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   <data>
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   <supplemental></supplemental>
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  <points>
   <conditions>
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    <unit>$\pu{K}$</unit>
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    <unit>mol/kg</unit>
   </data>
   <data>
    <exponent>0</exponent>
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    <unit>mol/kg</unit>
   </data>
   <data>
    <exponent>0</exponent>
    <number>1.2987e+00</number>
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    <sigfigs>5</sigfigs>
    <significand>1.2987</significand>
    <unit>g/cm&lt;sup&gt;3&lt;/sup&gt;</unit>
   </data>
   <data>
    <exponent>0</exponent>
    <number>1.22e+00</number>
    <property>Activity Coefficent</property>
    <sigfigs>3</sigfigs>
    <significand>1.22</significand>
    <unit>1</unit>
   </data>
   <pntnum>26</pntnum>
   <supplemental></supplemental>
  </points>
  <series>1</series>
 </dataset>
 <keywords>Solubility, Solubility data series</keywords>
 <method>Either pure $\ce{CO2}$ gas or $\ce{CO2}-\ce{N2}$ mixtures were used in the experiments to maintain a constant P($\ce{CO2}$). The $\ce{CO2}-\ce{N2}$ mixtures were made by pumping predetermined amounts of $\ce{CO2}$ and $\ce{N2}$ into a gas tank and their composition was verified by gas chromatography.&lt;br/&gt;$\ce{CO2}$ or $\ce{CO2}-\ce{N2}$ gas mixtures were equilibrated with the aqueous solutions in a series of stirred water-jacketed reaction vessels with condensers. The gas was pre-moistured by first passing it through distilled water at the temperature of experiment. Fine bubbles were obtained by using gas-dispersion tubes. The bubbling rate was 90-95 mL/min.&lt;br/&gt;The mole fraction of $\ce{CO2}$ in the $\ce{CO2}-\ce{N2}$ mixture was determined using a Hewlett Packard (5790A) gas chromatograph.</method>
 <publisher>The International Union of Pure and Applied Chemistry</publisher>
 <sources>
  <citation>He, S.; Morse, J. W.; Geochim. Cosmochim. Acta 1993, 57, 3533-54.</citation>
  <pubtype>paper</pubtype>
  <url>https://doi.org/10.1016/0016-7037(93)90137-l </url>
 </sources>
 <substances>
  <casrn>124-38-9</casrn>
  <constituent>1</constituent>
  <formula>CO2</formula>
  <inchi>InChI=1S/CO2/c2-1-3</inchi>
  <inchikey>CURLTUGMZLYLDI-UHFFFAOYSA-N</inchikey>
  <molweight>44.0095</molweight>
  <name>Carbon dioxide</name>
  <sample>Commercial; purity 99.9%</sample>
 </substances>
 <substances>
  <casrn>10043-52-4</casrn>
  <constituent>2</constituent>
  <formula>CaCl2</formula>
  <inchi>InChI=1S/Ca.2ClH/h;2*1H/q+2;;/p-2</inchi>
  <inchikey>UXVMQQNJUSDDNG-UHFFFAOYSA-L</inchikey>
  <molweight>110.98</molweight>
  <name>Calcium chloride</name>
  <sample>Source not mentioned. Analytical reagent-grade which met ACS specifications. $\ce{CaCl2.2H2O}$ was weighed and dissolved in water. The concentration of $\ce{CaCl2}$ in solutions was determined by analyzing $\ce{Cl^{-}}$ concentration via $\ce{AgNO3}$ titration in stock solutions.</sample>
 </substances>
 <substances>
  <casrn>7732-18-5</casrn>
  <constituent>3</constituent>
  <formula>H2O</formula>
  <inchi>InChI=1S/H2O/h1H2</inchi>
  <inchikey>XLYOFNOQVPJJNP-UHFFFAOYSA-N</inchikey>
  <molweight>18.0153</molweight>
  <name>Water</name>
  <sample>18 M&amp;#937; water obtained from a Milli-Q Super-Q water system.</sample>
 </substances>
 <system>Carbon dioxide with Calcium chloride and Water</system>
 <title>Solubility data from IUPAC SDS Volume 62 (page ?) - Carbon dioxide with Calcium chloride and Water</title>
</compilation>