Mole concept molality

Complete the following concept map using the following terms molarity, mole fraction, molality, moles of solute. 

We now have the foundation for applying thermodynamics to chemical processes. We have defined the potential that moves mass in a chemical process and have developed the criteria for spontaneity and for equilibrium in terms of this chemical potential. We have defined fugacity and activity in terms of the chemical potential and have derived the equations for determining the effect of pressure and temperature on the fugacity and activity. Finally, we have introduced the concept of a standard state, have described the usual choices of standard states for pure substances (solids, liquids, or gases) and for components in solution, and have seen how these choices of standard states reduce the activity to pressure in gaseous systems in the limits of low pressure, to concentration (mole fraction or molality) in solutions in the limit of low concentration of solute, and to a value near unity for pure solids or pure liquids at pressures near ambient. 

This chapter develops the concepts of thermodynamics (Chapters 6 and 7). The material assumes an acquaintance with the nature of inter-molecular forces (Sections 5.1-5.5). The compositions of some of the solutions we discuss are expressed in terms of mole fraction and molality (Section G). 

Physiologists studying osmotic relationships of organisms, however, are often concerned with the total concentration of all dissolved substances, not just the concentrations of specific solutes. For expressing the total number of osmotically active particles in a solution, the concept of osmolality is commonly employed to refer to the osmotic pressure characteristic of a solution. One osmole is defined as the osmotic pressure of a 1.0 molal solution of an ideal solute. Because conditions of ideality do not pertain to the case of biological fluids, it is not possible to extrapolate precisely from chemical determinations of moles of solute per kilogram (or liter) of fluid to the osmolality of that fluid. Rather, this value must be determined empirically. 

Gas laws, including the ideal gas law, Dalton s law, and Graham s law Stoichiometric relations using the concept of the mole titration calculations Mole fractions molar and molal solutions... 

Zavitsas [16,17] took the concept, according to which the amount of water bound by the hydrated ions should be deducted from the total amount of solvent, a step further, but apparently too far as is demonstrated below. According to Zavitsas ideas, the mole fraction of the ions of a strong aqueous electrolyte of molality dissociating into V ions per formula is ... 

Molality, abbreviated molal or m, is useful for colligative properties because it is a more direct ratio of molecules of solute to molecules of solvent. The unit molarity automatically includes the concept of partial molar volumes because it is defined in terms of liters of solution, not liters of solvent. It is also dependent on the amounts of solvent and solute (in mole and kilogram units), but independent of volume or temperature. Thus, as T changes, the concentration in molality units remains constant while the concentration in molarity units varies due to expansion or contraction of the solutions volume. 

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