of Chemicals</a> Regulations 2007 (REACH) were discussed. Following the registration and review completed as part of REACH, the classification of boric acid CAS 10043-35-3 / 11113-50-1 is listed from 1 December 2010 is <i>H360FD (May damage fertility. May damage the unborn child)</i>.<a class="footnote-ref" id="fnref:44" href="#fn:44"><sup>44</sup></a><a class="footnote-ref" id="fnref:45" href="#fn:45"><sup>45</sup></a> </p> <h2 id="physics">Physics</h2> <p>Sound absorption in <a href="/facts/Ocean/8W8lYgjD">oceans</a> not only depends on <a href="/facts/Water_molecule/FFsl65l1">water molecules</a> but also on dissolved salts present in low <a href="/facts/Concentration/wqBmz5od">concentration</a> in <a href="/facts/Seawater/fRBJjbws">seawater</a>.<a class="footnote-ref" id="fnref:46" href="#fn:46"><sup>46</sup></a><a class="footnote-ref" id="fnref:47" href="#fn:47"><sup>47</sup></a> Boric acid and <a href="/facts/Borate/5XwkBTv1">borate</a> ([B] ≈ 4 × 10-4 M in seawater)<a class="footnote-ref" id="fnref:48" href="#fn:48"><sup>48</sup></a> <a href="/facts/Relaxation_(physics)/IhdVkDQ4">relaxation</a> contributes to absorbing <a href="/facts/Sound/DlKXlPuF">sounds</a> in the low‐<a href="/facts/Frequency/QUSbPaW8">frequency</a> region (0.2–10 <a href="/facts/Hertz/6Wshj5qm">kHz</a>).<a class="footnote-ref" id="fnref:49" href="#fn:49"><sup>49</sup></a> At higher frequencies, between 10 and 1000 kHz <a href="/facts/Magnesium_sulfate/o3GwKEoQ">magnesium sulfate</a> (formed by the second most abundant <a href="/facts/Cation/wrbwhF3z">cation</a> and <a href="/facts/Anion/wrbwhF3z">anion</a> species in seawater) is the main contributor to the absorption of <a href="/facts/Acoustic_wave/Mf8m46AI">acoustic waves</a> in seawater.<a class="footnote-ref" id="fnref:50" href="#fn:50"><sup>50</sup></a> </p> <h2 id="uses">Uses</h2> <h3>Industrial</h3> <p>The primary industrial use of boric acid is in the manufacture of monofilament <a href="/facts/Fiberglass/T6MtJ4ep">fiberglass</a>, which is usually referred to as textile fiberglass. Textile fiberglass is used to reinforce plastics in applications that range from boats to industrial piping to computer circuit boards.<a class="footnote-ref" id="fnref:51" href="#fn:51"><sup>51</sup></a> </p><p>In the jewelry industry, boric acid is often used in combination with <a href="/facts/Denatured_alcohol/wQjVC0Ts">denatured alcohol</a> to reduce surface <a href="/facts/Oxidation/Pyd5RVcj">oxidation</a> and formation of <a href="/facts/Firescale/fzoD208u">firescale</a> on metals during <a href="/facts/Annealing_(metallurgy)/2AfoCE4X">annealing</a> and <a href="/facts/Soldering/fod6dLHD">soldering</a> operations.<a class="footnote-ref" id="fnref:52" href="#fn:52"><sup>52</sup></a><a class="footnote-ref" id="fnref:53" href="#fn:53"><sup>53</sup></a> </p><p>Boric acid is used in the production of glass in <a href="/facts/Liquid_crystal_display/8B6xGBEz">LCD</a> <a href="/facts/Flat_panel_display/jw0LWETN">flat panel displays</a>.<a class="footnote-ref" id="fnref:54" href="#fn:54"><sup>54</sup></a><a class="footnote-ref" id="fnref:55" href="#fn:55"><sup>55</sup></a> </p><p>In <a href="/facts/Electroplating/HbKf0SBb">electroplating</a>, boric acid is used as part of some proprietary formulas. One known formula uses about a 1 to 10 ratio of H3BO3 to <a href="/facts/Nickel(II)_sulfate/HURkbNgq">NiSO4</a>, a very small portion of <a href="/facts/Sodium_lauryl_sulfate/H0Q2z7W3">sodium lauryl sulfate</a> and a small portion of <a href="/facts/Sulfuric_acid/Wom6fymJ">H2SO4</a>. </p><p>The solution of orthoboric acid and borax in 4:5 ratio is used as a <a href="/facts/Fire_retardant/RkwChTJu">fire retarding agent</a> of wood by impregnation.<a class="footnote-ref" id="fnref:56" href="#fn:56"><sup>56</sup></a> Also, it is used in combination with other chemicals for the fire retardancy of wood-based materials.<a class="footnote-ref" id="fnref:57" href="#fn:57"><sup>57</sup></a> </p><p>It is also used in the manufacturing of ramming mass, a fine <a href="/facts/Silica/A3WILp6J">silica</a>-containing powder used for producing <a href="/facts/Induction_furnace/MI49lJYl">induction furnace</a> linings and <a href="/facts/Ceramic/9JKudpqX">ceramics</a>. </p><p>Boric acid is added to <a href="/facts/Borax/IQrXRJ3N">borax</a> for use as <a href="/facts/Welding/6EJ62mYV">welding</a> <a href="/facts/Flux_(metallurgy)/ruKFTPGD">flux</a> by <a href="/facts/Blacksmith/StvqhmLx">blacksmiths</a>.<a class="footnote-ref" id="fnref:58" href="#fn:58"><sup>58</sup></a> </p><p>Boric acid, in combination with <a href="/facts/Polyvinyl_alcohol/gGLGMTVP">polyvinyl alcohol</a> (PVA) or <a href="/facts/Silicone_oil/zeg2chHf">silicone oil</a>, is used to manufacture <a href="/facts/Silly_Putty/59KMx47U">Silly Putty</a>.<a class="footnote-ref" id="fnref:59" href="#fn:59"><sup>59</sup></a> </p><p>Boric acid is also present in the list of chemical additives used for <a href="/facts/Hydraulic_fracturing/cCTzfwkg">hydraulic fracturing</a> (fracking) in the <a href="/facts/Marcellus_Shale/SDEvtlGg">Marcellus Shale</a> in Pennsylvania.<a class="footnote-ref" id="fnref:60" href="#fn:60"><sup>60</sup></a> It is often used in conjunction with <a href="/facts/Guar_gum/Q7BLEnAd">guar gum</a> as <a href="/facts/Cross-link/zeQ9hEAA">cross-linking</a> and gelling agent for controlling the <a href="/facts/Viscosity/QLVfrdCz">viscosity</a> and the rheology of the fracking fluid injected at high pressure in the well. It is important to control the fluid viscosity for keeping in suspension on long transport distances the grains of the <a href="/facts/Hydraulic_fracturing_proppants/NJqeT6Ca">propping agents</a> aimed at maintaining the cracks in the <a href="/facts/Shale/bsIhqY5F">shales</a> sufficiently open to facilitate the gas extraction after the hydraulic pressure is relieved.<a class="footnote-ref" id="fnref:61" href="#fn:61"><sup>61</sup></a><a class="footnote-ref" id="fnref:62" href="#fn:62"><sup>62</sup></a><a class="footnote-ref" id="fnref:63" href="#fn:63"><sup>63</sup></a> The rheological properties of borate cross-linked guar gum <a href="/facts/Hydrogel/kYMJum9P">hydrogel</a> mainly depend on the <a href="/facts/PH/RnSv8D7y">pH</a> value.<a class="footnote-ref" id="fnref:64" href="#fn:64"><sup>64</sup></a> </p><p>Boric acid is used in some <a href="/facts/Fuse_(electrical)/xN78ylMS">expulsion-type electrical fuses</a> as a de-ionization/extinguishing agent.<a class="footnote-ref" id="fnref:65" href="#fn:65"><sup>65</sup></a> During an <a href="/facts/Electrical_fault/QaCmxu1r">electrical fault</a> in an expulsion-type fuse, a <a href="/facts/Plasma_(physics)/1d3btMVU">plasma</a> arc is generated by the disintegration and rapid <a href="/facts/Spring_(device)/jknGXzTq">spring</a>-loaded separation of the fusible element, which is typically a specialized metal rod that passes through a compressed mass of boric acid within the fuse assembly. The high-temperature plasma causes the boric acid to rapidly decompose into <a href="/facts/Water_vapor/DX5IUFG0">water vapor</a> and <a href="/facts/Boron_trioxide/N9o3sNUJ">boric anhydride</a>, and in-turn, the vaporization products de-ionize the plasma, helping to interrupt the electrical fault.<a class="footnote-ref" id="fnref:66" href="#fn:66"><sup>66</sup></a> </p> <h3>Medical</h3> <p class="note">See also: <a href="/facts/Boric_acid_(vaginal)/Wj2ygPwQ">Boric acid (vaginal)</a></p> <p>Boric acid can be used as an <a href="/facts/Antiseptic/ua05WK9M">antiseptic</a> for minor burns or cuts and is sometimes used in salves and <a href="/facts/Medical_dressing/ujJX6p2n">dressings</a>, such as <a href="/facts/Boracic_lint/QC7c3SjI">boracic lint</a>. Boric acid is applied in a very dilute solution as an eye wash. Boric acid <a href="/facts/Intravaginal_administration/kIwGRMDf">vaginal suppositories</a> can be used for recurrent <a href="/facts/Candidiasis/gklGEfuq">candidiasis</a> due to non-albicans candida as a second line treatment when conventional treatment has failed.<a class="footnote-ref" id="fnref:67" href="#fn:67"><sup>67</sup></a><a class="footnote-ref" id="fnref:68" href="#fn:68"><sup>68</sup></a> It is less effective than conventional treatment overall.<a class="footnote-ref" id="fnref:69" href="#fn:69"><sup>69</sup></a> Boric acid largely spares <a href="/facts/Lactobacilli/uKhIxU67">lactobacilli</a> within the vagina.<a class="footnote-ref" id="fnref:70" href="#fn:70"><sup>70</sup></a> As <a href="/facts/TOL-463/QYSyMvmw">TOL-463</a>, it is under development as an <a href="/facts/Vaginal_administration/kIwGRMDf">intravaginal</a> medication for the treatment for <a href="/facts/Vulvovaginal_candidiasis/vcrTlo0C">vulvovaginal candidiasis</a>.<a class="footnote-ref" id="fnref:71" href="#fn:71"><sup>71</sup></a><a class="footnote-ref" id="fnref:72" href="#fn:72"><sup>72</sup></a><a class="footnote-ref" id="fnref:73" href="#fn:73"><sup>73</sup></a> </p><p>As an <a href="/facts/Antibacterial/sF1kIfxg">antibacterial</a> compound, boric acid can also be used as an <a href="/facts/Acne/TKJxhHSd">acne</a> treatment. It is also used as a prevention of <a href="/facts/Athlete%2527s_foot/PdCHxFTx">athlete's foot</a>, by inserting powder in the socks or stockings. Various preparations can be used to treat some kinds of <i><a href="/facts/Otitis_externa/NhjVqRWT">otitis externa</a></i> (ear infection) in both humans and animals.<a class="footnote-ref" id="fnref:74" href="#fn:74"><sup>74</sup></a> The preservative in <a href="/facts/Urine/oNUYVtvX">urine</a> sample bottles in the UK is boric acid.<a class="footnote-ref" id="fnref:75" href="#fn:75"><sup>75</sup></a> </p><p>Boric acid solutions used as an eye wash or on abraded skin are known to be toxic, particularly to infants, especially after repeated use; this is because of its slow elimination rate.<a class="footnote-ref" id="fnref:76" href="#fn:76"><sup>76</sup></a> </p><p>Boric acid is one of the most commonly used substances that can counteract the harmful effects of reactive <a href="/facts/Hydrofluoric_acid/wdXqu4bE">hydrofluoric acid</a> (HF) after accidental contact with the skin. It works by forcing the free F− anions into the inert <a href="/facts/Tetrafluoroborate/46EEToo6">tetrafluoroborate</a> anion. This process defeats the extreme toxicity of hydrofluoric acid, particularly its ability to <a href="/facts/Chelation/4G79sXBB">sequester</a> <a href="/facts/Calcium_in_biology/wgUxKej5">ionic calcium</a> from <a href="/facts/Serum_(blood)/a22tvug9">blood serum</a> which can lead to <a href="/facts/Cardiac_arrest/HIAm9AWX">cardiac arrest</a> and bone decomposition; such an event can occur from just minor skin contact with HF.<a class="footnote-ref" id="fnref:77" href="#fn:77"><sup>77</sup></a> </p> <h3>Insecticidal</h3> <p>Boric acid was first registered in the US as an insecticide in 1948 for control of <a href="/facts/Cockroach/mKJP7W6j">cockroaches</a>, <a href="/facts/Termite/KRFbDumW">termites</a>, <a href="/facts/Fire_ant/lnATxBTs">fire ants</a>, <a href="/facts/Flea/hFLUFK24">fleas</a>, <a href="/facts/Silverfish/8sFsWdka">silverfish</a>, and many other <a href="/facts/Insect/IgDNvnUL">insects</a>. The product is generally considered safe in household kitchens to control cockroaches and ants. It acts as a stomach poison affecting the insects' <a href="/facts/Metabolism/WxDrm8k5">metabolism</a>. The dry powder is <a href="/facts/Abrasive/UJ9TvVMx">abrasive</a> to the insects' <a href="/facts/Exoskeleton/Wlmru4GW">exoskeletons</a>.<a class="footnote-ref" id="fnref:78" href="#fn:78"><sup>78</sup></a><a class="footnote-ref" id="fnref:79" href="#fn:79"><sup>79</sup></a><a class="footnote-ref" id="fnref:80" href="#fn:80"><sup>80</sup></a> It is in non-specific <a href="/facts/Insecticide_Resistance_Action_Committee/j72wrfn1">IRAC</a> group 8D. Boric acid is also known as "the gift that keeps on killing" because cockroaches cross over lightly dusted areas and do not die immediately. Still, the effect is like shards of glass cutting them apart. This often allows a cockroach to return to the nest, where it soon dies. Cockroaches, being <a href="/facts/Cannibalism_(zoology)/eKhe7wT9">cannibalistic</a>, eat others killed by contact or consumption of boric acid, consuming the powder trapped in the dead roach and killing them, too. </p><p>Boric acid is also widely used in wood treatment to protect against termites. The full complexity of its mechanism is not fully understood. Still, aside from causing dose-dependent mortality, boric acid causes <a href="/facts/Dysbiosis/nq80zc9d">dysbiosis</a> in the <a href="/facts/Reticulitermes_flavipes/9J1ULo7l">Eastern Subterranean termite</a>, leading to the opportunistic rise of insect pathogens that could be contributing to mortality.<a class="footnote-ref" id="fnref:81" href="#fn:81"><sup>81</sup></a> In Japan the practice of laying newspapers treated with o-boric acid and borax under buildings has been effective in controlling <a href="/facts/Coptotermes_formosanus/HufUHaBd">Coptotermes formosanus</a> and <a href="/facts/Reticulitermes_speratus/8G1xpTNR">Reticulitermes speratus</a> populations. Decaying wood treated with 0.25 to 0.5 percent <a href="/facts/Disodium_octaborate/abzmWugc">disodium octaborate</a> (Na2B8O13·4H2O, commonly abbreviated DOT) is also effective for baiting <a href="/facts/Heterotermes_aureus/Y2EfxI4Y">Heterotermes aureus</a> populations. A 1997 paper concluded: "Borate baits would undoubtedly be helpful in the long-term, but do not appear sufficient as a sole method of structural protection."<a class="footnote-ref" id="fnref:82" href="#fn:82"><sup>82</sup></a> </p> <h3>Preservation</h3> <p>In combination with its use as an insecticide, boric acid also prevents and destroys existing wet and dry rot in timbers. It can be used in combination with an <a href="/facts/Ethylene_glycol/stFz6CVe">ethylene glycol</a> carrier to treat external wood against fungal and insect attack. It is possible to buy borate-impregnated rods for insertion into wood via drill holes where dampness and moisture are known to collect and sit. It is available in a gel form and injectable paste form for treating rot-affected wood without replacing the timber. Concentrates of borate-based treatments can be used to prevent slime, mycelium, and algae growth, even in marine environments. </p><p>Boric acid is added to salt in the curing of cattle hides, <a href="/facts/Calfskin/wNjUFSsL">calfskins</a>, and <a href="/facts/Sheepskin/wQzEsDLY">sheepskins</a>. This helps to control bacterial development and insects. </p> <h3>pH buffer</h3> <p>Boric acid in equilibrium with its conjugate base the borate ion is widely used (in the concentration range 50–100 ppm boron equivalents) as a primary or adjunct pH buffer system in <a href="/facts/Swimming_pools/32DUFtdN">swimming pools</a>. Boric acid is a weak acid, with p<i>K</i>a (the pH at which buffering is strongest because the free acid and borate ion are in equal concentrations) of 9.24 in pure water at 25 °C. But apparent p<i>K</i>a is substantially lower in swimming pool or ocean waters because of interactions with various other molecules in solution. It will be around 9.0 in a saltwater pool. No matter which form of soluble boron is added, within the acceptable range of pH and boron concentration for swimming pools, boric acid is the predominant form in aqueous solution, as shown in the accompanying figure. The boric acid – borate system can be useful as a primary buffer system (substituting for the <a href="/facts/Bicarbonate/zzSVVAl1">bicarbonate</a> system with p<i>K</i>a1 = 6.0 and p<i>K</i>a2 = 9.4 under typical salt-water pool conditions) in pools with salt-water chlorine generators that tend to show upward drift in pH from a working range of pH 7.5–8.2. <a href="/facts/Buffer_capacity/zrLz9eaa">Buffer capacity</a> is greater against rising pH (towards the pKa around 9.0), as illustrated in the accompanying graph. The use of boric acid in this concentration range does not allow any reduction in free <a href="/facts/Hypochlorous_acid/tGrX1C7z">HOCl</a> concentration needed for pool sanitation. Still, it may add marginally to the photo-protective effects of <a href="/facts/Cyanuric_acid/KSmuJvtB">cyanuric acid</a> and confer other benefits through anti-corrosive activity or perceived water softness, depending on overall pool solute composition.<a class="footnote-ref" id="fnref:83" href="#fn:83"><sup>83</sup></a> </p> <h3>Lubrication</h3> <p>Colloidal suspensions of nanoparticles of boric acid dissolved in petroleum or vegetable oil can form a remarkable lubricant on ceramic or metal surfaces<a class="footnote-ref" id="fnref:84" href="#fn:84"><sup>84</sup></a> with a coefficient of sliding friction that decreases with increasing pressure to a value ranging from 0.10 to 0.02. Self-lubricating B(OH)3 films result from a spontaneous chemical reaction between water molecules and B2O3 coatings in a humid environment. On a bulk scale, an inverse relationship exists between the friction coefficient and the Hertzian contact pressure induced by the applied load. </p><p>Boric acid is used to lubricate <a href="/facts/Carrom/5ERJjNNc">carrom</a> and <a href="/facts/Novuss/fuF6lESC">novuss</a> boards, allowing for faster play.<a class="footnote-ref" id="fnref:85" href="#fn:85"><sup>85</sup></a> </p> <h3>Nuclear power</h3> <p>Boric acid is used in some <a href="/facts/Nuclear_power_plant/IJj5pJUn">nuclear power plants</a> as a <a href="/facts/Neutron_poison/bkruR3yz">neutron poison</a>. The boron in boric acid reduces the probability of <a href="/facts/Nuclear_fission/LfkIylvm">thermal fission</a> by absorbing some <a href="/facts/Thermal_neutron/UMKR4XgJ">thermal neutrons</a>. <a href="/facts/Nuclear_chain_reaction/3l0lHBM4">Fission chain reactions</a> are generally driven by the probability that free neutrons will result in fission and is determined by the material and geometric properties of the reactor. Natural boron consists of approximately 20% boron-10 and 80% boron-11 isotopes. Boron-10 has a high <a href="/facts/Nuclear_cross_section/AtghNytD">cross-section</a> for absorption of low-energy (thermal) neutrons. By increasing boric acid concentration in the reactor coolant, the probability that a neutron will cause fission is reduced. Changes in boric acid concentration can effectively regulate the rate of fission taking place in the reactor. During normal at power operation, boric acid is used only in <a href="/facts/Pressurized_water_reactor/2hSL4Hv0">pressurized water reactors</a> (PWRs), whereas <a href="/facts/Boiling_water_reactor/nc0lJKTS">boiling water reactors</a> (BWRs) employ <a href="/facts/Control_rod/VvMTweU5">control rod</a> pattern and coolant flow for power control. However, BWRs can use an aqueous solution of boric acid and <a href="/facts/Borax/IQrXRJ3N">borax</a> or <a href="/facts/Sodium_pentaborate/qptVAgTQ">sodium pentaborate</a> for an emergency shutdown system if the control rods fail to insert. Boric acid may be dissolved in <a href="/facts/Spent_fuel_pool/WIzyHf4B">spent fuel pools</a> used to store <a href="/facts/Spent_nuclear_fuel/jWDWvJ6d">spent fuel</a> elements. The concentration is high enough to keep neutron multiplication at a minimum. Boric acid was dumped over Reactor 4 of the <a href="/facts/Chernobyl_disaster/mNj9JHyf">Chernobyl</a> nuclear power plant after its <a href="/facts/Nuclear_meltdown/ISGm78Mv">meltdown</a> to prevent another reaction from occurring. </p> <h3>Pyrotechnics</h3> <p>Boron is used in <a href="/facts/Pyrotechnics/Gocs5Gcu">pyrotechnics</a> to prevent the <a href="/facts/Amide/C6kCzYEA">amide</a>-forming reaction between <a href="/facts/Aluminium/7wmR8jYE">aluminium</a> and <a href="/facts/Nitrate/5AnVlYnL">nitrates</a>. A small amount of boric acid is added to the composition to neutralize alkaline amides that can react with the aluminium. </p><p>Boric acid can be used as a colorant to make fire green. For example, when dissolved in <a href="/facts/Methanol/EIfpoNCg">methanol</a>, it is popularly used by <a href="/facts/Torch_(juggling)/SGJUdYW3">fire jugglers</a> and fire spinners to create a deep green flame much stronger than copper sulfate.<a class="footnote-ref" id="fnref:86" href="#fn:86"><sup>86</sup></a> </p> <h3>Agriculture</h3> <p>Boric acid is used to treat or prevent <a href="/facts/Boron_deficiency_(plant_disorder)/l3l6x0zm">boron deficiencies</a> in plants. It is also used in the preservation of grains such as rice and wheat.<a class="footnote-ref" id="fnref:87" href="#fn:87"><sup>87</sup></a> </p> <h2 id="further-reading">Further reading</h2> <ul><li>Jolly, W. L. (1991). <i>Modern Inorganic Chemistry</i> (2nd ed.). New York: McGraw-Hill. <a href="/facts/ISBN_(identifier)/15AdSPa9">ISBN</a> 978-0-07-112651-9.</li> <li>Goodman, L.; Gilman, A.; Brunton, L.; Lazo, J.; Parker, K. (2006). <i>Goodman & Gilman's The Pharmacological Basis of Therapeutics</i>. New York: McGraw Hill.</li> <li>Cordia, J.A., Bal, E.A., Mak, W.A. and Wils, E.R.J. (2003). <i>Determination of some physico-chemical properties of Optibor</i> EP. Rijswijk, The Netherlands: TNO Prins Maurits Laboratory, report PML 2002-C42rr, GLP, Unpublished, confidential data provided by Borax Europe Limited.</li></ul> <h2 id="external-links">External links</h2> <ul><li> Media related to Boric acid at Wikimedia Commons</li> <li><a href="http://npic.orst.edu/factsheets/archive/borictech.pdf">Boric Acid Technical Fact Sheet – National Pesticide Information Center</a></li> <li><a href="http://npic.orst.edu/factsheets/boricgen.pdf">Boric Acid General Fact Sheet – National Pesticide Information Center</a></li> <li><a href="http://www.inchem.org/documents/icsc/icsc/eics0991.htm">International Chemical Safety Card 0991</a></li> <li><a href="https://web.archive.org/web/20080406065032/http://www.epa.gov/oppsrrd1/REDs/factsheets/0024fact.pdf">US EPA Pesticide Reregistration Eligibility Decision</a></li> <li><a href="https://web.archive.org/web/20060209040519/http://www.npi.gov.au/database/substance-info/profiles/15.html">National Pollutant Inventory – Boron and compounds</a></li> <li><a href="https://web.archive.org/web/20021212234630/http://www.chemicalland21.com/arokorhi/industrialchem/inorganic/BORIC%20ACID.htm">Boric acid at ChemicalLand21</a></li> <li><a href="https://web.archive.org/web/20100401084438/http://echa.europa.eu/doc/press/pr_10_03_svhc_consultation_20100308.pdf">European Chemicals Agency (ECHA) "New Public Consultation on Eight Potential Substances of Very High Concern" – includes Boric Acid. Closes 22 April 2010</a></li> <li><a href="http://chemsub.online.fr/name/Boric_acid.html">ChemSub Online: Boric acid</a></li></ul> <h2 id="references">References</h2> <ol> <li id="fn:1"><p>Entry "boracic acid" in the online Merriamm-Webster Dictionary. Gives the first use as 1790. Retrieved 2022-06-24. <a href="https://www.merriam-webster.com/dictionary/boracic%20acid" target="_blank">https://www.merriam-webster.com/dictionary/boracic%20acid</a> <a href="#fnref:1" class="footnote-back-ref">↩</a></p></li> <li id="fn:2"><p>Ronald Eisler (2007). Eisler's Encyclopedia of Environmentally Hazardous Priority Chemicals. Elsevier. p. 59. ISBN 978-0-08-054707-7. <a href="978-0-08-054707-7" target="_blank">978-0-08-054707-7</a> <a href="#fnref:2" class="footnote-back-ref">↩</a></p></li> <li id="fn:3"><p>Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. p. 1291. ISBN 978-0-08-037941-8. <a href="978-0-08-037941-8" target="_blank">978-0-08-037941-8</a> <a href="#fnref:3" class="footnote-back-ref">↩</a></p></li> <li id="fn:4"><p>Andrei Rotaru (2017): "Thermal and kinetic study of hexagonal boric acid versus triclinic boric acid in air flow." Journal of Thermal Analysis and Calorimetry, volume 127, pages 755–763. doi:10.1007/s10973-016-5583-7 <a href="/wiki/Doi_(identifier)" target="_blank">/wiki/Doi_(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>Gajhede, M.; Larsen, S.; Rettrup, S. (1 December 1986). "Electron density of orthoboric acid determined by X-ray diffraction at 105 K and ab initio calculations". Acta Crystallographica Section B Structural Science. 42 (6): 545–552. Bibcode:1986AcCrB..42..545G. doi:10.1107/S0108768186097720. <a href="https://www.crystallography.net/cod/9007675.html" target="_blank">https://www.crystallography.net/cod/9007675.html</a> <a href="#fnref:6" class="footnote-back-ref">↩</a></p></li> <li id="fn:7"><p>Shuvalov, Robert R.; Burns, Peter C. (15 June 2003). "A new polytype of orthoboric acid, H 3 BO 3 -3 T". Acta Crystallographica Section C Crystal Structure Communications. 59 (6): i47 – i49. Bibcode:2003AcCrC..59I..47S. doi:10.1107/S0108270103009685. PMID 12794317. <a href="/wiki/Bibcode_(identifier)" target="_blank">/wiki/Bibcode_(identifier)</a> <a href="#fnref:7" class="footnote-back-ref">↩</a></p></li> <li id="fn:8"><p>Housecroft, C. E.; Sharpe, A. G. (2008). "Chapter 13: The Group 13 Elements". Inorganic Chemistry (3rd ed.). Pearson. p. 340. ISBN 978-0-13-175553-6. <a href="978-0-13-175553-6" target="_blank">978-0-13-175553-6</a> <a href="#fnref:8" class="footnote-back-ref">↩</a></p></li> <li id="fn:9"><p>Gurwinder Kaur, Shagun Kainth, Rohit Kumar, Piyush Sharma and O. P. Pandey (2021): "Reaction kinetics during non-isothermal solid-state synthesis of boron trioxide via boric acid dehydration." Reaction Kinetics, Mechanisms and Catalysis, volume 134, pages 347–359. doi:10.1007/s11144-021-02084-8 <a href="/wiki/Doi_(identifier)" target="_blank">/wiki/Doi_(identifier)</a> <a href="#fnref:9" class="footnote-back-ref">↩</a></p></li> <li id="fn:10"><p>Siavash Aghili, Masoud Panjepour, and Mahmood Meratian (2018): "Kinetic analysis of formation of boron trioxide from thermal decomposition of boric acid under non-isothermal conditions." Journal of Thermal Analysis and Calorimetry, volume 131, pages 2443–2455. doi:10.1007/s10973-017-6740-3 <a href="/wiki/Doi_(identifier)" target="_blank">/wiki/Doi_(identifier)</a> <a href="#fnref:10" class="footnote-back-ref">↩</a></p></li> <li id="fn:11"><p>Gurwinder Kaur, Shagun Kainth, Rohit Kumar, Piyush Sharma and O. P. Pandey (2021): "Reaction kinetics during non-isothermal solid-state synthesis of boron trioxide via boric acid dehydration." Reaction Kinetics, Mechanisms and Catalysis, volume 134, pages 347–359. doi:10.1007/s11144-021-02084-8 <a href="/wiki/Doi_(identifier)" target="_blank">/wiki/Doi_(identifier)</a> <a href="#fnref:11" class="footnote-back-ref">↩</a></p></li> <li id="fn:12"><p>Siavash Aghili, Masoud Panjepour, and Mahmood Meratian (2018): "Kinetic analysis of formation of boron trioxide from thermal decomposition of boric acid under non-isothermal conditions." Journal of Thermal Analysis and Calorimetry, volume 131, pages 2443–2455. doi:10.1007/s10973-017-6740-3 <a href="/wiki/Doi_(identifier)" target="_blank">/wiki/Doi_(identifier)</a> <a href="#fnref:12" class="footnote-back-ref">↩</a></p></li> <li id="fn:13"><p>Balci, Suna; Sezgi, Naime; Eren, Esin (2012). "Boron Oxide Production Kinetics Using Boric Acid as Raw Material". Industrial & Engineering Chemistry Research. 51 (34): 11091–11096. doi:10.1021/ie300685x. <a href="/wiki/Doi_(identifier)" target="_blank">/wiki/Doi_(identifier)</a> <a href="#fnref:13" class="footnote-back-ref">↩</a></p></li> <li id="fn:14"><p>Gurwinder Kaur, Shagun Kainth, Rohit Kumar, Piyush Sharma and O. P. Pandey (2021): "Reaction kinetics during non-isothermal solid-state synthesis of boron trioxide via boric acid dehydration." 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