What is the molality of a 10.4 M CH3OH solution in H2O?

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To find the molality of a 10.4 M CH3OH solution with a density of 0.858 g/mL, one must first understand the definitions of molarity and molality. Molarity is moles of solute per liter of solution, while molality is moles of solute per kilogram of solvent. Using the density, the mass of the solution can be calculated, which allows for determining the mass of the solvent (H2O) after accounting for the mass of the solute (methanol). The calculation involves unit conversions and applying the definitions appropriately. Engaging with the problem and showing initial efforts is encouraged before seeking direct answers.
mate1000
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Would anyone be able to help me with this question?
The density of a 10.4 M CH3OH (methanol) solution is 0.858 g/mL. What is the molality (m) of this solution? H2O is the solvent.
Anhy help is appreciated cheers.
 
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Start with definitions of both molarity and molality. See what and how you can calculate from the information given, what you need to find out molality.

See percentage to molality conversion example for hints on the general approach to this type of the question.
 


That is the most unhelpful post i have ever read
 


mate1000, Borek gave you advice on how to start. You must know and use the definitions of molarity and molality. The rest is simple unit conversions and simple concentration information. We posters on this board are expected not to plainly answer questions with full solution until the original questioner has tried to solve and shown some effort to do so.
 
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