answersLogoWhite

Top Answer
User Avatar
Wiki User
Answered 2011-09-07 02:19:32

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.

001
๐Ÿ™
0
๐Ÿคจ
0
๐Ÿ˜ฎ
0
๐Ÿ˜‚
0
User Avatar

Your Answer

Related Questions


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


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


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


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


Molarity is Moles/Liter, Molality is Moles/kg


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


"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.


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.


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.


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.


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 of a solution is equal to mol/L.



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 = 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.


Check out the link Molarity, Molality and Normality



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.



Copyright ยฉ 2021 Multiply Media, LLC. All Rights Reserved. The material on this site can not be reproduced, distributed, transmitted, cached or otherwise used, except with prior written permission of Multiply.