Chemistry

# Why molality is preferred over molarity in expressing the concentration of a solution?

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

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## Related Questions 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.)  1.percent concentrationa.percent by massb.percent by volumec.percent by mass-volume2.molarity3.molality4.mole fraction5.normality 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. This is known as the concentration or more technically the molarity or molality 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. Neither. Molarity is moles per litre. Molality is moles in a kilogram. The concentration of solution means to express the amount of solute in specific amount of solvent or solution, there are different ways to represent the concentration of a solution as, 1-Molarity.. moles/dm3 2-Molality.. moles /K.g 3-Normality .. gram equivalent/dm3 4-Mole fraction 5-ppm 6-ppb. 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 == Molality== (1000xMolarity)/((1000xdensity of solution)- (MolarityxMolecular weight of Solute)) == If there is not a constant volume, then different, incorrect data could be given when concerning concentration, molarity, molality, etc. the amount of of solute dissolved into a solvent determines the concentration of a solution. The greater the amount of solute the stronger the concentration. in other words, the properties of molarity and molality determine the concentration of said 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. "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. im not so sure but from what we've just studied this is the list: 1.percent by mass Pm 2.percent by volume Pv 3.percentage mass-volume Pm/v 4.mole fraction Nf 5.molarity 6.molality In chemistry we might use moles per litre. In physics we'd be more likely to use g per litre or g per centimetre cubed. 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 a measure of concentration in SI. Molarity is an indication for concentration. Yes, molarity is (number of moles/liters of solution). If you increase the numerator, the molarity number will be greater. ###### ChemistryScienceChemical EngineeringMath and ArithmeticBiologyElements and CompoundsAcids and Bases Copyright © 2020 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.