The concentrations of chloride and

If the precipitates were completely dissolved, the concentrations of chloride and iodide ions would be... 

That fraction of a gram molecular weight which splits into ions is called the degree of electrolytic dissociation a. For example, in a 0.01 N sodium chloride solution a equals 0.9. Then the concentration of undissociated salt is 0.1 X 0.01 = 0.001, and the concentration of chloride and sodium ions is 0.9 X 0.01 = 0.009. 

Prepare a spreadsheet to plot the titration curve of 100 mL 0.1 M chloride titrated with 0.1 M silver nitrate (Figure 11.1). See your CD for a suggested setup. Use the spreadsheet to change the concentrations of chloride and silver (e.g., 0.2 M each, 0.05 M each), and notice how the titration curve changes. Note that there is a limit to how low the concentrations can go in these calculated plots because eventually the solubility of the AgCl at 99.9 and 100.1 mL titrant becomes appreciable. 

At higher elevations, there is fume and carry-over with the flue gases that cause deposits to form on the superheater, generating bank, and economizer tubes. Deposits may be molten depending on the concentrations of chloride and potassium. Superheater temperatures are usually between 300 C at the steam inlet and 500°C at the outlet. Although there are a variety of materials used in superheaters, ranging from chromium-molybdenum steels to stainless steels and nickel-base alloys, changing materials offers httle improvement when superheater deposits are molten. 

Equation 8.7 explains the solubility curve for AgCl shown in Figure 8.1. As Ch is added to a solution of Ag+, the solubility of AgCl initially decreases because of reaction 8.1. Note that under these conditions, the final three terms in equation 8.7 are small, and that equation 8.1 is sufficient to describe the solubility of AgCl. Increasing the concentration of chloride, however, leads to an increase in the solubility of AgCl due to the soluble chloro-complexes formed in reactions 8.3-8.5. ... 

Membrane Sep r tion. The separation of components ofhquid milk products can be accompHshed with semipermeable membranes by either ultrafiltration (qv) or hyperfiltration, also called reverse osmosis (qv) (30). With ultrafiltration (UF) the membrane selectively prevents the passage of large molecules such as protein. In reverse osmosis (RO) different small, low molecular weight molecules are separated. Both procedures require that pressure be maintained and that the energy needed is a cost item. The materials from which the membranes are made are similar for both processes and include cellulose acetate, poly(vinyl chloride), poly(vinyHdene diduoride), nylon, and polyamide (see AFembrane technology). Membranes are commonly used for the concentration of whey and milk for cheesemaking (31). For example, membranes with 100 and 200 p.m are used to obtain a 4 1 reduction of skimmed milk. 

IQ. To determine the concentration of chloride ion, - a 5-mL aliquot of the methyl lithium solution is cautiously added to 25 ml of water and the resulting solution is acidified with concentrated sulfuric acid and then treated with 2-3 ml of ferric ammonium sulfate [Fe(NH4)( 04)2 12 H2O] indicator solution and 2-3 ml of benzyl alcohol. The resulting mixture is treated with 10.0 mL of standard aqueous 0.100 M silver nitrate solution and then titrated with standard aqueous 0.100 H potassium thiocyanate solution to a brownish-red endpoint. 

It is apparent that the critical pitting potential for a given alloy depends on the concentration of chloride ions, on the concentration of inhibiting anions in the solution and on the temperature of the solution. Unfortunately, the situation is complicated further by the fact that there is an induction period for the onset of pitting, which means that the pitting propensity... 

The electrons released are partly accepted by dissolved oxygen at the surface millscale and partly by the H, with the consequent formation of Hj gas. The concentration of chloride ions within the pit will increase owing to migration, and this too will stimulate dissolution. 

Waters of intermediate hardness frequently contain fair amounts of other constituents and there is often a tendency for the scale to be loosely attached, permitting corrosion to occur irregularly underneath. In most waters the bicarbonate content is less than the hardness, but a few natural waters are known where the reverse is the case. These waters have been partially softened by the zeolite process which occurs underground, and then contain sodium bicarbonate which, together with the high concentration of chloride and other minerals, may accelerate attack. 

Aggressive environments include marine conditions and particularly industrial atmospheres containing high concentrations of acid gases such as sulphur dioxide rain washing is benehcial in both environments, while dampness and condensation alone can accentuate the rate of attack in the presence of chlorides and acidic sulphates. 

Galvanised steelwork buried in the soil in the form of service pipes or structural steelwork withstands attack better than bare steel, except when the soil is more alkaline than pH 9-4 or more acid than pH 2-6. Poorly aerated soils are corrosive to zinc, although they do not necessarily cause pitting. However, soils with fair to good aeration containing high concentrations of chlorides and sulphates may do so. Bare iron may be attacked five... 

Precipitation of silver bromide will occur when the concentration of the bromide ion in the solution is 2.0 x 103 times the iodide concentration. The separation is therefore not so complete as in the case of chloride and iodide, but can nevertheless be effected with fair accuracy with the aid of adsorption indicators (Section 10.75(c)). 

In the last calculation, pCl- = 1.48, hence pAg+ =9.92 - 1.48 = 8.44. In this manner, the various concentrations of chloride and silver ions can be computed up to the equivalence point. At the equivalence point ... 

Sulfate ions have reactions similar to those of chloride. They are corrosion-causative agents (similar to oxygen and hydrogen) of the various types of concentration cell corrosion. In addition, they also are depassivation agents and may greatly accelerate the risk of stress corrosion mechanisms. Saline corrosion pits resulting from high concentrations of chloride and sulfate salts also may be associated with low pH corrosion because hydrochloric acid and sulfuric acid can form within the pit, under deposits. 

With gallium chloride, ferric chloride and antimony pentachloride the rate coefficients were dependent upon the concentration of chlorobenzene and the square of the concentration of the catalyst, but the third-order coefficients varied with the initial concentration of the catalyst (Table 103)394. The overall kinetic equation was, therefore,... 

G.19 In medicine it is sometimes necessary to prepare solutions with a specific concentration of a given ion. A lab technician has made up a 100.0-mL solution containing 0.50 g of NaCl and 0.30 g of KCl, as well as glucose and other sugars. What is the concentration of chloride ions in the solution ... 

Self-Tfst 11.14B Chloride ion is added to a solution containing the following concentrations of soluble salts 0.020 mol-L 1 Pb(NO,)2(aq) and 0.0010 mol-L 1 AgN03(aq). (a) Use the information in Table 11.4 to determine the order in which each ion precipitates as the concentration of chloride ion is increased and give the concentration of Cl when precipitation of each begins, (b) Calculate the concentration of the first ion to precipitate that remains in solution when the second ion precipitates. 

The concentration of chloride ion in seawater is around 0.55 M. To compare the solubility of Pb freshwater vs. seawater, calculate the solubility in g/L of PbCb in pure water and in 0.55 M NaCl. 

The effect of chloride ions was investigated first by Silverman and Dodson. These authors observed an increase in as the concentration of chloride ion was increased from 0 to 0.55 M in perchlorate media of constant acidity. The rate expression found to fit the experimental data was... 

Shikazono (1978) theoretically derived that the concentrations of alkali and alkali earth elements in chloride-rich hydrothermal solution are nearly in equilibrium with hydrothermal alteration minerals such as albite, K-feldspar, K-mica, quartz, calcite, wairakite, and Mg-chlorite. If we use 500 mmol/kg H2O as the average Cl concentration of hydrothermal solution from the back-arc basin, which is in equilibrium with... 

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