What's the Difference Between Molarity and Molality?

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What's the difference between molarity and molality? They are both measures of concentration, but molarity has to do with volume (in Liters) and molality has to do with mass (in kilograms). Also, molarity talks about the volume of the total solution (solute and solution combined), and molality is about mass of the solute and solvent separately.

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Normality?

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Clearest definition of Molarity and Molality I've found! The visuals help so much

[@tdewitt451]

Yes, you're absolutely right. But usually that difference is so small that it doesn't matter, even in solvents of different densities. The one situation where it does really start to matter is in solutions that have a very high concentration of solute, so if you're dissolving a whole ton of something into a solvent, then that can really start to add up.

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Thank you so much for explaining the significance and differences between molality and molarity. Very often do instructors tell you to simply "plug the numbers into the formula". However, it is so much better to have access to a more thorough explanation.

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This guy....is saving my life...this and the gas laws and all that...helping me for passing the exams...Thanks a lot! :) But which is greater...Molaltiy or Molarity?

[@niggamog_69]

Molality does not change with temperature but molarity does

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Shouldn't it depend on the density of solution and solvent?

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one more thing, the reason some chemical equation preferred molal over molarity is that molality wont be effected by the temperature. the heat that is generated towards the solution will make it's molecules expanding therefore the volume increased, but the mass remains the same

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Do you think you could make a video on molality practice problems?

[@ery1502]

I have a funny question, is it molar and molal concentration of solute or solution? You mention a molar of solution but isn't it molar concentration of solute in a solution (or simply molar concentration of solute)? I know it's just the naming but it still confuses me a bit, I would say molar concentration of solute in a solution and molal concentration of solute per solvent?

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Do you also need to add solute to the 3rd flask then a solvent again until it reaches 1 liter or just add solvent up to 1liter???

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[@ery1502]

I'm sorry I forgot to say this, so the correct term would be the molar or molal concentration of the solute (in a solution), right? And one more thing, so we just assume the entire amount of solute is dissolved, right? Like there isn't any part of it that is not dissolved, since the definition of concentration is the amount of solute dissolved in a solution. I hope you can answer my questions, thank you.

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[@ery1502]

When people say a solution is less or more concentrated, they actually mean that the moles(atoms/molecules) of the solute are less or more crowded together in a solution? Shouldn't that say that the concentration is actually the concentration of a solute (in a solution )? I think about certain details so I'm sorry if it sounds weird.

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[@ABeardedDad]

So if I'm interpreting this right, there should also be another very slight (in this example at least) difference, but still important. In a 1M sol'n there is 1L of CaCl2 + Water, which would weight out to basically 1kg. However in the Molality it will actually be 1.111kg, which is 1kg of Water + 111.0g of CaCl2. Is this correct?? This would no doubt become a more significant difference also in different density solvents.

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I am confused that temperature doesn't​ affect molality because mass remains unaffected . How?will you please explain sir?

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so is Molality ALWAYS greater than molarity in aqueous solutions, or are there factors such as density that will change that ?

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