Bagged Hydrate

Hydrate is generally bagged in 2 or 3-ply paper sacks. They may be delivered loose, or on pallets, and are handled by bag truck or by fork lift truck. Their effective bulk density is about 500 kg/m.  

To avoid deterioration of the bags by moisture and of the hydrated lime by re-carbonation, bagged hydrate should be stored under cover. The ideal store is a brick or concrete building constructed to minimise draughts. It should have a low roof to minimise internal air space and be unheated. Under such conditions, bagged hydrate can be stored for a year without significant deterioration [21.1]. 

If hydrated lime is kept in a general store, care should be taken to ensure that it does not come into contact with other chemicals with which it might react. The sacks should be covered by an impervious sheet. 

Pallets of bagged hydrate have been stored successfully out-of-doors. The pallet is covered by a plastic sheet, the bags placed on the sheet and the pack shrink-wrapped. Such pallets should be moved into a covered store before unloading. 

Handling arrangements for bagged hydrate are usually quite basic, involving manual loading into a hopper with a screw or vibrating feeder arrangement to transfer the hydrate into the process. 

---

Automobile safety air bags use sodium azide [26628-22-8] NaN, for gas generation. It can be made from hydrazine by refluxing ethyl or Abutyl nitrite with hydrazine hydrate and sodium hydroxide in alcohol (209,210) ... 

In recent years, lime treatment has been advocated for corrosion control by removing lead and copper from distribution systems, mainly by raising the pH to around 7.5, which prevents these heavy metals from solubilizing. This type of treatment is appHcable to all water suppHes, and especially for small systems. Itinvolves the use of hydrated lime, generally deHvered in bags (see Water). 

Beryllium Nitrate. BeryUium nitrate tetrahydrate [13516-48-0], Be(N02)2 4H2O, is prepared by crystallization from a solution of beryUium hydroxide or beryllium oxide carbonate in a slight excess of dilute nitric acid. After dissolution is complete, the solution is poured into plastic bags and cooled to room temperature. The crystallization is started by seeding. Crystallization from more concentrated acids yields crystals with less water of hydration. On heating above 100°C, beryllium nitrate decomposes with simultaneous loss of water and oxides of nitrogen. Decomposition is complete above 250°C. 

Plutonium components, normally kept under argon, were accidentally exposed to air and moisture, probably forming plutonium hydride and hydrated oxides. When the plastics containing bag was disturbed, ignition occurred, causing widespread radiation contamination. 

Dampproofing admixtures are water-repelling materials such as wax emulsions, soaps and fatty acids which react with cement hydrates [84, 85]. The most widely used water-repelling materials are the calcium or ammonium salts of fatty acids such as stearates. Proprietary products are available both as dry powders and liquids. Usually, a stearate soap is blended with talc or fine silica sand and used at the prescribed dosage per weight or bag of cement. In commercial liquid preparations, the fatty-acid salt (soap) content is usually 20% or less, the balance of the solid material is made up of lime or CaCl2. Some proprietary admixtures combine two or more admixtures, e. 

Limewater is a saturated aqueous calcium hydroxide, Ca(OH)2, solution. To make limewater, a small amount of calcium hydroxide is needed. Calcium hydroxide is marketed commercially as slaked lime or hydrated lime. It is used for cement, increasing the pH in soils, and water treatment. Lime may be obtained from building material stores in the cement section and in agricultural stores. The smallest quantities sold are generally 5- or 10-pound bags, which cost a few dollars. Because only a teaspoon of lime is needed (the solubility of calcium hydroxide in water is 0. Ig per 100 mL), ask the sales clerk if there are any broken bags from which you can take a tablespoon of lime. Often there will be enough lime dust where it is stored to obtain an ample amount for this activity. 

The hydrated electron, if the major reducing species in water. A number of its properties are important either in understanding or measuring its kinetic behavior in radiolysis. Such properties are the molar extinction coefficient, the charge, the equilibrium constant for interconversion with H atoms, the hydration energy, the redox potential, the reaction radius, and the diffusion constant. Measured or estimated values for these quantities can be found in the literature. The rate constants for the reaction of Bag with other products of water radiolysis are in many cases diffusion controlled. These rate constants for reactions between the transient species in aqueous radiolysis are essential for testing the "diffusion from spurs" model of aqueous radiation chemistry. 

This same crystal, after it was used to determine the structure of hydrated Bag-A, was evacuated at 10 - Torr for 2 days at 50°C. While still in vacuum, it was sealed in its capillary with a torch. 

It is easy to distinguish Ba + ions from Na+ for several reasons. Firstly, their atomic scattering factors are quite different, 54 e for Ba2+ vs 10 e for Na+. Secondly, their ionic radii are quite different, Ba2+ = 1.34 X and Na = 0.97 X (5). Also, the approach distances between these ions and zeolite oxide ions in dehydrated Na 2 A (16) and hydrated Bag-A are known (see Table III). Finally, the requirement that 12 cationic charges be placed per unit cell does not allow the major positions to refine to acceptable occupancies with an alternative assignment of ionic identities. 

Figures 3 and 4 show plausible sodalite unit and large cavity structures which are consistent with the structural parameters determined for hydrated Bag-A.

The ion at Ba(4) is associated with 8-ring oxygens. This position is located on the plane of an 8-ring but is off its center to enable more favorable approaches to framework oxide ions (Ba(4)-0(1) = 2.88 A, and Ba(4)-0(2) = 2.92 A). These Ba-0 contact distances are again shorter than those in hydrated Bag-A (see Table III). The final Eg value, 0.042, and the unusually featureless final difference Fourier function suggest that little or no water is present in this crystal. 

Crystal stability is related to the amount of barium and water in the zeolite. Single crystal data by their number tend to indicate a decrease in the crystal quality of zeolite A at higher and lower H2O contents. Although hydrated Bag-A had... 

The structural basis for the instability may be found in the inability of Ba " " to adjust to low coordination numbers. Barium ions in naturally occurring minerals and oxides have coordination numbers ranging from 6 to 10 (21). Some Baz+ ions in hydrated Bag-A have a coordination number of 6, which, upon dehydration, would be reduced to 3, the partially Baz+-exchanged structures indicate, if dehydrated Bag-A were to form. 

The structural basis for the instability may be found in the greater tendency of Ba " ", compared to Ca2+ or Srz+ (4), to occupy 8-ring sites. Even evacuation of hydrated Bag-A at 50°C results in a BaZ+ ion in every 8-ring. Simultaneously, of course, fewer Ba2+ ions are available to occupy 6-ring sites, which are too small to accommodate such large cations anyway. 

In contrast, yellow iron oxide begins to lose its water of hydration above 177°C and converts to Fe203. Consequently, its use in plastics is limited to low-temperature processes. It is well suited for weatherable flexible vinyl applications. At one time, truckloads of yellow iron oxides were used in the coloration of low-density polyethylene disposable green garbage bags. 

Neutralizing a spill often consists of mixing fnll-strength bleach with hydrated lime and working this mixture into the spill site with a coarse broom. Fresh absorbent material is then spread over the spill site to soak np the nen-tralizing liquid. This material is swept up and placed in a plastic drum or bag for disposal. You may be instructed to repeat the process several times to make sure that the site is thoroughly neutralized. 

The method outlined here uses a modification of the Hedley technique (9,10) to prepare nuclear suspensions from the paraffin-embedded tissue samples. Microtome sections are dewaxed, hydrated, and incubated in pepsin with intermittent vortexing and mechanical disruption to release the nuclei. After completion of the tissue digestion, the nuclei are either suspended in 70% ethanol for storage or stained with propidium iodide (PI) for FCM analysis. There are three alternative techniques for preparation of the nuclei on microslides, in tea bags, or in test tubes. 

---