Solutes molar concentrations

Amount of solute = Molar concentration x Volume of solution... 

The germanium is extracted from hydrochloric acid solution (molar concentration 8) with the aid of chloroform and subsequently reextracted by shaking out with water. 

The total free energy of a mass of material obviously depends on its weight and the form in which it occurs. In order to compare the free energy of one mass of material with that of another, we must reduce both to comparable standard conditions. Standard free energy (AF ) is used for this purpose and is the free energy of one mole of the material in its normal physical form at 298°K and one atmosphere pressure. In solution, molar concentration is the standard form. 

The chromatographic partition (distribution) coefficient for dissolution, K, given by eqn (2.38) will be denoted by K, in this section to distinguish it from partition coefficients for adsorption at the gas-liquid, and gas-solid, Ka, interfaces. It is defined by the ratio of solute molar concentration in stationary and mobile phase ... 

Equation (107) can be converted into solution molar concentrations by division by the total volume of solution in the system,... 

Equation (153) is the adsorption equation for divalent cation adsorption, 0j, at the aqueous S—MO interface as a fimction of cation solution molar concentration,... 

Equation (273) is the adsorption equation for divalent anion adsorption, at the aqueous S-MO interface as a function of anion solution molar concentration, xa-The adsorption equation for divalent anion adsorption, can be expressed as a function of total or initial anion solution molar concentration, cj, by first solving the... 

Using the mass action adsorption constant, K Y fitting parameter, one can see that Fig. 33 appears to give satisfactory agreement between the mole fraction of surface sites complexed with solute, QgY equilibrium solute solution molar concentration, Xy, the data of James and Healy [23] for Co(ll) adsorption on silica. 

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. 

Figure Bl.22.8. Sum-frequency generation (SFG) spectra in the C N stretching region from the air/aqueous acetonitrile interfaces of two solutions with different concentrations. The solid curve is the IR transmission spectrum of neat bulk CH CN, provided here for reference. The polar acetonitrile molecules adopt a specific orientation in the air/water interface with a tilt angle that changes with changing concentration, from 40° from the surface nonnal in dilute solutions (molar fractions less than 0.07) to 70° at higher concentrations. This change is manifested here by the shift in the C N stretching frequency seen by SFG [ ]. SFG is one of the very few teclnhques capable of probing liquid/gas, liquid/liquid, and even liquid/solid interfaces.

Find the partial molal volume of ZnCl2 in these solutions at 0.5, 1.0, 1.5 and 2.0 molar concentrations. 

Nitration in the presence of strong acids or Lewis acids Solutions of dinitrogen pentoxide in sulphuric acid nitrate 1,3-dimethyl-benzene-4,6-disulphonic acid twice as fast as a solution of the same molar concentration of nitric acid. This is consistent with Raman spectroscopic and cryoscopic data, which establish the following ionisation ... 

Both molarity and formality express concentration as moles of solute per liter of solution. There is, however, a subtle difference between molarity and formality. Molarity is the concentration of a particular chemical species in solution. Formality, on the other hand, is a substance s total concentration in solution without regard to its specific chemical form. There is no difference between a substance s molarity and formality if it dissolves without dissociating into ions. The molar concentration of a solution of glucose, for example, is the same as its formality. 

A stock solution is prepared by weighing out an appropriate portion of a pure solid or by measuring out an appropriate volume of a pure liquid and diluting to a known volume. Exactly how this is done depends on the required concentration units. For example, to prepare a solution with a desired molarity you would weigh out an appropriate mass of the reagent, dissolve it in a portion of solvent, and bring to the desired volume. To prepare a solution where the solute s concentration is given as a volume percent, you would measure out an appropriate volume of solute and add sufficient solvent to obtain the desired total volume. 

Calculate the molar concentration of NaCl, to the correct number of significant figures, if 1.917 g of NaCl is placed in a beaker and dissolved in 50 mF of water measured with a graduated cylinder. This solution is quantitatively transferred to a 250-mF volumetric flask and diluted to volume. Calculate the concentration of this second solution to the correct number of significant figures. 

The true thermodynamic equilibrium constant is a function of activity rather than concentration. The activity of a species, a, is defined as the product of its molar concentration, [A], and a solution-dependent activity coefficient, Ya. 

A quantitative solution to an equilibrium problem may give an answer that does not agree with the value measured experimentally. This result occurs when the equilibrium constant based on concentrations is matrix-dependent. The true, thermodynamic equilibrium constant is based on the activities, a, of the reactants and products. A species activity is related to its molar concentration by an activity coefficient, where a = Yi[ ] Activity coefficients often can be calculated, making possible a more rigorous treatment of equilibria. 

In the absence of Fe +, the membrane is colorless, but when immersed in a solution of Fe + and C, the membrane develops a red color as a result of the formation of a Fe +-bathophenanthroline complex. A calibration curve determined using a set of external standards with known molar concentrations of Fe + gave a standardization relationship of... 

Table 2 Hsts examples of compounds with taste and their associated sensory quaUties. Sour taste is primarily produced by the presence of hydrogen ion slightly modified by the types of anions present in the solution, eg, acetic acid is more sour than citric acid at the same pH or molar concentration (43). Saltiness is due to the salts of alkaU metals, the most common of which is sodium chloride. However, salts such as cesium chloride and potassium iodide are bitter potassium bromide has a mixed taste, ie, salty and bitter (44). Thus saltiness, like sourness, is modified by the presence of different anions but is a direct result of a small number of cations.

The viscosity of hydiochloiic acid solutions, T], incieases slightly with incieasing concentration and is related to the molar concentration c by... 

Traditional chemical kinetics uses notation that is most satisfactory in two cases all components are gases with or without an inert buffer gas, or all components are solutes in a Hquid solvent. In these cases, molar concentrations represented by brackets, are defined, which are either constant throughout the system or at least locally meaningful. The reaction quotient Z is defined as... 

Fig. 1. Concentration of NO2 in mol/1000 g solution. NO/ concentrations increase with decreased amounts of water. The highest NO/ concentrations occur at approximately 2 1 molar ratios of H2SO4 to HNO. At high concentrations of H2SO4, almost all of the HNO is ionized to form NO/. About 3%...

When the mobile phase modulator is a ddiite solute in a solvent, as when the modulator is a salt,

[Pg.1536]

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