Sulfuric acid requirements

Economics. In contrast to NSP, the high nutrient content of TSP makes shipment of the finished product preferable to shipping of the raw materials. Plants, therefore, are located at or near the rock source. The phosphoric acid used, and the sulfuric acid required for its manufacture, usually are produced at the site of the TSP plant. As in the case of NSP, the cost of raw materials accounts for more than 90% of the total cost. Most of this is the cost of acid. 

Nonferrous Metal Production. Nonferrous metal production, which includes the leaching of copper and uranium ores with sulfuric acid, accounts for about 6% of U.S. sulfur consumption and probably about the same in other developed countries. In the case of copper, sulfuric acid is used for the extraction of the metal from deposits, mine dumps, and wastes, in which the copper contents are too low to justify concentration by conventional flotation techniques or the recovery of copper from ores containing copper carbonate and siUcate minerals that caimot be readily treated by flotation (qv) processes. The sulfuric acid required for copper leaching is usually the by-product acid produced by copper smelters (see Metallurgy, extractive Minerals RECOVERY AND PROCESSING). 

Because calcium sulfide contained in the black ash had a highly unpleasant odor, methods were developed to remove the odor by recovering the sulfur, therein providing at least part of the raw-material for the sulfuric acid required in the first part of the process. Thus, the Leblanc prtKcss demonstrated, at the very beginning, the typical ability of the chemical industry to develop new processes and new products, and often in so doing to turn a liability into an asset. 

The addition of sulfuric acid requires ca. 1 hour. Occasional swirling of the Erlenmeyer flask is recommended for smooth generation of methyl nitrite. 

The theoretical amount of sulfurous acid required to reduce a given amount of chromium can be calculated from the above equation. The actual amount of sulfurous acid required to treat a wastewater will be greater than this because other compounds and ions present in the wastewater may consume some of the acid. Primary among these is dissolved oxygen, which oxidizes sulfurous acid to sulfuric acid according to the following reaction ... 

In addition to the sulfuric acid required for pH adjustment, some amount of acid is consumed by the reduction reaction (Equation 8.15). If sulfur dioxide is used as the reducing agent, it will provide all the acid consumed by this reaction, and additional acid will not be required. However, if sodium bisulfite or sodium metabisulfite is used, additional acid must be supplied to satisfy the acid demand. This acid requirement is stoichiometric and can be calculated from Equations 6.19 to 6.22. 

Standardization of a solution of sulfuric acid required 29.03 mL of 0.06477 M NaOH when exactly 25.00 mL of H2S04 was used. What is the molarity of H2S04 Refer to Equation (4.5) for the reaction involved. 

Sulfuric acid has found limited use in boiler cleaning operations. It is not feasible for removal of hardness scales due to the formation of highly insoluble calcium sulfate. It has found some use in cases where a high-strength, low-chloride solvent is necessary. Use of sulfuric acid requires high water usage in order to rinse the boiler sufficiently. 

B = average mis of 0.5N sulfuric acid required for titration of the blan ks C = normality of acid corrected for temperature F = factor for EtAcet specified in Table II as 0.0881, and... 

CAUTION Chemical substances such as sodium hydroxide and sulfuric acid require special handling see appendix 2b for guidelines. 

Calculate the volume of 2 mol dm-3 solution of sulfuric acid required to react with 24g of magnesium. 

Carbonate (as K2C03) Each milliliter of 1 N sulfuric acid required between the phenolphthalein and methyl orange endpoints in the Assay (above) is equivalent to 138.2 mg of carbonate. 

Assay Based on the stated or labeled percentage of Potassium Hydroxide (KOH), accurately weigh a volume of the solution equivalent to about 1.5 g of Potassium Hydroxide, and dilute it to 40 mL with recently boiled and cooled water. Continue as directed under Assay in the monograph for Potassium Hydroxide, beginning with cool to 15°.. .. Carbonate (as K2C03) Each milliliter of 1 N sulfuric acid required between the phenolphthalein and methyl orange endpoints in the Assay is equivalent to 138.2 mg of carbonate. Lead Determine as directed under Lead Limit Test, Appendix IIIB, preparing the Sample Solution as follows Dilute the equivalent of 1 g of Potassium Hydroxide (KOH), calculated on the basis of the Assay, with a mixture of 5 mL of water and 11 mL of 2.7 N hydrochloric acid. Use 2 p,g of lead (Pb) ion in the control. 

A = mis of 0.5N sulfuric acid required for titration of sample, as described under opn h... 

Sulfuric Acid Requirements for Industrial Alkylation Plants... 

One patented process (40) was introduced in the mid- 60s to reduce the amount of sulfuric acid required by alkylation it was called the Sulfuric Acid Recovery Process (SARP) and was jointly licensed by Texaco Development Corporation and Stratford Engineering Corporation. Chemically, SARP proved all claims made for it. Utilized only with propylene/butylene alkylation the acid requirement was reduced as much as 70% actual acid dilution rates were lower than 0. 2 acid/gallon alkylate. However, the spent acid from SARP was different and could not be regenerated at the same rate as regular spent alkylation acid. This caused the chemical companies to increase the charges for regenerating the SARP spent acid to a point where there was no economic incentive to operate SARP. The two commercial SARP installations are not in use at the present time although new possibilities for SARP have arisen just in the past few months. 

Reaction is carried out simply by bringing the reactants into contact a gaseous alkene is bubbled through the acid, and a liquid alkene is stirred or shaken with the acid. Since alkyl hydrogen sulfates are soluble in sulfuric acid, a clear solution results. The alkyl hydrogen sulfates are deliquescent solids, and are difficult to isolate. As the examples below show, the concentration of sulfuric acid required for reaction depends upon the particular alkene involved we shall later account for this in a reasonable way (Sec. 6.11). 

A) n-Butyl Bromide (Sm.). Enter in your note book the calculated amounts of 1-butanol, hydrobromic acid (48 per cent), and sulfuric acid required for the preparation of n-butyl bromide, starting with 0.1 mole of the alcohol. If the instructions in your laboratory are to use the sodium bromide method, calculate the amount as shown in the equation above and use 10 ml of water to dissolve the sodium bromide. Have the instructor approve the amounts before you begin the experiment. 

TABLE 15.7 Ratios of Sodium Carbonate to Sulfurous Acid° Required for Sulfite Pulping at Various pHs... 

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