<compilation>
 <compilers>H. Lawrence Clever</compilers>
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   </data>
   <pntnum>14</pntnum>
   <supplemental></supplemental>
  </points>
  <points>
   <conditions>
    <exponent>2</exponent>
    <number>3.03e+02</number>
    <property>Ambient temperature</property>
    <sigfigs>3</sigfigs>
    <significand>3.03</significand>
    <unit>$\pu{K}$</unit>
   </conditions>
   <conditions>
    <exponent>1</exponent>
    <number>3.0e+01</number>
    <property>Ambient temperature</property>
    <sigfigs>2</sigfigs>
    <significand>3.0</significand>
    <unit>&amp;deg;C</unit>
   </conditions>
   <conditions>
    <exponent>0</exponent>
    <number>1.311e+00</number>
    <property>Amount concentration (2)</property>
    <sigfigs>4</sigfigs>
    <significand>1.311</significand>
    <unit>mol/L</unit>
   </conditions>
   <data>
    <exponent>0</exponent>
    <number>1.358e+00</number>
    <property>Molality (2)</property>
    <sigfigs>4</sigfigs>
    <significand>1.358</significand>
    <unit>mol/kg</unit>
   </data>
   <data>
    <exponent>1</exponent>
    <number>1.7713e+01</number>
    <property>Percent mass fraction (2)</property>
    <sigfigs>5</sigfigs>
    <significand>1.7713</significand>
    <unit>1</unit>
   </data>
   <data>
    <exponent>-1</exponent>
    <number>3.672e-01</number>
    <property>Bunsen Coefficient</property>
    <sigfigs>4</sigfigs>
    <significand>3.672</significand>
    <unit>$\pu{cm3(g) cm-3(l) atm-1}$</unit>
   </data>
   <data>
    <exponent>0</exponent>
    <number>1.173e+00</number>
    <property>Relative density</property>
    <sigfigs>4</sigfigs>
    <significand>1.173</significand>
    <unit>1</unit>
   </data>
   <pntnum>15</pntnum>
   <supplemental></supplemental>
  </points>
  <points>
   <conditions>
    <exponent>2</exponent>
    <number>3.03e+02</number>
    <property>Ambient temperature</property>
    <sigfigs>3</sigfigs>
    <significand>3.03</significand>
    <unit>$\pu{K}$</unit>
   </conditions>
   <conditions>
    <exponent>1</exponent>
    <number>3.0e+01</number>
    <property>Ambient temperature</property>
    <sigfigs>2</sigfigs>
    <significand>3.0</significand>
    <unit>&amp;deg;C</unit>
   </conditions>
   <conditions>
    <exponent>0</exponent>
    <number>2.643e+00</number>
    <property>Amount concentration (2)</property>
    <sigfigs>4</sigfigs>
    <significand>2.643</significand>
    <unit>mol/L</unit>
   </conditions>
   <data>
    <exponent>0</exponent>
    <number>2.860e+00</number>
    <property>Molality (2)</property>
    <sigfigs>4</sigfigs>
    <significand>2.860</significand>
    <unit>mol/kg</unit>
   </data>
   <data>
    <exponent>1</exponent>
    <number>3.1194e+01</number>
    <property>Percent mass fraction (2)</property>
    <sigfigs>5</sigfigs>
    <significand>3.1194</significand>
    <unit>1</unit>
   </data>
   <data>
    <exponent>-1</exponent>
    <number>2.231e-01</number>
    <property>Bunsen Coefficient</property>
    <sigfigs>4</sigfigs>
    <significand>2.231</significand>
    <unit>$\pu{cm3(g) cm-3(l) atm-1}$</unit>
   </data>
   <data>
    <exponent>0</exponent>
    <number>1.343e+00</number>
    <property>Relative density</property>
    <sigfigs>4</sigfigs>
    <significand>1.343</significand>
    <unit>1</unit>
   </data>
   <pntnum>16</pntnum>
   <supplemental></supplemental>
  </points>
  <series>2</series>
  <title>Strontium chloride; SrCl&lt;sub&gt;2&lt;/sub&gt;; [10476-85-4]</title>
 </dataset>
 <keywords>Solubility, Solubility data series</keywords>
 <method>The apparatus consisted of a bulb of known volume in which the initial pressure and carbon dioxide (reduced to 0 °C) was measured; a bulb of known volume for the solvent; and a manometer system to adjust the final volume of the unabsorbed wet gas and measure its total pressure (reduced to 0 °C). . The final total pressure of wet gas was reduced to the partial pressure of carbon dioxide by subtraction of the solution water vapor pressure.&lt;br/&gt;There was a statement that the carbon dioxide solubility in water was measured, but no solubility values were given.</method>
 <publisher>The International Union of Pure and Applied Chemistry</publisher>
 <sources>
  <citation>Mackenzie, J. J.; Ann. Phys. (Leipzig) [3] 1877, 1, 438-51.</citation>
  <pubtype>paper</pubtype>
  <url>https://doi.org/10.1002/andp.18772370709</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>Carbon dioxide. Prepared by action of sulfuric acid on marble. Dried by bubbling through sulfuric acid.</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>Water. Nothing specified.</sample>
 </substances>
 <substances>
  <constituent>2</constituent>
  <formula>None</formula>
  <molweight>0.0</molweight>
  <name>Chloride salts (x3)</name>
  <sample>Salts. Recrystallized. Solution prepared by weight and checked by evaporation to dry salt.</sample>
 </substances>
 <system>Carbon dioxide with Chloride salts (x3) and Water</system>
 <title>Solubility data from IUPAC SDS Volume 62 (page ?) - Carbon dioxide with Chloride salts (x3) and Water</title>
</compilation>