The following data (for 25°C) were obtained at the pzc for the Hg-aqueous NaF interface. Estimate and plot it as a function of the mole fraction of salt in solution. In the table,/ is mean activity coefficient such that a = f m , where m is mean molality.  [c.216]

Experiments on sufficiently dilute solutions of non-electrolytes yield Henry s laM>, that the vapour pressure of a volatile solute, i.e. its partial pressure in a gas mixture in equilibrium with the solution, is directly proportional to its concentration, expressed in any units (molar concentrations, molality, mole fraction, weight fraction, etc.) because in sufficiently dilute solution these are all proportional to each other.  [c.360]

Procedure. Calculate the heats of solution of the two species, KF and KF HOAc, at each of the four given molalities from a knowledge of the heat capacity. Calculate the enthalpy of solution per mole of solute at each concentration. Find  [c.74]

Emsley, in the same paper referred to in Computer Project 3-1, presents viscosity measurements T] for solutions of KE in HOAc as a function of molality m with the following results  [c.79]

Molality basis (mol m ) = line  [c.94]

Molality basis Band variance 0-2  [c.100]

Donor ionization energy Eo Molality basis  [c.102]

Hartmann number Ha Molality basis  [c.103]

Mach number Ma Molality b  [c.104]

Molality basis K Polymeric form pol  [c.105]

Solutions in water are designated as aqueous, and the concentration of the solution is expressed in terms of the number of moles of solvent associated with 1 mol of the solute. If no concentration is indicated, the solution is assumed to be dilute. The standard state for a solute in aqueous solution is taken as the hypothetical ideal solution of unit molality (indicated as std. state or ss). In this state  [c.532]

The values for unit weight of solvent (molality scale) can be obtained by multiplying the corresponding values for unit volume by the square root of the density of water at the appropriate temperature.  [c.832]

Molality Weight % Molality Weight % Molality Weight %  [c.1084]

Molality is used in thermodynamic calculations where a temperature independent unit of concentration is needed. Molarity, formality and normality are based on the volume of solution in which the solute is dissolved. Since density is a temperature dependent property a solution s volume, and thus its molar, formal and normal concentrations, will change as a function of its temperature. By using the solvent s mass in place of its volume, the resulting concentration becomes independent of temperature.  [c.18]

Source Values taken from Bates, R. G. Determination of pH Theory and Practice, 2nd ed. Wiley New York, 1973. Concentrations are given in molality (moles solute per kilograms solvent).  [c.492]

It is conventional to use molality—moles of solute per kilogram of solvent (symbol m)—as the concentration unit in electrolyte thermodynamics. Accordingly, we shall represent the concentrations of both the indifferent electrolyte and the polymer in these units in this section m3 and m2, respectively. In the same dilute (with respect to polymer) approximation that we have used elsewhere in this chapter, m2 is related to the mass volume system of units C2 by  [c.570]

The activity of an ion is related to its molality through the mean activity coefficient 7+ therefore  [c.571]

Table 1. Solution pH Standards, Molality Scale Table 1. Solution pH Standards, Molality Scale
Ion Product. The ion product of water is the product of the molality of the hydrogen and hydroxide ions, oh - temperature  [c.353]

Table 1 gives the calculated open circuit voltages of the lead—acid cell at 25°C at the sulfuric acid molalities shown. The corrected activities of sulfuric acid from vapor pressure data (20) are also given.  [c.573]

The solubility of boric acid in water (Table 6) increases rapidly with temperature. The heat of solution is somewhat concentration dependent. For solutions having molalities in the range 0.03—0.9 the molar heats of solution fit the empirical relation (49)  [c.192]

The assigned values of pH, according to the Bates-Guggenheim convention [Pure Applied Chem. 1 163 (I960)], for the primary standard solutions prepared from salts issued by the National Institute for Science and Technology (NIST, US) (U.S.) are given in Table 8.14. These are smoothed values. The ionic strength of these reference solutions is 0.1 or less. Strictly speaking the NIST scale uses a molality concentration system however, values are given in molarity units for convenience.  [c.931]

See pages that mention the term Molality : [c.263]    [c.145]    [c.356]    [c.360]    [c.365]    [c.584]    [c.585]    [c.585]    [c.74]    [c.78]    [c.78]    [c.81]    [c.94]    [c.94]    [c.94]    [c.94]    [c.100]    [c.829]    [c.935]    [c.16]    [c.18]    [c.18]    [c.32]    [c.775]    [c.239]    [c.590]   
Computational chemistry using the PC (2003) -- [ c.78 , c.79 ]

Modern analytical chemistry (2000) -- [ c.18 ]

Modern Analytical Chemistry (2000) -- [ c.18 ]

Standard Handbook of Petroleum and Natural Gas Engineering Volume 1 (1996) -- [ c.327 ]