Annoucement : Welcome to visit our website, Any inquiry, please check CONTACT US. Payment related business, please confirm with our salesman, Have a nice visit trip.
EnglishViews: 2 Author: Site Editor Publish Time: 2023-04-25 Origin: Site
Ferrous chloride is an inorganic substance with the chemical formula FeCl2. green to yellow in color. It is soluble in water, ethanol and methanol. There is the tetrahydrate FeCl2-4H2O, which is a transparent blue-green monoclinic crystal. Density 1.93 g/cm3, easily deliquescent, soluble in water, ethanol, acetic acid, slightly soluble in acetone, insoluble in ether. Anhydrous ferrous chloride is a yellow-green hygroscopic crystal, forming a light green solution after dissolving in water. It is a tetrahydrate salt and becomes a dihydrate salt when heated to 36.5℃.
Ferrous chloride is white or gray-green crystals. It is easily hygroscopic. It is easily oxidized in air and gradually turns yellow, and sublimates at about 700°C in the hydrogen chloride stream. Easily soluble in water, methanol, ethanol, slightly soluble in acetone and benzene, insoluble in ether.
FeCl2-4H2O is a blue-green monoclinic crystal. Density 4.93g/cm3. easily deliquescent. Soluble in water, ethanolacetic acid slightly soluble in acetone insoluble in ether in air gradually oxidized to alkaline ferric chloride. Anhydrous ferrous chloride is yellow-green hygroscopic crystals dissolved in water to form a light green solution.
1. Will not decompose if used and stored according to specifications.
2. Avoid contact with oxides, moisture/moisture. Freely soluble in water, methanol, ethanol, slightly soluble in acetone and benzene, insoluble in ether. Sublimates when heated to about 700°C in a stream of hydrogen chloride (vapor pressure 1599 .8Pa). Soluble in water, ethanol and acetone; insoluble in ether, slightly soluble in benzene. Generates ferric chloride and iron oxide when heated in air.
1. Keep the receptacle sealed.
2. Put into tight receptacles and store in a cool, dry place.
1. In a solution with a certain concentration of hydrochloric acid, gradually add a certain amount of iron filings to the reaction. Equation: Fe + 2HCl == FeCl2 + H2↑ After cooling, filtering, adding a little washed iron in the filtrate to prevent the generated ferrous chloride from being oxidized, evaporating the filtrate until crystallization occurs, filtering while hot, cooling crystallization, solid-liquid separation, and rapid drying to produce.
2. Put anhydrous ferric chloride in a rigid glass tube quickly, pass the dried hydrogen gas from one end of the tube, fully replace the air inside the tube, then heat the reaction tube, the other end of the tube will have a large amount of hydrogen chloride discharge, which can be absorbed into dilute hydrochloric acid with water. When the release of hydrogen chloride slows down and the ferric chloride turns into white crystals, the reaction is completed, stop heating, and bring the product in the tube to room temperature in a weak hydrogen flow. The reaction tube is closed and stored, and then quickly filled into the packaging container to produce anhydrous ferrous chloride.
3. You can first synthesize anhydrous ferric chloride with iron and chlorine (refer to the synthesis of FeCl3). Load FeCl3 according to the original device, replace the chlorine gas with nitrogen, and then pass into the dry pure hydrogen, heated to 300 ~ 350 ℃ for reduction. As FeCl3 chloride below 300 ℃ will still sublimate, while above 350 ℃ is FeCl3 is reduced to metallic iron, so you need to use a longer reaction tube and electric furnace, and should pay strict attention to the hydrogen flow rate and temperature regulation.
4. In a three-necked flask, put 162g of anhydrous ferric chloride and 225g of chlorobenzene, and then install a thermometer, reflux condenser and powerful stirrer. Then absorb the generated hydrogen chloride with water and titrate with 2 mol/L sodium hydroxide solution. The material was first stirred vigorously and heated at 126°C for 30 min, and then turned into a black sludge. However, when this state was reached, only 1 mL of 2 mol/L sodium hydroxide solution was consumed, and then the solution was heated at 128-139°C for 2 h. The solution gradually became lighter in color and less viscous, and the 2 mol/L sodium hydroxide solution consumed at this time was approximately close to the theoretical value (250 mL). After continued heating for 1h, the solution was left to cool, and the solid was filtered out under air isolation, washed several times with chloroform or benzene, and then dried in vacuum. The yield is 99%. The product should be stored away from air and moisture.
Reducing agent. Detection of selenium. Sewage treatment agent.
Directly used in sewage and wastewater treatment, as reducing agent and mordant, widely used in fabric printing and dyeing, pigment dyeing, manufacturing and other industries, and also used in ultra-high pressure lubricant components, also used in medicine, metallurgy and photographic.
Ferrous chloride has unique decolorization ability and is suitable for wastewater treatment in dyeing and dyestuff intermediates, printing and dyeing, and paper industries. It can simplify the water treatment process, shorten the water treatment cycle and reduce the cost of water treatment; it has obvious treatment effect on all kinds of sewage, electroplating, leather and paper wastewater, and the removal rate of all kinds of heavy metal ions in wastewater and sewage is close to 100%; the treatment cost is low and it is a more ideal agent for sewage treatment. Directly used in sewage, wastewater treatment, as a reducing agent and mordant, widely used in fabric printing and dyeing, pigment printing and dyeing, manufacturing and other industries, together with the also used in ultra-high pressure lubricant components, and used in medicine, metallurgy and photographic.
Take 1ml specimen in 300ml triangular flask, add 100ml distilled water, 25ml sulfur phosphorus mixed acid, 5-6 drops of sodium diphenylamine sulfonate indicator, titrate with potassium dichromate standard solution until the solution changes from colorless to purple as the end point.
Steps
1. Preparation
Weigh 11.7672g of potassium dichromate dried at 120℃ for 4h in a 1L volumetric flask, add 100mL of distilled water, shake well until dissolved, then dilute to the scale with distilled water.
2. Calibration
Take 25.00ml of potassium dichromate standard solution in 250ml volume, add 10ml of 50% sulfuric acid, 15ml of 20% potassium iodide, place in the dark for 5 minutes, remove and add 100ml of distilled water, immediately drop to light yellow with sodium thiosulfate solution. Then add 2m10.5% starch solution, titrate until the blue just disappears and light green, that is the end point.
3. Calculation
Where: C(K2Cr2O7)-material concentration of potassium dichromate, mol/L
C(Na2S2O3)-material concentration of sodium thiosulfate solution, mol/L
V(K2Cr2O7)-the amount of potassium dichromate solution when measured, ml
V(Na2S2O3)-the amount of sodium thiosulfate solution consumed during titration, ml
