User:Allison K. Alix/Notebook/CHEM581/2012/11/02
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* <math> molality = \frac {mol solute}{kg solvent} </math>  * <math> molality = \frac {mol solute}{kg solvent} </math>  
  <math> \frac {6 moles NaCl}{1 kg water} \times \frac {57.54 g NaCl}{moles NaCl} </math>  +  
+  <math> \frac {6 moles NaCl}{1 kg water} \times \frac {57.54 g NaCl}{moles NaCl} = \frac {345.24g NaCl}{1 kg water}</math>  
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+  
+  <math> 1 kg water \times \frac {1000 g water} {1 kg water} \times \frac {1 mL water} {1 g water} = 1000 mL water</math>  
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+  <math> \frac {345.24g NaCl}{1 kg water} \times \frac {1 kg water} {1000 mL water} = \frac {34.524 g NaCl} {100 mL water}</math>  
==Notes==  ==Notes== 
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Experimental Chemistry  Main project page Previous entry Next entry 
Objective
Description
DataPreparation of 6m NaCl
NotesThis area is for any observations or conclusions that you would like to note.
