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Molality-molarity conversion

The conversion is more involved because the molality is defined in terms of the mass of solvent but the molarity is defined in terms of the volume of solution. To carry out the conversion we need to know the density of the solution. [Pg.449]

We have information about molarity (mol/L) and density (g/mL) and are asked to find molality (mol/kg) and mole fraction (mol/mol). A good way to approach conversions from molarity to another measure is to choose a convenient volume for the solution, determine its mass and the mass of solute, and find the mass of water by difference. Then convert mass of water to kilograms and to moles to complete the calculations. [Pg.833]

Lewis and Randall stated that in dilute solutions the activity coefficient of a strong electrolyte is the same in all solutions of the same ionic strength this statement was confirmed in thermodynamic deductions of activity coefficients. The molality version of 7 can be applied in a fully analogous way and allows a more straightforward treatment of solution properties. [Conversion of molality into molarity requires the solution densities e.g., for a solute of molar mass M and a solution of density q we have... [Pg.51]

Solubility concentratiorrs can be expressed many ways, including molarity (mol/L), molality (mol/kg), mole fraction, weight percent, mass per unit volume (e g., g/L), etc. The conversion formttlas for solutiotts having different concentration units are presented in Table 1. [Pg.20]

The preceding sections have used standard molar concentration units for RNA and ions, indicated by brackets or the abbreviation M. Thermodynamic definitions of interaction coefficients are made in terms of molal units, abbreviated m, the moles of solute per kilogram of solvent water. Molal units have the convenient properties that the concentration of water is a constant 55.5 m regardless of the amount ofsolute(s) present, and the molality of one solute is unaffected by addition of a second solute. For dilute solutions, M and m units are interchangeable. We use molal units for the thermodynamic derivations in this section, and indicate later (Section 3.1) the salt concentrations where a correction for molar-molal conversion is required. [Pg.439]

Values of the constant determined via least-squares fits of density data for aqueous solutions of the alkali metal halides are given in table 3.6. Similar fits may be made for other electrolyte solutions so that the conversion of molality to molarity is easily carried out. Once the concentration units are known, values of y are easily calculated from y using equation (3.6.9). These quantities are given in table 3.7 for the NaCl system for concentrations up to 2.4 m. [Pg.120]

Since a large part of the NEA-TDB project deals with the thermodynamics of aqueous solutions, the units describing the amount of dissolved substance are used very frequently. For convenience, this review uses M as an abbreviation of mol-dm for molarity, c, and, in Appendices B and C, m as an abbreviation of mol-kg for molality, m. It is often necessary to convert concentration data from molarity to molality and vice versa. This conversion is used for the correction and extrapolation of equilibrium data to zero ionic strength by the specific ion interaction theory, which works in molality units (c/ Appendix B). This conversion is made in the following way. Molality is defined as moles of substance B dissolved in 1 kilogram of pure water. Molarity is defined as Cg moles of substance B dissolved in (/ - c M) kilogram of pure water, where p is the density of the solution in kg-dm and the molar weight of the solute in kg-mof. ... [Pg.25]

Baes and Mesmer [76BAE/MES], (p.439) give a table with conversion factors (from molarity to molality) for nine electrolytes and various ionic strengths. Conversion factors at 298.15 K for twenty four electrolytes, calculated using the density equations reported by Sohnel and Novotny [85SOH/NOV], are reported in Table 11-5. [Pg.26]

X Vg is the sum of the stoichiometric coefficients of the reaction, cf. Eq.(II.54) and the values of g are the factors for the conversion of molarity to molality as tabulated in Table II-5 for several electrolyte media at 298.15 K. In the case of very dilute solutions, these factors are approximately equal to the reciprocal of the density of the pure solvent. Then, if the solvent is water, molarity and molality may be used interchangeably, and A",. The differences between the values in Table 11-5 and the values listed in the uranium NEA-TDB review [92GRE/FUG] (p.23) are found at the highest concentrations, and are no larger than + 0.003 dm -kgreflecting the accuracy expected in this type of conversion. The uncertainty introduced by the use of Eq. (11.38) in the values of log will be no larger than + 0.001 X Vg. ... [Pg.26]

Table II-5 Factors q for the conversion of molarity, cb, to molality, of a substance B, in various media at 298.15 K (calculated from densities in [85SOH/NOV])... Table II-5 Factors q for the conversion of molarity, cb, to molality, of a substance B, in various media at 298.15 K (calculated from densities in [85SOH/NOV])...
As you can see, the density of the solution serves as a conversion factor between molality and molarity. [Pg.473]

Outline the steps required for conversion between molarity, molality, and percent by mass. [Pg.498]

You want to convert among molarity, molality, and mole fraction of a solution. You know the masses of solute and solvent and the volume of solution. Is this enough information to carry out all the conversions Explain. [Pg.419]

For aqueous-phase chemical reactions the commonly used concentration unit is mol L 1. Aqueous solutions in cloud and raindrops are characterized by concentrations in the range of pmolL. For a dilute aqueous solution molality (mol kg-1) is approximately equal to molarity (mol L-1). The conversion between molar concentration c and molality m is... [Pg.1180]


See other pages where Molality-molarity conversion is mentioned: [Pg.61]    [Pg.63]    [Pg.489]    [Pg.87]    [Pg.437]    [Pg.10]    [Pg.623]    [Pg.628]    [Pg.16]    [Pg.393]    [Pg.398]    [Pg.540]    [Pg.14]    [Pg.28]   
See also in sourсe #XX -- [ Pg.429 ]




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