Both express moles of solute in the numerator.
Molarity is a measure of the concentration of a solution, and therefore cannot be said to be just moles.It is in fact moles per litre (mol/L), or molars.
Mol is a cocentration unit !
- molarity- molality-percentage composition
1.12 m
Concentration
through molarity,molality, normality. through molarity,molality, normality.
In dilute solutions... ie closer a solution is to pure water the closer molality and molarity come to equalling each other. This is because the molality uses mass and molarity uses volume, the ratio of these two (mass and volume) is density, and water has the density of 1 therefore the mass and volume are equal to each other. THEREFORE calculating the molarity of water is the same as calculating the molality of water.
The number of moles of solute dissolved in 1 L of a solution would be the molarity. As an example, if you had 2 moles of solute in 1 liter the molarity would be 2M.
"MolaRity" is the correct spelling for mass per amount solution."MolaLity" is the correct spelling for mass per amount solvent.The conversions of molality, b, to and from the molarity , c,for one-solute solutions are:c = ρ.b / [1 + b.M]andb = c / [ρ -c.M]where ρ is the mass density of the solution, b is the molality, and M is the molar mass of the solute.
Molality is used when temperature varies in an exothermic or endothermic reaction because it is not dependent on temperature or pressure. Molality does not depend on tempratute whereas molarity does.
HCl is a strong acid no matter the molarity or molality.
Molarity is a measure of the concentration of a solution, and therefore cannot be said to be just moles.It is in fact moles per litre (mol/L), or molars.
Molarity or Molality
Mol is a cocentration unit !
4 mol over 0.800 kg
Molality is independent of temperature, so when you are trying to find changes in boiling and freezing points you need something that will stay constant regardless of the change in temperature. Molarity is temperature dependent and also is based on the volume of a solution, both of which are needed to calculate pressure using the ideal gas law, PV=nRT. Osmotic pressure is similar but we substitute the number of moles of the solution and the volume by using the molarity, you cannot do this with molality, since it is dependent on mass, not volume.
moles of solute over kg of solvent