Sodium chloride reactions forming

Step C Preparation ofthebase-A 300 ml one-necked, round-bottomed flask, equipped with a water-cooled condenser, calcium chloride tube and magnetic stirrer is charged with anhydrous methanol (150 ml) and sodium metal (5.75 g,0.25 g atom). When the reaction is complete, the solution is treated with dry guanidine hydrochloride (26.3 g, 0.275 mol) and stirred for 10 minutes. The sodium chloride that forms is removed by filtration. The solution is concentrated in vacuo to a volume of 30 ml and the residue treated with the product of Step B, heated one minute on a steam bath and kept at 25°C for 1 hour. The product is filtered, washed well with water, dissolved In dilute hydrochloric acid and the free base precipitated by addition of sodium hydroxide to give the amllorlde product base, a solid which melts at 240.5°-241.5°C. 

A solid that contains cations and anions in balanced whole-number ratios is called an ionic compound. Sodium chloride, commonly known as table salt, is a simple example. Sodium chloride can form through the vigorous chemical reaction of elemental sodium and elemental chlorine. The appearance and composition of these substances are very different, as Figure 2-24 shows. Sodium is a soft, silver-colored metal that is an array of Na atoms packed closely together. Chlorine is a faintly yellow-green toxic gas made up of diatomic, neutral CI2 molecules. When these two elements react, they form colorless ciystals of NaCl that contain Na and Cl" ions in a 1 1 ratio. 

The main cell reaction involves chlorination of high surface area nickel powder with sodium chloride to form the nickel chloride positive electrode and sodium ... 

Except for the inert gases, atoms tend to interact with other atoms to form molecules. Hydrogen, oxygen, and nitrogen each readily form simple diatomic molecules. Invariably, molecules have properties that are quite different from those of the constituent elements. For example, a molecule of sodium chloride contains one atom of sodium (Na) and one atom of chlorine (Cl). Sodium is a highly reactive silvery metal, whereas chlorine is a corrosive yellow gas. When equal numbers of Na and Cl atoms interact, vigorous reaction occurs and white crystalline solid sodium chloride is formed. 

After the flask containing the sodium borohydride solution has cooled for about half an hour, the tributyltin chloride solution is added dropwise with rapid stirring over a 30-minute period. A white sodium chloride precipitate forms as each drop of the tributyltin chloride solution is added. The reaction mixture is allowed to stand at —10 to — 11°C. for 10-15 minutes after the last of the tributyltin chloride solution has been added. Without filtration, the entire reaction mixture is now transferred cold under nitrogen or helium into a 1-1., single-necked, round-bottomed flask the flask is attached to a flash evaporator (Buchler Model PTFE-1G or equivalent) and immersed in a bath maintained at 0°C. The evaporator s receiving flask (also 1-1., single-necked, round-bottomed) is immersed in a — 80°C. bath of Dry Ice-acetone. 

The equation representing the reaction in which sodium chloride is formed from sodium and chlorine may be easily written. It is... 

The number in front of the formula for water and also in front of the formula for table salt indicates the number of units of each that enter into the reaction. Two water molecules react with two units of sodium chloride to form one unit of sodium hydroxide, one molecule of chlorine gas, Clj, and one molecule of hydrogen gas, Hj. In other words, if we were to write each reactant individually, the reaction would be... 

You already know that atoms with very different electronegativities bond by an electron transfer. For example, sodium chloride is formed by the transfer of electrons from sodium atoms to chlorine atoms in the reaction shown in Figure 1 and described by the following equation ... 

In the modern process for making sodium hydroxide, an electric current is run through a sodium chloride solution, forming hydrogen and chlorine along with the sodium hydroxide. Both sodium chloride and water are reactants. Write a balanced equation, without including states, for this reaction. 

All of the equations for the Solvay process described in problem 70 can be summarized by a single equation, called a net equation, that describes the overall change for the process. This equation shows calcium carbonate reacting with sodium chloride to form sodium carbonate and calcium chloride. Write a balanced equation, without including states, for this net reaction. 

As we saw in Chapter 3, this transfer of electrons from metal atoms to nonmetal atoms is the general process for the formation of any binary ionic compound from its elements. For example, when sodium chloride is formed from the reaction of metallic sodium with gaseous chlorine, each sodium atom loses an electron, and each chlorine atom gains one. 

Similarly, sodium chloride is formed in the absorber by the reaction of chloride, present in the flue gas as HC1 vapor, with the alkaline sodium solutions. The level of sodium chloride in the system builds up to a steady state concentration, such that the rate at which sodium chloride leaves the system with the washed filter cake is equivalent to the rate at which it is absorbed by the process liquor in the absorber. 

In the synthesis of phenylacetic acid, the Pd-TPPTS system was used as a catalyst by Kohlpaintner and Beller (Hoechst) [15] in a biphasic carbonylation of benzyl chloride as a greener alternative to the classical process the reaction of benzyl chloride with sodium cyanide (Equations 4.4 and 4.5). Although in the new process 1 equiv. of sodium chloride is formed, this is far less salt waste than in the original process. Moreover, sodium cyanide is about seven times more expensive per kilogram than carbon monoxide. 

CAPBs is typically below 0.3%, which is normally achieved by controlling the reaction pH. The dimethyl aminoamine content is controlled to be below 15 ppm, which is regarded as safe. Sodium chloride is formed as the main by-product, and is present in most betaine solutions in concentrations of about 5%. Typically, the salt is left in the surfactant solution as it has no negative side effects for most applications. It is even desirable for the enhancement of viscosity in ready-to-use preparations such as shampoos. 

This process is cheaper than the transesterification and leads to higher molar masses. But it is difficult to remove the sodium chloride also formed from the product, by, for example, extrusion volatilization. The Schotten-Baumann reaction is carried out either in organic solvents (aromatics, chlorohydro-carbons) with addition of acceptors (pyridine, /-amines) or in aqueous alkali under addition of water-insoluble organic compounds otherwise high molar masses are not obtained. 

Sodium chloride, NaCl, formed by the reaction of hydrochloric acid with sodium hydroxide ... 

Hunter process. As initiaUy practiced at General Electric (GE) in 1910 by Mathew A. Hunter, the Hunter process reacted titanium tetrachloride with elemental sodium in an inert-gas atmosphere in a sealed steel retort at a temperature of about 900 C. Titanium sponge and molten sodium chloride are formed upon completion of the reaction ... 

Mercury(I) ions (Hg2 ) can be removed from solution by precipitation with Q . Suppose a solution contains aqueous Hg2(N03)2- Write complete ionic and net ionic equations to show the reaction of aqueous Hg2(N03)2 with aqueous sodium chloride to form solid Hg2Cl2 and aqueous sodium nitrate. 74. Lead ions can be removed from solution by precipitation with sulfate ions. Suppose a solution contains lead(II) nitrate. Write a complete ionic and net ionic equation to show the reaction of aqueous lead(II) nitrate with aqueous potassium sulfate to form solid lead(II) sulfate and aqueous potassium nitrate. 

EXAMPLE 8.1 Mole-to-Mole Conversions Sodium chloride, NaCl, forms by this reaction between sodium and chlorine. 2 Na(s) + Cl2(y) > 2 NaCl(s) How many moles of NaCl result from the complete reaction of 3.4 mol of CI2 Assume that there is more than enough Na. ... 

A chemist combines 11 grams of sodium with 14 grams of chlorine. A spectacular reaction occurs and produces sodium chloride. After the reaction, the chemist finds that all the chlorine was used up by the reaction, but 2 grams of sodium remained. How many grams of sodium chloride were formed ... 

In the chlorohydrination step, the reactants propylene and hypochlorous acid (chlorine and water) are converted into two propylene chlorohydrin isomers (90% l-chloro-2-propanol and 10% 2-chloro-l-propanol). Yields of up to 94% can be achieved in modern commercial plants. The main by-products formed in this reaction step are dichloropropane (3-10%), dichloropropanol (0.3-1.2%), and dichlorodiisopropyl ether (0.2-1.7%). In the second step (dehydrochlorination, also called epoxidation or saponification ) the aqueous propylene chlorohydrin solution is treated with slaked lime or caustic soda. Propylene oxide and calcium or sodium chloride are formed. In a commercial process 1.4-1.5 units of chlorine are consumed to produce one unit of propylene oxide. Typical by-products are monopropylene glycol, epichlorohydrin, glycerol monochlorohydrin, glycerol, propanal, and acetone. In dehydrochlorination, propylene oxide yields of up to 96% can be obtained. 

The combined mass of the sodium and chlorine that react (the reactants) exactly equals the mass of the sodium chloride that forms (the product). This law is consistent with the idea that matter is composed of small, indestructible particles. The particles rearrange during a chemical reaction, but the amount of matter is conserved because the particles themselves are indestructible (at least by chemical means). 

Mercury(I) ions (Hg2 ) can be removed from solution by precipitation with CF. Suppose that a solution contains aqueous Hg2(N03)2. Write complete ionic and net ionic equations to show the reaction of aqueous Hg2(N03)2 with aqueous sodium chloride to form solid Hg2Cl2 and aqueous sodium nitrate. 

A reaction between sodium hydroxide and hydrogen chloride gas produces sodium chloride and water. A reaction of 22.85 g of sodium hydroxide with 20.82 g of hydrogen chloride gives off 10.29 g of water. What mass of sodium chloride is formed in the reaction ... 

The high sodium ion concentration results in facile crystallisation of the sodium salt. This process of salting out with common salt may be used for recrystallisation, but sodium benzenesulphonate (and salts of other acids of comparable molecular weight) is so very soluble in water that the solution must be almost saturated with sodium chloride and consequently the product is likely to be contaminated with it. In such a case a pure product may be obtained by crystallisation from, or Soxhlet extraction with, absolute alcohol the sul-phonate is slightly soluble but the inorganic salts are almost insoluble. Very small amounts of sulphones are formed as by-products, but since these are insoluble in water, they separate when the reaction mixture is poured into water ... 

A sodium stannite solution was prepared by addition of aqueous sodium hydroxide (2.5 mol, lOOg) to aqueous stannous chloride (0.25 mol, 56g). The initially formed precipitate redissolved to form a clear solution. This solution was gradually added to a solution of 16.3g (0.1 mol) phenyl-2-nitropropene in THF at room temperature. A slightly exothermic reaction ensued, and the reaction mixture was stirred for 30 min, a saturated sodium chloride solution was added, and the solution was extracted with ether and the pooled extracts were evaporated under vacuum to give essentially pure P2P oxime in 80% yield. 

The acetonitrile and mercuric nitrate amounts remain the same except they are to be accompanied by 12.6g of fuming nitric acid (see chemicals section) in the reaction flask. Then, with cooling, the safrole or allylbenzene is added just like before. The reaction is immediate and takes no more than 20 minutes of stirring after which lOOmL ice cold dH20 is slowly added. Next, with vigorous stirring, saturated sodium chloride solution is slowly added until a pronounced precipitate forms. This yellowish mass is the chloride. 

Acetaldehyde reacts with phosphoms pentachloride to produce 1,1-dichloroethane [75-34-3] and with hypochlorite and hypoiodite to yield chloroform [67-66-3] and iodoform [75-47-8], respectively. Phosgene [75-44-5] is produced by the reaction of carbon tetrachloride with acetaldehyde in the presence of anhydrous aluminum chloride (75). Chloroform reacts with acetaldehyde in the presence of potassium hydroxide and sodium amide to form l,l,l-trichloro-2-propanol [7789-89-1] (76). 

Acetaldehyde can be isolated and identified by the characteristic melting points of the crystalline compounds formed with hydrazines, semicarbazides, etc these derivatives of aldehydes can be separated by paper and column chromatography (104,113). Acetaldehyde has been separated quantitatively from other carbonyl compounds on an ion-exchange resin in the bisulfite form the aldehyde is then eluted from the column with a solution of sodium chloride (114). In larger quantities, acetaldehyde may be isolated by passing the vapor into ether, then saturating with dry ammonia acetaldehyde—ammonia crystallizes from the solution. Reactions with bisulfite, hydrazines, oximes, semicarb azides, and 5,5-dimethyl-1,3-cyclohexanedione [126-81 -8] (dimedone) have also been used to isolate acetaldehyde from various solutions. 

This carbon dioxide-free solution is usually treated in an external, weU-agitated liming tank called a "prelimer." Then the ammonium chloride reacts with milk of lime and the resultant ammonia gas is vented back to the distiller. Hot calcium chloride solution, containing residual ammonia in the form of ammonium hydroxide, flows back to a lower section of the distiller. Low pressure steam sweeps practically all of the ammonia out of the limed solution. The final solution, known as "distiller waste," contains calcium chloride, unreacted sodium chloride, and excess lime. It is diluted by the condensed steam and the water in which the lime was conveyed to the reaction. Distiller waste also contains inert soHds brought in with the lime. In some plants, calcium chloride [10045-52-4], CaCl, is recovered from part of this solution. Close control of the distillation process is requited in order to thoroughly strip carbon dioxide, avoid waste of lime, and achieve nearly complete ammonia recovery. The hot (56°C) mixture of wet ammonia and carbon dioxide leaving the top of the distiller is cooled to remove water vapor before being sent back to the ammonia absorber. 

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