Including water in molar mass for molarity?

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SUMMARY

The discussion centers on calculating the mass of potassium sodium tartrate (KNaC4H4O6*4H2O) needed to prepare a 1M solution. To achieve the desired molarity, it is essential to use the full formula weight, which includes the mass of water (H2O) associated with the compound. Specifically, for 60 mL of a 1M solution, the total molar mass calculation must account for the four water molecules, ensuring accurate measurement of the compound's mass.

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  • Understanding of molarity and solution preparation
  • Knowledge of molar mass calculations
  • Familiarity with potassium sodium tartrate (KNaC4H4O6*4H2O)
  • Basic chemistry concepts related to solvation and hydration
NEXT STEPS
  • Research the molar mass of potassium sodium tartrate (KNaC4H4O6*4H2O)
  • Learn about solution preparation techniques for molarity
  • Explore the concept of hydration in chemical compounds
  • Study the impact of solvation on molecular weight calculations
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Chemistry students, laboratory technicians, and anyone involved in solution preparation and molarity calculations will benefit from this discussion.

mishima
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Hi, let's say I need 60 mL of a 1M solution of potassium sodium tartrate, I am looking for how many grams to measure out of my stock. So I need to convert mol to grams using molar mass. Do I use the full formula weight that includes water KNaC4H4O6*4H2O, or simply the KNaC4H4O6?
 
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You need a specific number of molecules of your substance. If every molecule carries 4 H2O around, you have to take more mass to get the same number of molecules.
Use the full formula weight, including H2O.
 
Thanks for that clarification.
 

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