Sulfuric acid calculating normality

In a 500-cc. three-neck flask, fitted with a reflux condenser and a mechanical stirrer (Note t), is placed 45.5 g. (0.25 mole) of 2,4-dinitrotoIuene (Note 2), 85 g. (1.5 moles) of iron (Note 3), and 100 cc. of 50 per cent (by weight) ethyl alcohol (Note 4). The mixture is heated to boiling on a water bath, the stirrer is started (Note 5) and a solution of 5.2 cc. (0.06 mole) of concentrated hydrochloric acid in 25 cc. of 50 per cent (by weight) ethyl alcohol is added slowly (Note 6). The mixture is refluxed for two hours after addition of the acid is complete. At the end of this time the apparatus is disconnected and the hot mixture is made just alkaline to litmus by the addition of the calculated amount of 15 per cent alcoholic potassium hydroxide solution (Note 7). Without allowing the mixture to cool, the iron is removed by filtration and the reaction flask is rinsed with two 50-cc. portions of 95 per cent ethyl alcohol the same alcohol is used to wash the iron residue. To the filtrate is added 84 cc. of 6 N sulfuric acid the normal sulfate of 2,4-diaminotoluene precipitates. The mixture is cooled to 250 and filtered by suction. The product is washed with two 35-rc. portions of 95 per... 

At present all licensers offer very high rates of S02-conversion, up to 99.8%, and heat recovery as much as 90%. Production-scale capacities are usually between 1,000 tpd and 3,000 tpd. At the normal operating time of about 330 days per year this amounts to 330,000-990,000 tpy of sulfuric acid calculated as 100% H2SO4. 

The parent acids of common polyprotic acids other than sulfuric are weak and the acidity constants of successive deprotonation steps are normally widely different. As a result, except for sulfuric acid, we can treat a polyprotic acid or the salt of any anion derived from it as the only significant species in solution. This approximation leads to a major simplification to calculate the pH of a polyprotic acid, we just use Kal and take only the first deprotonation into account that is, we treat the acid as a monoprotic weak acid (see Toolbox 10.1). Subsequent deprotonations do take place, but provided Kal is less than about fCal/1000, they do not affect the pH significantly and can be ignored. 

Pure parathion is a pale yellow, practically odorless oil, which crystallizes in long white needles melting at 6.0° C. (17). It is soluble in organic solvents, except kerosenes of low aromatic content, and is only slightly soluble in water (15 to 20 p.p.m. at 20° to 25° C.). Peck (35) measured its rate of hydrolysis to diethyl thiophosphate and nitro-phenate ions in alkaline solutions. He found that the reaction kinetics are first order with respect to the ester and to hydroxyl ion. In normal sulfuric acid the rate of hydrolysis was the same as in distilled water. Peck concluded that hydrolysis takes place by two mechanisms—a reaction catalyzed by hydroxyl ions and an independent uncatalyzed reaction with water. He calculated that at a pH below 10 the time for 50% hydrolysis at 25° C. is 120 days in the presence of saturated lime water the time is 8 hours. The over-all velocity constant at 25° C. is k = 0.047 [OH-] + 4 X 10-6 min.-1... 

Quenching of the drained fluids was calculated as a function of the initial fluid temperature, and of the ratio between fluid and cold sulfuric acid. As a result of an automatic drain at 30°C above normal, the resulting temperature was found to be 90°C. 

Accurately weigh 0.3 g of std p-MNA, transfer to 250 ml vol flask, dissolve in ca 100 ml distd w an equal amt of 40% sulfuric acid and dilute to tbe mark. After thorough mixing, pipette two 25 ml aliquots into two 500 ml Erlen flasks, add to each flask 25 ml 40% sulfuric acid, 50 ml 95% ethanol 100 ml distd w. Sweep the flask for 10 mins with a strong current of COa, add 50 ml of 0,15N TiCl, soln and proceed as described above under (e). Calculate normality of TiCls by the following formula Wt... 

Calculate the mass (g) of FeSC>4 that will be oxidized by 24.0 mL of 0.250 N KM11O4 in a solution acidified with sulfuric acid. The unbalanced equation for the reaction is below. The statement of normality of KMnC>4 is with respect to this reaction (Mn changes from +7 to +2 during this reaction). 

Assay With the aid of about 25 mL of water, transfer about 125 mg of sample, accurately weighed, into a 300-mL Erlenmeyer flask. Add 50.0 mL of 0.5 A potassium dichromate, mix, then carefully add 100 mL of sulfuric acid, and heat to boiling. Remove the flask from the heat, allow the solution to stand at room temperature for 15 min, cool it in a water bath, and transfer the solution to a 250-mL volumetric flask. Dilute with water almost to volume, cool to 25°, dilute to volume with water, and mix. Titrate a 50-mL aliquot with 0.1 A ferrous ammonium sulfate, using 2 or 3 drops of ortho-phenanthroline TS. Perform a blank determination (see General Provisions), and make any necessary correction. Calculate the normality, A, of the ferrous ammonium sulfate solution by the formula... 

Ceric Sulfate, 0.01 N [3.322 g Ce(S04)2 per 1000 mL] Dissolve 4.2 g of ceric sulfate [Ce(S04)2-4H20] or 5.5 g of the acid sulfate [Ce(HS04)4] in about 500 mL of water containing 28 mL of sulfuric acid, and dilute to 1000 mL. Allow the solution to stand overnight, and filter. Standardize this solution daily as follows Weigh accurately about 275 mg of hydroquinone (CgHg02), dissolve it in sufficient 0.5 N Alcoholic Sulfuric Acid to make 500.0 mL, and mix. To 25.0 mL of this solution add 75 mL of 0.5 N sulfuric acid, 20 mL of water, and 2 drops of Diphenylamine TS. Titrate with the ceric sulfate solution at a rate of about 25 drops per 10 s until an endpoint is reached that persists for 10 s. Perform a blank determination using 100 mL of 0.5 N Alcoholic Sulfuric Acid, 20 mL of water, and 2 drops of Diphenylamine TS, and make any necessary correction. Calculate the normality of the ceric sulfate solution by the formula... 

Ferrous Ammonium Sulfate, 0.1 N [39.21 g Fe(NH4)2-(S04)2-6H20 per 1000 mL] Dissolve 40 g of ferrous ammonium sulfate hexahydrate in a previously cooled mixture of 40 mL of sulfuric acid and 200 mL of water, dilute to 1000 mL with water, and mix. On the day of use, standardize the solution as follows Transfer from 25 to 30 mL of the solution, accurately measured, into a flask, add 2 drops of Orthophenanthroline TS, and titrate with 0.1 N Ceric Sulfate until the red color is changed to pale blue. From the volume of 0.1 N Ceric Sulfate consumed, calculate the normality. 

Before being charged to an alkylation unit, olefin streams are normally treated for removal of sulfur compounds. The type of treating used depends for the most part on the amount and kind of sulfur compounds present. Quantities are normally reported in parts per million units. According to Industry sources, estimates of the amount of sulfuric acid diluted lie in a range of 15 to 60 pounds per pound of sulfur in the feed. A very commonly used factor is 20 pounds per pound. In the case of methyl mercaptan, if one assumes a mole for mole reaction occurs and that the reaction products are soluble in the acid and do not titrate, then the calculated amount of acid diluted is 53.7 pounds per pound of mercaptan sulfur (dilution range 98.5 to 90.0%). This is a very severe assumption however commercial tests indicate about 45 pounds per pound and this is probably more realistic. Somewhat lower dilution rates are normally assumed for H2S and COS, typically ranging between 15 and 18 pounds per pound of sulfur present. 

Calculate the molarity and the normality of a sulfuric acid solution if 32.75 mL of it reacts with 0.4011 g of sodium carbonate. 

A solution of sulfuric acid contains 86 g of H2SO4 per liter of solution. Calculate the normality of this solution. 

The electrolyte in automobile lead storage batteries is a 3.75Msulfuric acid solution that has a density of 1.230 g/mL. Calculate the mass percent, molality, and normality of the sulfuric acid. 

Based on the concentration dependence of adhesion (similar to that presented in Fig. 3.38) the formulation of an antirust coating has been calculated [79]. It is composed of polyethylene and a sulfuric 8-oxyquinalin Cl. At 5 wt% content of this Cl adhesion of the coating to a steel substrate shows a maximum adhesion A = 0.4kN/m corresponding to the antiplastification peak of polyethylene by Cl. It is peculiar to this composition that, after endurance in a 50% aqua solution of sulfuric acid for ten days, adhesion of the initial polyethylene coating drops almost to zero, while adhesion of the inhibited ones, though sure to reduce, remains at a level (0.1-0.2kN/m) sufficient for normal operation. 

Since various sulfuric acid concentrations were used in the study, a method to normalize its effect was developed. Conductivity ratio was calculated using equation 2 to mitigate the effect of sulfuric acid conductivity. The conductivity ratio is simply the ratio of the measured electrical conductivity of the agglomerate bed divided by the conductivity of the sulfuric acid solution used during agglomeration. 

A simple way to estimate the molecular weight of PBIs is the measurement of intrinsic viscosity (f/iv) of the polymer in solution at a fixed temperature (normally 25-30 °C). The intrinsic viscosity is obtained by plotting the specific viscosity (tj p) as a function of the polymer concentration and extrapolating to zero concentration. In order to simplify the measurement process, a single-point method was proposed to calculate the tjiy from using (7.1) [35,50-52], where C is the polymer concentration in a concentrated acid, e.g., 96 wt% sulfuric acid. 

Polybenzimidazoles are normally soluble in concentrated sulfuric acid, in which the viscosity usually is determined using a capillary viscometer. For mPBI it has been demonstrated that a one-point viscosity measurement at low polymer concentrations can be used to calculate a good approximate value of the intrinsic viscosity [15], which in turn can be used to estimate the weight average molecular weight using the Mark-... 

Calculate the normality of a solution of sodium carbonate if a 25.0-mL sample requires 39.8 mL of 0.405 N sulfuric acid in a titration. 

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