Ammonium sulfate concentration calculation

Results For the St. Louis data, the target transformation analysis results for the fine fraction without July Uth and 5th are given in table 6. The presence of a motor vehicle source, a sulfur source, a soil or flyash source, a titanium source, and a zinc source are indicated. The sulfur, titanium and zinc factors were determined from the simple initial test vectors for those elements. The concentration of sulfur was not related to any other elements and represents a secondary sulfate aerosol resulting from the conversion of primary sulfur oxide emissions. Titanium was found to be associated with sulfur, calcium, iron, and barium. Rheingrover ( jt) identified the source of titanium as a paint-pigment factory located to the south of station 112. The zinc factor, associated with the elements chlorine, potassium, iron and lead, is attributed to refuse incinerator emissions. This factor could also represent particles from zinc and/or lead smelters, though a high chlorine concentration is usually associated with particles from refuse incinerators ( ). The sulfur concentration in the refined sulfate factor is consistent with that of ammonium sulfate. The calculated lead concentration in the motor vehicle factor of ten percent and a lead to bromine ratio of about 0.28 are typical of values reported in the literature (25). The concentration of lead in... 

Mass concentration (M) of various soluble components in the large particle size range under different geographical conditions (Junge, 1963). Curve (b) gives sulfate concentrations calculated from ammonium concentrations and the stoichiometric ratio of SOj to NH4 in ammonium sulfate (By courtesy of... 

For best results the current density at the anode should be about 0.15 amp/cm, but it will probably be necessary to exceed this value to complete the experiment in a reasonable time. Pass a current of 3 to 4 amp for at least 4 hours. During the first 2 hours, take out 2.0-ml samples every 20 minutes, run them into an excess of 6N sulfuric acid, and titrate the permanganate with O.IN ferrous ammonium sulfate solution. Calculate the permanganate concentration, and plot on a graph the number of equivalents of permanganate produced against the number of faradays of electricity passed, and also the current efficiency. This will be less than 30 per cent. 

As a preliminary, ferric sulfate is made by the oxidation of ferrous sulfate. Dissolve 100 g. of ferrous sulfate in 100 cc. of boiling water, to which has been added before heating 10 cc. of sulfuric acid. Add concentrated nitric acid portionwise to the hot solution, until a diluted sample gives a reddish-brown (not black) precipitate with ammonia. This will require about 25 cc. Boil the solution down to a viscous liquid to get rid of excess nitric acid, dilute to about 400 cc., and add the calculated weight of ammonium sulfate. The crystallization is conducted as in the former exercise, preferably under 20°. By the addition of potassium sulfate, the corresponding potassium iron alum may be secured. In this case, it is necessary to concentrate the solution until there is about four parts of water to one of the hydrated alum and cool to about zero to secure crystallization. Both of these alums are amethyst in color, the potassium salt being much less stable and having a rather low transition point. 

ALS was isolated from barley seedlings as a 0-33% Ammonium Sulfate precipitate and examined for inhibition by TP. It is apparent from Figure 5 that the enzyme is very sensitive to the compound. The 1(50) value (concentration required for 50% inhibition) was calculated to be 0.047 uM. This value is within the range reported for CS tested against ALS from different species (19). Imidazolinones are less potent with 1(50) values in the range 2-12 uM (26). ALS isolated from several species and their 1(50) values for TP is shown in Table I. 

Transfer 50 mL of filtrate to a 250-mL flask. Add 2 mL of 6 N nitric acid, 5 mL of nitrobenzene, and 10 mL of standardized 0.1 N silver nitrate solution. Shake the flask until the silver chloride coagulates. Prepare a saturated solution of ferric ammonium sulfate, and add just enough concentrated nitric acid to discharge the red color add 1 mL of this solution to the 250-mL flask to serve as the indicator. Titrate with 0.1 N ammonium thiocyanate solution that has been standardized against the silver nitrate solution until the color persists after shaking for 1 min. Calculate the weight percent of sodium chloride, P, by the equation... 

Calculate the concentration of protein (in milligrams per milliliter) present in FR-I, FR-II, and each of the ammonium sulfate saturation trials. 

A solution is prepared by dissolving 25.0 g of ammonium sulfate in enough water to make 100.0 mL of stock solution. A 10.00-mL sample of this stock solution is added to 50.00 mL of water. Calculate the concentration of ammonium ions and sulfate ions in the final solution. 

Finally, the quantity of ammonium sulfate added must be considered. A number of methods have been proposed to express the quantities of salt added. Figure 10-6 depicts an approach based upon the degree of saturation. At 25 C a saturated solution of ammonium sulfate is 4.1 M in ammonium sulfate (767 g of salt/liter of water). The table indicates the amount of ammonium sulfate that must be added per liter of solution, either free of ammonium sulfate or at some initial concentration, to yield any of the final concentrations listed. Concentrations shown are in terms of percent saturation at 25°C. Since the solubility of ammonium sulfate does not decrease significantly as the temperature drops (3.9M at 0°C), these values are useful regardless of the temperature. If saturated solutions of ammonium sulfate are used the amount to be added may be calculated using the equation... 

In using high concentrations of salts, allowance must be made for the fact that there are considerable volume changes when amounts of salt of the required order are dissolved in water, or when saturated solutions are diluted with water. Knowledge of these changes is necessary for the calculation of the concentration. In the case of ammonium sulfate, a nomograph is available (Dixon, 1953) which avoids much troublesome calculation. 

The specific volume of solid ammonium sulfate is 0.565 ml/g. The solubility of ammonium sulfate at 0 C is 706 g/1000 g water. Calculate (a) the concentration of ammonium sulfate in a saturated solution ati)°C nd (b) the amount of solid ammonium sulfate that must be added at 0°C to 500 ml of a "40% saturated solution to bring it to 60% saturation. ... 

Test diets were formulated by substituting bread for a portion of the glucose monohydrate in the basal iron bioassay diet (see ref. 10 or 11 for details of semipurified diet). Comparable dietary iron concentrations were attained with the same amount of bread in each diet. In addition to diets that contained bread with the iron compound baked in, each compound was added to diets that contained equal amounts of unenriched bread. The bioassay results are shown in Figure 4. The comparison diet (RBV = 100) contained ferrous ammonium sulfate with unenriched bread. There were no differences in the RBV s (calculated by slope ratio) of... 

The curve labelled b gives calculated sulfate quantities from measured NH4 concentrations and the stoichiometric ratio of SO4 to NH4 in ammonium sulfate. In the large size range this practically coincides with the measured sulfate values indicating that the particles are composed of (NH4)2S04. 

A solution of sodium carbonate (62 g, 0.50 mole) in water (250 ml) is placed in a 1-1 flask fitted with a stirrer and thermometer and cooled in ice-salt to 5°C, whereupon 30% hydrogen peroxide (70 g, 0.6 mole) is added in one portion. This mixture is cooled to 0° and treated with finely powdered and sieved phthalic anhydride (75 g, ca. 0.5 mole), then stirred rapidly at — 5° to 0° for 30 min or until almost all the anhydride has dissolved. Next the solution is treated in a separatory funnel with ether (350 ml) and shaken with a cold solution of concentrated sulfuric acid (30 ml) in water (150 ml), then extracted three times with ether (150 ml portions). The ether extracts are united, washed with 40 % ammonium sulfate solution (200 ml), and dried overnight in the ice-chest over anhydrous magnesium sulfate (50 g). The content of peroxyphthalic acid is determined by titration. The yield is 78% (calculated on phthalic anhydride). 

The accurate calculation of the ammonium nitrate concentrations for this rather complicated system is usually performed using computational thermodynamic models (see Section 10.4.6). However, one can often estimate the ammonium nitrate concentration in an air parcel with a rather simple approach taking advantage of appropriate diagrams that summarize the results of the computational models. For ammonia-poor systems one can assume as a first-order approximation that the ammonium nitrate concentration is very small. For ammonia-rich systems when the particles are solid, the approach is the same as that of Section 10.4.3 with one important difference. In these calculations one uses the free ammonia instead of the total ammonia. The free ammonia in the system is defined as the total ammonia minus the ammonia required to neutralize the available sulfate. So in molar units, we have... 

For ammonia-rich aqueous systems the ammonium nitrate calculation is complicated by the dependence of Kp not only on Tand RH but also on the sulfate concentration. This dependence is usually expressed by the parameter Y (Figure 10.21). The parameter Pis the ionic strength fraction of ammonium sulfate and is calculated as... 

CMB Application to Central California PM Chow et al. (1992) apportioned source contributions to aerosol concentrations in the San Joaquin Valley of California. The source profiles used for CMB application are shown in Table 26.1. The standard deviations oa.. of the profiles (three or more samples were taken) are also included. To account for secondary aerosol components in the CMB calculations, ammonium sulfate, ammonium nitrate, sodium nitrate, and organic carbon were expressed as secondary source profiles using the stoichiometry of each compound. The average elemental concentrations observed at one of the receptors—Fresno, California, in 1988-1989— are shown in Table 26.2. The ambient concentrations of some species (c.g., Ga, As, Y, Mo, Ag) included in the source profiles were below the detection limits. These species... 

It is possible to calculate the forces involved in these electrostatic interactions, especially those that vary according to the concentration of salts. It has thus been demonstrated that the scope of electrostatic interactions decreases with the salt concentration. When the medium is saturated with salts, the electrostatic forces become negligible as compared to the Van der Waals forces, so the particles tend to agglomerate and precipitate. This explains why proteins precipitate in an aqueous solution saturated with ammonium sulfate. It is also clear that colloids, occurring either naturally or following a treatment, are flocculated by salts in the wine. 

The concentrations of the carbon sources and the precursors were determined by HPLC (Animex HPX87-H, RI-Detector). Ammonium sulfate was detected with an ammonia-sensitive electrode (Orion Research Inc., Boston, USA). Polymer concentrations were determined after Braunegg s method described earlier. To determine the cell dry weight (CDW) 5 mL of the culture broth were centrifuged at 4000 rpm for ten minutes in preweighted glass tubes. After lyophilisation of the pellets, the CDW was calculated from the weigh difference. 

It is also to be noted that the usual procedure of expressing concentrations in terms of the fractional saturation of the solution with ammonium sulfate is sometimes ambiguous. The temperature coefficient of solubility is considerable for these solutions, and unless the temperature of the measurements is specified, the given conditions may be difficult for other investigators to reproduce exactly. For temperature values in the neighborhood of 20 to 25 °C. half saturated ammonium sulfate may be taken as equivalent to a 2.05 molal solution. Other fractional saturations may be calculated by proportionality (see also 43). 

In these separations, McMeekin added the ammonium sulfate used for crystallization by dialysis through a rotating cellophane bag immersed in the protein solution. The amount of salt initially placed in the bag was calculated so as to give the desired final conoenfration of ammonium sulfate in the whole system at eqmlibrium. In this way, the increase of salt concentration wi time was very gradual and conditions for crystallization were more favorable than when the salt was added rapidly. 

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