Elements and Compounds

# What is the difference between molarity and molality?

###### Wiki User

The difference is in the denominators.

Molarity (M) - the number of moles of solute divided by the number of liters of solution.

Molality(m) - the number of moles of solute divided by the number of kilograms of solvent.

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## Related Questions

because molality is independent of temperature and molarity is dependent on temperature further molality is dilute while molarity is concentrated.

== Molality== (1000xMolarity)/((1000xdensity of solution)- (MolarityxMolecular weight of Solute)) ==

through molarity,molality, normality. through molarity,molality, normality.

Molarity is defined as grams of solute dissolved in 1 liter of solution and molality is defined as grams of solute dissolvd in 1Kg of solvent

Neither. Molarity is moles per litre. Molality is moles in a kilogram.

why molarity is preferred over molarity in expressing the concentration of a solution

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.

in molarity we dissolved no of moles of solute in 1 dm3 volume of its solution but in molality we dissolved no of moles of solute in 1000 gram or 1 kg of solvent in molarity we don't know the exact amount of solvent quantity but in mplality we know the exact volume of solvent ( water)

"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 = &rho;.b / [1 + b.M]andb = c / [&rho; -c.M]where &rho; is the mass density of the solution, b is the molality, and M is the molar mass of the solute.

Both express moles of solute in the numerator.

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 concentration in moles/L (symbolized by M). Molality is a different way of expressing molarity, but in moles of solute/mass of solvent in mol/kg (symbol m). Normality is molarity x number of equivalents (symbolized by N). Equivalents are the ions that it would dissociate into (H+, OH-, e-, etc.)

The molality of this solution is 1,905; to calculate the molarity you need the density of the solution.

Concentrations in molality (moles of solute per kilograms of solvent) are independent of temperature and pressure whereas concentrations in molarity (moles of solute per total volume of solution in liters) are not.

This is known as the concentration or more technically the molarity or molality of the solution.

Molality of a solution remains constant as mass of a solution independent of temperature.

Molarity:1.0 mol (NaOH) /L(solution) = 1.0 M NaOHThe conversions of molality, b, to and from the molarity , c,for one-solute solutions are:c = &rho;.b / [1 + b.M]andb = c / [&rho; -c.M]where &rho; is the mass density of the solution, b is the molality, and M is the molar mass of the solute.

Molarity solution is not a term that I have ever heard used. Molarity is always a term used to describe a concentration of solute in a solvent, i.e. of a solution. The closest I've heard to molarity solution is when people ask "what is the solution's molarity".

if one scientist reports concentrations measured in molality, another scientist elsewhere can exactly replicate the work. This is not possible with molarity. I chose the above answer on my quiz and it was actually incorrect. The correct answer should be - two solutions of the same molality have equivalent ratios of solute to water, but two solutions of the same molarity may not have equivalent ratios.

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