unit:PH

URI: http://qudt.org/vocab/unit/PH

Type
Description

In chemistry the unit $\textit{pH}$, also referred to as $\textit{acidity}$ or $\textit{basicity}$, is the negative logarithm (base 10) of the concentration of free protons (or hydronium ions). The definition of $pH$ in terms of hydrogen ions in solution is: $$\text{pH}=-\log_{10}(a_{H^+})\equiv-\log_{10}\left(\left[H^+\right]\right)$$ Where $a_{H^+}$ is the equilibrium molar concentration of $H^+$ in the solution, the activity of the hydrogen ion in the solution. $$$$ This definition is appropriate for concentrations equal to, or less than $1\ mol/l$, where $aH+ \equiv [H+]$, that is, $1\ mol/L\ HCl$ has a $pH$ of zero. $$$$ To relate this to standard molality ($b^\circ$), typically taken as $1 \ mol/kg$, consideration is given to the activity ($a_{H^+}$) of the hydrogen ions. $$$$ The activity can be expressed as: $$a_{H^+} = \gamma_{H^+} \times m_{H^+}$$ Where, $\gamma_{H^+}$ is the activity coefficient, which adjusts the molality to account for non-ideal behavior due to interactions between ions in the solution. $m_{H^+}$ is the molality of hydrogen ions in the solution relative to the standard molality, expressed in $mol/kg$. $$$$ The expansion of $pH$ then becomes: $$\text{pH} = -log_{10}\left(m_{H+}\times\gamma_{H^+}\right)$$ $$$$ This definition is relevant in more concentrated solutions or when precise thermodynamic calculations are required. It reflects how the properties of the solution deviate from ideal behavior and provides a more accurate understanding of the $pH$ under various conditions. $$$$ While $pH$ is a universally recognized scale for expressing hydrogen ion activity, its appropriateness and accuracy can diminish under conditions of extremely high ionic strength, non-aqueous environments, high temperatures, or very high or low $pH$ values. In such cases, alternative measurement strategies might be required to obtain meaningful and accurate descriptions of acidity or basicity.

Properties
qudt:applicableSystem
qudt:hasDimensionVector
qudt:hasQuantityKind
qudt:symbol
pH
rdf:type
qudt:ucumCode
[pH]
Annotations
rdfs:comment
Unsure about dimensionality of pH; conversion requires a log function not just a multiplier(en)
dcterms:description
In chemistry the unit $\textit{pH}$, also referred to as $\textit{acidity}$ or $\textit{basicity}$, is the negative logarithm (base 10) of the concentration of free protons (or hydronium ions). The definition of $pH$ in terms of hydrogen ions in solution is: $$\text{pH}=-\log_{10}(a_{H^+})\equiv-\log_{10}\left(\left[H^+\right]\right)$$ Where $a_{H^+}$ is the equilibrium molar concentration of $H^+$ in the solution, the activity of the hydrogen ion in the solution. $$$$ This definition is appropriate for concentrations equal to, or less than $1\ mol/l$, where $aH+ \equiv [H+]$, that is, $1\ mol/L\ HCl$ has a $pH$ of zero. $$$$ To relate this to standard molality ($b^\circ$), typically taken as $1 \ mol/kg$, consideration is given to the activity ($a_{H^+}$) of the hydrogen ions. $$$$ The activity can be expressed as: $$a_{H^+} = \gamma_{H^+} \times m_{H^+}$$ Where, $\gamma_{H^+}$ is the activity coefficient, which adjusts the molality to account for non-ideal behavior due to interactions between ions in the solution. $m_{H^+}$ is the molality of hydrogen ions in the solution relative to the standard molality, expressed in $mol/kg$. $$$$ The expansion of $pH$ then becomes: $$\text{pH} = -log_{10}\left(m_{H+}\times\gamma_{H^+}\right)$$ $$$$ This definition is relevant in more concentrated solutions or when precise thermodynamic calculations are required. It reflects how the properties of the solution deviate from ideal behavior and provides a more accurate understanding of the $pH$ under various conditions. $$$$ While $pH$ is a universally recognized scale for expressing hydrogen ion activity, its appropriateness and accuracy can diminish under conditions of extremely high ionic strength, non-aqueous environments, high temperatures, or very high or low $pH$ values. In such cases, alternative measurement strategies might be required to obtain meaningful and accurate descriptions of acidity or basicity.
qudt:informativeReference
rdfs:isDefinedBy
rdfs:label
Acidity(en)
View as:  CSV

Work in progress

RDF/XML 
<rdf:RDF
    xmlns:rdf="http://www.w3.org/1999/02/22-rdf-syntax-ns#"
    xmlns:j.0="http://qudt.org/schema/qudt/"
    xmlns:j.1="http://purl.org/dc/terms/"
    xmlns:owl="http://www.w3.org/2002/07/owl#"
    xmlns:rdfs="http://www.w3.org/2000/01/rdf-schema#"
    xmlns:xsd="http://www.w3.org/2001/XMLSchema#" > 
  <rdf:Description rdf:about="http://qudt.org/vocab/unit/PH">
    <rdfs:isDefinedBy rdf:resource="http://qudt.org/2.1/vocab/unit"/>
    <j.0:informativeReference rdf:datatype="http://www.w3.org/2001/XMLSchema#anyURI">https://iupac.org/wp-content/uploads/2019/05/IUPAC-GB3-2012-2ndPrinting-PDFsearchable.pdf</j.0:informativeReference>
    <j.0:applicableSystem rdf:resource="http://qudt.org/vocab/sou/ASU"/>
    <j.0:ucumCode rdf:datatype="http://qudt.org/schema/qudt/UCUMcs">[pH]</j.0:ucumCode>
    <rdfs:label xml:lang="en">Acidity</rdfs:label>
    <j.0:hasQuantityKind rdf:resource="http://qudt.org/vocab/quantitykind/Basicity"/>
    <j.0:applicableSystem rdf:resource="http://qudt.org/vocab/sou/CGS-EMU"/>
    <j.0:hasQuantityKind rdf:resource="http://qudt.org/vocab/quantitykind/Acidity"/>
    <j.0:symbol>pH</j.0:symbol>
    <j.0:applicableSystem rdf:resource="http://qudt.org/vocab/sou/CGS-ESU"/>
    <j.1:description rdf:datatype="http://qudt.org/schema/qudt/LatexString">
  In chemistry the unit $\textit{pH}$, also referred to as $\textit{acidity}$ or $\textit{basicity}$,
   is the negative logarithm (base 10) of the concentration of free protons (or hydronium ions).
  The definition of $pH$ in terms of hydrogen ions in solution is:

  $$\text{pH}=-\log_{10}(a_{H^+})\equiv-\log_{10}\left(\left[H^+\right]\right)$$

  Where $a_{H^+}$ is the equilibrium molar concentration of $H^+$ in the solution, the activity of
   the hydrogen ion in the solution.
  $$$$
  This definition is appropriate for concentrations equal to, or less than $1\ mol/l$, 
   where $aH+ \equiv [H+]$, that is, $1\ mol/L\ HCl$ has a $pH$ of zero.
  $$$$
  To relate this to standard molality ($b^\circ$), typically taken as $1 \ mol/kg$, 
   consideration is given to the activity ($a_{H^+}$) of the hydrogen ions.
  $$$$
  The activity can be expressed as:

  $$a_{H^+} = \gamma_{H^+} \times m_{H^+}$$ 

  Where, $\gamma_{H^+}$ is the activity coefficient, which adjusts the molality to account for
   non-ideal behavior due to interactions between ions in the solution.
  $m_{H^+}$ is the molality of hydrogen ions in the solution relative to the standard molality, 
   expressed in $mol/kg$.
  $$$$
  The expansion of $pH$ then becomes:

  $$\text{pH} = -log_{10}\left(m_{H+}\times\gamma_{H^+}\right)$$

  $$$$
  This definition is relevant in more concentrated solutions or when precise thermodynamic calculations are required. 
  It reflects how the properties of the solution deviate from ideal behavior and provides a more accurate understanding of the $pH$ under various conditions.
  $$$$
  While $pH$ is a universally recognized scale for expressing hydrogen ion activity,
  its appropriateness and accuracy can diminish under conditions of extremely high
  ionic strength, non-aqueous environments, high temperatures, or very high or low $pH$ values.
  In such cases, alternative measurement strategies might be required to obtain meaningful and accurate descriptions of acidity or basicity.
  </j.1:description>
    <rdf:type rdf:resource="http://qudt.org/schema/qudt/Unit"/>
    <j.0:applicableSystem rdf:resource="http://qudt.org/vocab/sou/SI"/>
    <j.0:hasDimensionVector rdf:resource="http://qudt.org/vocab/dimensionvector/A0E0L0I0M0H0T0D1"/>
    <j.0:applicableSystem rdf:resource="http://qudt.org/vocab/sou/IMPERIAL"/>
    <j.0:applicableSystem rdf:resource="http://qudt.org/vocab/sou/CGS-GAUSS"/>
    <j.0:applicableSystem rdf:resource="http://qudt.org/vocab/sou/PLANCK"/>
    <rdfs:comment xml:lang="en">Unsure about dimensionality of pH; conversion requires a log function not just a multiplier</rdfs:comment>
    <j.0:applicableSystem rdf:resource="http://qudt.org/vocab/sou/CGS"/>
  </rdf:Description>
</rdf:RDF>
TURTLE 
@prefix owl: <http://www.w3.org/2002/07/owl#> .
@prefix rdf: <http://www.w3.org/1999/02/22-rdf-syntax-ns#> .
@prefix rdfs: <http://www.w3.org/2000/01/rdf-schema#> .
@prefix xsd: <http://www.w3.org/2001/XMLSchema#> .

<http://qudt.org/vocab/unit/PH>
  rdf:type <http://qudt.org/schema/qudt/Unit> ;
  <http://purl.org/dc/terms/description> """
  In chemistry the unit $\\textit{pH}$, also referred to as $\\textit{acidity}$ or $\\textit{basicity}$,
   is the negative logarithm (base 10) of the concentration of free protons (or hydronium ions).
  The definition of $pH$ in terms of hydrogen ions in solution is:

  $$\\text{pH}=-\\log_{10}(a_{H^+})\\equiv-\\log_{10}\\left(\\left[H^+\\right]\\right)$$

  Where $a_{H^+}$ is the equilibrium molar concentration of $H^+$ in the solution, the activity of
   the hydrogen ion in the solution.
  $$$$
  This definition is appropriate for concentrations equal to, or less than $1\\ mol/l$, 
   where $aH+ \\equiv [H+]$, that is, $1\\ mol/L\\ HCl$ has a $pH$ of zero.
  $$$$
  To relate this to standard molality ($b^\\circ$), typically taken as $1 \\ mol/kg$, 
   consideration is given to the activity ($a_{H^+}$) of the hydrogen ions.
  $$$$
  The activity can be expressed as:

  $$a_{H^+} = \\gamma_{H^+} \\times m_{H^+}$$ 

  Where, $\\gamma_{H^+}$ is the activity coefficient, which adjusts the molality to account for
   non-ideal behavior due to interactions between ions in the solution.
  $m_{H^+}$ is the molality of hydrogen ions in the solution relative to the standard molality, 
   expressed in $mol/kg$.
  $$$$
  The expansion of $pH$ then becomes:

  $$\\text{pH} = -log_{10}\\left(m_{H+}\\times\\gamma_{H^+}\\right)$$

  $$$$
  This definition is relevant in more concentrated solutions or when precise thermodynamic calculations are required. 
  It reflects how the properties of the solution deviate from ideal behavior and provides a more accurate understanding of the $pH$ under various conditions.
  $$$$
  While $pH$ is a universally recognized scale for expressing hydrogen ion activity,
  its appropriateness and accuracy can diminish under conditions of extremely high
  ionic strength, non-aqueous environments, high temperatures, or very high or low $pH$ values.
  In such cases, alternative measurement strategies might be required to obtain meaningful and accurate descriptions of acidity or basicity.
  """^^<http://qudt.org/schema/qudt/LatexString> ;
  <http://qudt.org/schema/qudt/applicableSystem> <http://qudt.org/vocab/sou/ASU> ;
  <http://qudt.org/schema/qudt/applicableSystem> <http://qudt.org/vocab/sou/CGS> ;
  <http://qudt.org/schema/qudt/applicableSystem> <http://qudt.org/vocab/sou/CGS-EMU> ;
  <http://qudt.org/schema/qudt/applicableSystem> <http://qudt.org/vocab/sou/CGS-ESU> ;
  <http://qudt.org/schema/qudt/applicableSystem> <http://qudt.org/vocab/sou/CGS-GAUSS> ;
  <http://qudt.org/schema/qudt/applicableSystem> <http://qudt.org/vocab/sou/IMPERIAL> ;
  <http://qudt.org/schema/qudt/applicableSystem> <http://qudt.org/vocab/sou/PLANCK> ;
  <http://qudt.org/schema/qudt/applicableSystem> <http://qudt.org/vocab/sou/SI> ;
  <http://qudt.org/schema/qudt/hasDimensionVector> <http://qudt.org/vocab/dimensionvector/A0E0L0I0M0H0T0D1> ;
  <http://qudt.org/schema/qudt/hasQuantityKind> <http://qudt.org/vocab/quantitykind/Acidity> ;
  <http://qudt.org/schema/qudt/hasQuantityKind> <http://qudt.org/vocab/quantitykind/Basicity> ;
  <http://qudt.org/schema/qudt/informativeReference> "https://iupac.org/wp-content/uploads/2019/05/IUPAC-GB3-2012-2ndPrinting-PDFsearchable.pdf"^^xsd:anyURI ;
  <http://qudt.org/schema/qudt/symbol> "pH" ;
  <http://qudt.org/schema/qudt/ucumCode> "[pH]"^^<http://qudt.org/schema/qudt/UCUMcs> ;
  rdfs:comment "Unsure about dimensionality of pH; conversion requires a log function not just a multiplier"@en ;
  rdfs:isDefinedBy <http://qudt.org/2.1/vocab/unit> ;
  rdfs:label "Acidity"@en ;
.
JSON 
{"resource":"Acidity" 
 ,"qname":"unit:PH" 
 ,"uri":"http:\/\/qudt.org\/vocab\/unit\/PH" 
 ,"properties":["applicable system":"sou:ASU" 
    ,"applicable system":"sou:CGS" 
    ,"applicable system":"sou:CGS-EMU" 
    ,"applicable system":"sou:CGS-ESU" 
    ,"applicable system":"sou:CGS-GAUSS" 
    ,"applicable system":"sou:IMPERIAL" 
    ,"applicable system":"sou:PLANCK" 
    ,"applicable system":"sou:SI" 
    ,"comment":"Unsure about dimensionality of pH; conversion requires a log function not just a multiplier" 
    ,"description":"\n  In chemistry the unit $\\textit{pH}$, also referred to as $\\textit{acidity}$ or $\\textit{basicity}$,\n   is the negative logarithm (base 10) of the concentration of free protons (or hydronium ions).\n  The definition of $pH$ in terms of hydrogen ions in solution is:\n\n  $$\\text{pH}=-\\log_{10}(a_{H^+})\\equiv-\\log_{10}\\left(\\left[H^+\\right]\\right)$$\n\n  Where $a_{H^+}$ is the equilibrium molar concentration of $H^+$ in the solution, the activity of\n   the hydrogen ion in the solution.\n  $$$$\n  This definition is appropriate for concentrations equal to, or less than $1\\ mol\/l$, \n   where $aH+ \\equiv [H+]$, that is, $1\\ mol\/L\\ HCl$ has a $pH$ of zero.\n  $$$$\n  To relate this to standard molality ($b^\\circ$), typically taken as $1 \\ mol\/kg$, \n   consideration is given to the activity ($a_{H^+}$) of the hydrogen ions.\n  $$$$\n  The activity can be expressed as:\n\n  $$a_{H^+} = \\gamma_{H^+} \\times m_{H^+}$$ \n\n  Where, $\\gamma_{H^+}$ is the activity coefficient, which adjusts the molality to account for\n   non-ideal behavior due to interactions between ions in the solution.\n  $m_{H^+}$ is the molality of hydrogen ions in the solution relative to the standard molality, \n   expressed in $mol\/kg$.\n  $$$$\n  The expansion of $pH$ then becomes:\n\n  $$\\text{pH} = -log_{10}\\left(m_{H+}\\times\\gamma_{H^+}\\right)$$\n\n  $$$$\n  This definition is relevant in more concentrated solutions or when precise thermodynamic calculations are required. \n  It reflects how the properties of the solution deviate from ideal behavior and provides a more accurate understanding of the $pH$ under various conditions.\n  $$$$\n  While $pH$ is a universally recognized scale for expressing hydrogen ion activity,\n  its appropriateness and accuracy can diminish under conditions of extremely high\n  ionic strength, non-aqueous environments, high temperatures, or very high or low $pH$ values.\n  In such cases, alternative measurement strategies might be required to obtain meaningful and accurate descriptions of acidity or basicity.\n  " 
    ,"has dimension vector":"dimension:A0E0L0I0M0H0T0D1" 
    ,"has quantity kind":"quantitykind:Acidity" 
    ,"has quantity kind":"quantitykind:Basicity" 
    ,"informative reference":"https:\/\/iupac.org\/wp-content\/uploads\/2019\/05\/IUPAC-GB3-2012-2ndPrinting-PDFsearchable.pdf" 
    ,"isDefinedBy":"&lt;http:\/\/qudt.org\/2.1\/vocab\/unit&gt;" 
    ,"label":"Acidity" 
    ,"symbol":"pH" 
    ,"type":"qudt:Unit" 
    ,"ucum code":"[pH]" 
    ]}
JSON-LD 
{
  "@id" : "http://qudt.org/vocab/unit/PH",
  "@type" : "http://qudt.org/schema/qudt/Unit",
  "description" : "\n  In chemistry the unit $\\textit{pH}$, also referred to as $\\textit{acidity}$ or $\\textit{basicity}$,\n   is the negative logarithm (base 10) of the concentration of free protons (or hydronium ions).\n  The definition of $pH$ in terms of hydrogen ions in solution is:\n\n  $$\\text{pH}=-\\log_{10}(a_{H^+})\\equiv-\\log_{10}\\left(\\left[H^+\\right]\\right)$$\n\n  Where $a_{H^+}$ is the equilibrium molar concentration of $H^+$ in the solution, the activity of\n   the hydrogen ion in the solution.\n  $$$$\n  This definition is appropriate for concentrations equal to, or less than $1\\ mol/l$, \n   where $aH+ \\equiv [H+]$, that is, $1\\ mol/L\\ HCl$ has a $pH$ of zero.\n  $$$$\n  To relate this to standard molality ($b^\\circ$), typically taken as $1 \\ mol/kg$, \n   consideration is given to the activity ($a_{H^+}$) of the hydrogen ions.\n  $$$$\n  The activity can be expressed as:\n\n  $$a_{H^+} = \\gamma_{H^+} \\times m_{H^+}$$ \n\n  Where, $\\gamma_{H^+}$ is the activity coefficient, which adjusts the molality to account for\n   non-ideal behavior due to interactions between ions in the solution.\n  $m_{H^+}$ is the molality of hydrogen ions in the solution relative to the standard molality, \n   expressed in $mol/kg$.\n  $$$$\n  The expansion of $pH$ then becomes:\n\n  $$\\text{pH} = -log_{10}\\left(m_{H+}\\times\\gamma_{H^+}\\right)$$\n\n  $$$$\n  This definition is relevant in more concentrated solutions or when precise thermodynamic calculations are required. \n  It reflects how the properties of the solution deviate from ideal behavior and provides a more accurate understanding of the $pH$ under various conditions.\n  $$$$\n  While $pH$ is a universally recognized scale for expressing hydrogen ion activity,\n  its appropriateness and accuracy can diminish under conditions of extremely high\n  ionic strength, non-aqueous environments, high temperatures, or very high or low $pH$ values.\n  In such cases, alternative measurement strategies might be required to obtain meaningful and accurate descriptions of acidity or basicity.\n  ",
  "applicableSystem" : [ "http://qudt.org/vocab/sou/ASU", "http://qudt.org/vocab/sou/CGS-EMU", "http://qudt.org/vocab/sou/CGS-ESU", "http://qudt.org/vocab/sou/SI", "http://qudt.org/vocab/sou/IMPERIAL", "http://qudt.org/vocab/sou/CGS-GAUSS", "http://qudt.org/vocab/sou/PLANCK", "http://qudt.org/vocab/sou/CGS" ],
  "hasDimensionVector" : "http://qudt.org/vocab/dimensionvector/A0E0L0I0M0H0T0D1",
  "hasQuantityKind" : [ "http://qudt.org/vocab/quantitykind/Basicity", "http://qudt.org/vocab/quantitykind/Acidity" ],
  "informativeReference" : "https://iupac.org/wp-content/uploads/2019/05/IUPAC-GB3-2012-2ndPrinting-PDFsearchable.pdf",
  "symbol" : "pH",
  "ucumCode" : "[pH]",
  "comment" : {
    "@language" : "en",
    "@value" : "Unsure about dimensionality of pH; conversion requires a log function not just a multiplier"
  },
  "isDefinedBy" : "http://qudt.org/2.1/vocab/unit",
  "label" : {
    "@language" : "en",
    "@value" : "Acidity"
  },
  "@context" : {
    "isDefinedBy" : {
      "@id" : "http://www.w3.org/2000/01/rdf-schema#isDefinedBy",
      "@type" : "@id"
    },
    "informativeReference" : {
      "@id" : "http://qudt.org/schema/qudt/informativeReference",
      "@type" : "http://www.w3.org/2001/XMLSchema#anyURI"
    },
    "applicableSystem" : {
      "@id" : "http://qudt.org/schema/qudt/applicableSystem",
      "@type" : "@id"
    },
    "ucumCode" : {
      "@id" : "http://qudt.org/schema/qudt/ucumCode",
      "@type" : "http://qudt.org/schema/qudt/UCUMcs"
    },
    "label" : {
      "@id" : "http://www.w3.org/2000/01/rdf-schema#label"
    },
    "hasQuantityKind" : {
      "@id" : "http://qudt.org/schema/qudt/hasQuantityKind",
      "@type" : "@id"
    },
    "symbol" : {
      "@id" : "http://qudt.org/schema/qudt/symbol"
    },
    "description" : {
      "@id" : "http://purl.org/dc/terms/description",
      "@type" : "http://qudt.org/schema/qudt/LatexString"
    },
    "hasDimensionVector" : {
      "@id" : "http://qudt.org/schema/qudt/hasDimensionVector",
      "@type" : "@id"
    },
    "comment" : {
      "@id" : "http://www.w3.org/2000/01/rdf-schema#comment"
    },
    "rdf" : "http://www.w3.org/1999/02/22-rdf-syntax-ns#",
    "owl" : "http://www.w3.org/2002/07/owl#",
    "xsd" : "http://www.w3.org/2001/XMLSchema#",
    "rdfs" : "http://www.w3.org/2000/01/rdf-schema#"
  }
}
Generated 2024-12-09T16:41:58.855-05:00 by lmdoc version 1.1 with  TopBraid SPARQL Web Pages (SWP)