اسماء المواد التي تستخدم في المتفجرات جديد ومهم

[معمر القذافى]

الرقم الاسم بالعربي الاسم بالإنجليزي الرمز أماكن وجوده او التحضير

1 حامض الكبريتيك Sulphuric acid H2SO4 تركيز ماء البطارية-أو مختبرات
2 حامض النيتريك Nitric acid HNO3 تفاعل النترات مع حمض الكبريتيك
3 نترات الامونيوم Ammonium nitrate NH4NO3 سماد زراعي "تركيز من 32% إلى 34%
تفاعل غاز الامونيا مع حمض النيتريك

4 نترات البوتاسيوم POTASSIUM NITRATE KNO3 سماد زراعي
تستخرج من روث الماعز
5 نترات الصوديوم SODIUM NITRATE NaNO3 تفاعل ملح الطعام مع حمض النيتريك
6 نترات الرصاص LEAD NITRATE Pb(NO3)2 تفاعل الرصاص مع حامض النيتريك
7 نترات الباريوم Barium nitrate BaNO3 تفاعل الباريوم مع حامض النيتريك
8 نترات اليوريا Urea nitrate Co(NO3)2 تفاعل اليوريا مع حامض النيتريك
9 حامض الليمون Citric acid C6H8O7 يباع في البقالات
10 حامض الهيدروكلوريك Hydrochloric acid HCl منظف الحمامات يباع في البقالات
11 حامض الخلليك Acetic acid C2H4O2 تركيز الخل
12 حامض الهيدروزيك Hydrozic acid HN3 اكسد الهيدرازين باستعمال H2O2
13 كبريتات النحاس Copper sulfate CuSO4 تفاعل النحاس مع حامض الكبريتيك
14 كبريتات البوتاسيوم Potassium sulfate K2SO4 تفاعل هدروكسيد البوتاسيوم مع حامض الكبريتيك
15 كبريتات الألمنيوم Alluminum solfate Al2(SO4)3 (تسمى الشبة) أو
تفاعل الألمنيوم مع حامض الكبريتيك
16 كبريتات الصوديوم Sodium sulfate Na2SO4 تفاعل الصوديوم مع حامض الكبريتيك
17 كبريتات الصوديوم Sodium sulfite Na2SO4 تستخدم لإزالة الألوان بعد التبييض
18 كبريتيت هيدروجين الصوديوم Sodium hydro sulfite NaHSO3 تستخدم في عملية التحميض كمثبت
19 كلوريد البوتاسيوم Potassium chloride KCl الملح البديل لأمراض الضغط الدموي
20 كلوريد الامونيوم Ammonium chloride NH4Cl تفاع لحمض الكلوردريك والامونيا
21 كلوريد الصوديوم Sodium chloride NaCl ملح الطعام
22 كلورات البوتاسيوم Potassium chloride KCLO3 مبيد الاعشاب الضارة
يحضر بأكسدة كلوريد البوتاسيوم
23 كلورات الصوديوم Sodium chlorate NaCLO3 يحضر بأكسدة كلوريد الصوديوم
24 الزئبق Mercury Hg تستعمل في موازين الحرارة. أو عند العشابين "السحر"
25 أزيد الصوديوم Soduim azid NaN3 معامل المحاليل الطبية
26 اليود Iodine I الصيدليات كمطهرالجروح
27 هيدروكسيد الامونيا Ammonium hydroxide NH4OH يباع ف الصيدليات ويستعمل في صبغة الشعر
يحضر من نترات المنيوم
28 هيدروكسيد الصوديوم Soduim hydroxide NaOH صود الغسيل. أو
يحضر من ملح الطعام
29 هيدروكسيد البوتاسيوم
Potassium hydroxide KOH صناعة الصابون السائل
30 بروكسيد الهيدروجين Hydrogen peroxide H2O2 يباع في الصيدليات كمطهر أو يستعمل لصبغ الشعر
31 الأسيتون ِAcetone C3H6O مذيب صباغة الاظافر
32 الهكسامين Hexamine C6H12N4 دواء للمسالك البولية
الفحم الابيض
33 اليوريا Urea Co(NH2)2 سماد زراعي 46%-
34 بودرة ألمنيوم Alluminum powder Al في محلات بيع زيوت الدهان
35 بودرة المغنسيوم Magnesium Mg يستخدم في صناعة التماثيل
36 بودرة الكبريت Sulfur powder S في محلات بيع مواد الزراعة
37 بودرة الفحم Charcoal powder C6H2O بعد حرق الأخشاب
38 معدن الصوديوم Soduim ****l Na بواسطة التحليل الكهربي لملح الطعام
39 معدن الفسفور Phosphorous P4 يدخل في صناعة سموم الحشرات
40 معدن الزنك Zinc powder Zn يستخدم في الطلاء
41 سداسي كلوروايثان Hexachloroethane C2Cl6 يحضر بكلورة الايثان
42 بارانيتروانلين pranitroanaline C6H4NH2(NO2) يحضر بنترجة الانيلين
43 الانيلين aniline C6H5NH2 يستخدم في الصباغة* ويحضر من البنزين
44 التلوين toluene C6H5CH3 يستخدم في الدهان وصناعة الصمغ
45 أكسيد الحديدوز ferrous oxide Fe2O3 من صدأ الحديد الأسود المغناطيس
46 أكسيد الحديديك ferric oxide Fe3O4 من صدأ الحديد الأحمر العادي
47 أكسيد الباريوم Barium oxide BaO بأكسدة عنصر الباريوم
48 انهيدرس هيدرازين anhydrous hydrazine N2H4 تفاعل غاز الامونيا مع هيبوكلوريت
49 هيدرازين هيدرات hydrazine hydrate N2H5OH الصوديوم في وجود جلائين وأسيتون
50 الكحول الايثيلي ethyl alcohol C2H5OH الكحول الطبي العادي
الصيدليات
51 الكحول الميثيلي methyl alcohol CH3OH المختبرات
52 الفينول phenol C6H5OH في الصيدليات يحضر من الأسبرين
53 الفانفتول phanphthol C10H8O يستعمل في الصباغة وضد التأكسد
54 الجلسرين gylycerine C3H5(OH)3 في الصيدليات لتليين الجلد "مرطب"
55 الجليكول glycol C2H8O2 تركيز سائل تبريد محرك السيارات
56 اوكسلات الامونيوم ammonium oxalate C2H8N2O4 يستخدم كمثبت للخلائط الكيميائية
57 برمنجنات البوتاسيوم potassium permanganate KMNO4 من الصيدليات ويستخدم لتطهير المياه. دواء للامراض الجلدية
58 النتروبنزين nitro benzene C6H5NO2 منظف لآلة التصوير ويحضر من البنزين
59 كربونات الصوديوم sodium carbonate Na2CO2 محلات البقالة صودا طعام
60 بيكربونات الصوديوم sodium bicarbonate NaHCO3 محلات البقالة صناعة الحلوى "خميرة الحلوى"
61 برافين(زيت) paraffin * الصيدليات كمسهل قبل العمليات
62 نترات الفضة silver nitrate AgNO3 في التصوير الفوتوغرافي
تفاعل الفضة مع النتريك
63 نفتالين naphthalene C10H8 الكافور لحفظ الملابس والفراش
64 فازلين vaseline C15H32 الصيدليات البقالات. "مرطب اليدين"



وهته الائحة مفصلة في "م. أبو خباب المصري" .

تحضير نترات الفضة: 25
كبريتات النحاس: 25
غاز الأستلين: 25
تصنيع الصودا الكاوية 26
NH3 تحضير الأمونياك 28
تحضير ماء الجير 30
تحضير الھيدرازين: 30
تحضير أكسيد الحديد : 31
تعريف الثرميت: 32
الحصول على بودرة الألمنيوم: 32


روابط تحميل خباب المصري

ليس لديك تصريح لمشاهدة الرابط، فضلا قم ب تسجيل الدخول او تسجيل

ليس لديك تصريح لمشاهدة الرابط، فضلا قم ب تسجيل الدخول او تسجيل

ليس لديك تصريح لمشاهدة الرابط، فضلا قم ب تسجيل الدخول او تسجيل

ليس لديك تصريح لمشاهدة الرابط، فضلا قم ب تسجيل الدخول او تسجيل

ليس لديك تصريح لمشاهدة الرابط، فضلا قم ب تسجيل الدخول او تسجيل

ليس لديك تصريح لمشاهدة الرابط، فضلا قم ب تسجيل الدخول او تسجيل

منقول طبعا من شبكة معارك سلفيه باركهم الله​

 

[معمر القذافى]

هته مجموعة باللغة الإنجليزية
Chemical *****alency list:
Acacia............................................ ....................Gum Arabic
Acetic Acid.............................................. ................Vinegar
Aluminum Oxide............................................. ...............Alumia
Aluminum Potassium Sulphate.......................................... .......Alum
Aluminum Sulfate........................................... .................Alum
Ammonium Carbonate......................................... ............Hartshorn
Ammonium Hydroxide......................................... ..............Ammonia
Ammonium Oleate............................................ .........Ammonia Soap
Amylacetate....................................... ....................Banana Oil
Barium Sulfide........................................... ..............Black Ash
Carbon Carbinate......................................... ..................Chalk
Carbontetrachloride............................... ................Cleaning Fluid
Calcium Hypochloride...................................... ......Bleaching Powder
Calcium Oxide............................................. ..................Lime
Calcium Sulfate........................................... ......Plaster of Paris
Carbonic Acid.............................................. ..............Seltzer
Cetyltrimethylammoniumbromide..................... .................Ammonium Salt
Ethylinedichloride................................ ...................Dutch Fluid
Furfuraldehyde.................................... ......................Bran Oil
Glucose........................................... ....................Corn Syrup
Graphite.......................................... ...................Pencil Lead
Hydrochloric Acid.............................................. ....Muriatic Acid
Hydrogen Peroxide.......................................... .............Peroxide
Lead Acetate........................................... ............Sugar of Lead
Lead Tero-oxide............................................. ............Red Lead
Magnesium Silicate.......................................... ................Talc
Magnesium Sulfate........................................... ..........Epsom Salt
Methylsalicylate.................................. ..............Winter Green Oil
Naphthalene....................................... .....................Mothballs
Phenol............................................ .................Carbolic Acid
Potassium Bicarbonate....................................... .....Cream of Tarter
Potassium Chromium Sulfate........................................... .Chromealum
Potassium Nitrate........................................... ..........Salt Peter
Sodium Oxide............................................. ...................Sand
Sodium Bicarbonate....................................... ............Baking Soda
Sodium Borate............................................ ..................Borax
Sodium Carbonate......................................... ...........Washing Soda
Sodium Chloride.......................................... ...................Salt
Sodium Hydroxide......................................... ....................Lye
Sodium Silicate.......................................... ..................Glass
Sodium Sulfate........................................... .........Glauber's Salt
Sodium Thiosulfate....................................... ....Photographer's Hypo
Sulfuric Acid.............................................. .........Battery Acid
Sucrose........................................... ....................Cane Sugar
Zinc Chloride.......................................... ...........Tinner's Fluid
Zinc Sulfate........................................... ............White Vitriol






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هذه مجموعة من المواد الأولية وكيفية تصنيعها بالتفصيل -اللغة الإنجليزية-
Chemical preparation and sources:
6.1 Ammonium chloride:
Formula: NH4Cl
Description: Ammonium chloride is used in smoke compositions. When heated ammonium chloride decomposes to HCl and NH3, both gasses. These recombine in the air to give a smoke consisting of fine particles of ammonium chloride.
Hazards: Ammonium chloride based smoke is irritating to the eyes and lungs as it contains some remaining HCl and NH3. Ammonium chloride itself is not poisonous and is even used in some type of candy. According to Shimizu ammonium chloride forms an exception to the rule that ammonium compounds should not be mixed with chlorates. Due to the lower solubility of potassium chlorate (compared to ammonium chlorate) no ammonium chlorate . I personally would still use these mixtures with great caution (or avoid them) since it seems inevitable that small amounts of ammonium chlorate will still form. The lower solubility of potassium chlorate will make it the -main- product in a double decomposition reaction but not the -only- product.
Sources: Ammonium chloride solution is easily prepared by neutralising ammonia solution with hydrochloric acid. It is advised to use a slight excess of ammonia. That is to make sure no remaining acid will be present in the ammonium chloride obtained on evaporation and crystallisation. Otherwise traces of the acid solution may be enclosed in the crystals, possibly leading to spontaneous ignition of mixtures made with it.
6.2 Ammonium nitrate:
Formula: NH4 NO3
Description: Ammonium nitrate is an oxidiser. It is very hygroscopic and therefore not used very often in fireworks. It finds some use in composite propellants, but performance is not as good as perchlorate based propellants.
Hazards: Large masses of ammonium nitrate have been known to explode on some occasions although it is very unsensitive. Smaller quantities are less likely to detonate. The risk of detonation increases when ammonium nitrate is molten or mixed with fuels such as ****l powders or organic substances. Ammonium nitrate should never be mixed with chlorates as this may result in ammonium chlorate formation, possibly leading to spontaneous ignition. Mixtures of ****l powders and ammonium nitrate are likely to heat up spontaneously and may ignite, especially when moist. This can sometimes be prevented by the addition of small amounts of boric acid (1 to 2%), but in general it is better to avoid these mixtures at all. The hygroscopic nature of ammonium nitrates makes this problem worse.
Sources: Ammonium nitrate solution can be prepared by neutralising ammonia solution with nitric acid. It is advised to use a slight excess of ammonia. That is to make sure no remaining acid will be present in the ammonium nitrate obtained on evaporation and crystallisation. Otherwise traces of the acid solution may be enclosed in the crystals, possibly leading to spontaneous ignition of mixtures made with it. Large quantities of ammonium nitrate can also be cheaply bought as fertilizer. In the Netherlands a fertilizer called 'kalkammonsalpeter' is sold. This consists of ammonium nitrate mixed with 'mergel', a mineral consisting mainly of calcium carbonate. The ammonium nitrate can be extracted with water.
6.3 Ammonium perchlorate:
Formula: NH4ClO4
Description: Ammonium perchlorate is an oxidiser used in a large number of compositions. Very impressive color compositions can be made with it, but their burn rate is often too low for use in star compositions. For lancework and torches slow burning is an advantage and it is therefore commonly used in these items. Ammonium perchlorate is also used in composite rocket propellants, including the propellants used in the solid propellant boosters used for the space shuttle. The decomposition products of ammonium perchlorate are all gasses which is very beneficial for rocket propellants.
Hazards: Ammonium perchlorate can detonate by itself, although it is not very sensitive. Larger amounts and mixtures of ammonium perchlorate with ****l powders or organic substances are more likely to detonate.
Sources: Ammonium perchlorate is usually bought from chemical suppliers or from dedicated pyro suppliers. Fine ammonium perchlorate powder is a regulated substance in most countries and cannot easily be bought or transported. Since it is such a usefull chemical in pyrotechnics it can be worth the time and effort to try to prepare it at home. This can be done by first making sodium perchlorate followed by double decomposition with ammonium chloride (other ammonium compounds can be used). The preparation of sodium perchlorate is most easily accomplished by electrolysis, the procedure for which is described elsewhere on this page.
6.4 Barium carbonate:
Formula: BaCO3
Description: Barium carbonate is used both in white and green color compositions. When chlorine donors are present in a composition a green color will result from the formation of BaCl+ in the flame. Without chlorine donors BaO will be formed which emits white light. Barium carbonate is convenient to use in chlorate based color compositions since it will neutralize residual acid which reduces the risk of spontaneous ignition.
Hazards: Most barium compounds are very poisonous, especially the more soluble barium compounds such as the chlorate and nitrate. A dust mask should be worn at all times when working with barium carbonate.
Sources: Barium carbonate is cheaply available in kilogram quantities from ceramic supply shops. However, this material is often contaminated with small amounts of barium sulfide which are left over from the production process. Therefore, ceramics grade barium carbonate should never be used in mixtures incompatible with sulfides such as chlorate based mixtures. Barium carbonate is not easily made at home.
6.5 Barium chlorate:
Formula: BaClO3
Description: Barium chlorate is used as an oxidiser in green color compositions. Fierce burning and high color purity compositions can be made with it.
Hazards: Barium chlorate is poisonous and a dust mask should be worn at all times when handling it. Barium chlorate should never be mixed with sulfur or sulfides or allowed to come in contact with mixtures containg sulfur or sulfides since this could result in spontaneous ignition. (Sulfur reacts with water and air to form small amounts of sulfuric acid. Sulfuric acid and chlorates react producing ClO2, an explosive gas which will ignite many organic materials on contact). Mixtures made with barium chlorate are often especially sensitive to friction and shock (even more so than potassium chlorate based mixtures) and should be handled with extra care.
Sources: Barium chlorate is usually purchased from chemical suppliers or from dedicated pyro suppliers. It can be made at home from sodium chlorate and barium chloride by double decomposition. Barium chlorate can also be prepared from barium chloride by electrolysis in a process analogous to that used for preparing sodium chlorate.
6.6 Barium nitrate:
Formula: BaNO3
Description: Barium nitrate is used as an oxidiser in both white and green color compositions. When chlorine donors are present in a composition a green color will result from the formation of BaCl+ in the flame. Without chlorine donors BaO will be formed which emits bright white light. Barium nitrate is seldom used as the sole oxidiser in green color compositions. It is usually combined with perchlorates to improve the color and increase the burning rate.
Hazards: Barium nitrate is poisonous and a dust mask should be worn at all times when handling it. Mixtures of ****l powders and barium nitrate sometimes heat up spontaneously and may ignite, especially when moist. This can usually be prevented by the addition of small amounts of boric acid (1 to 2%). It is advisable to avoid using water to bind such compositions. Red gum or shellac with alcohol or nitrocellulose lacquer are preffered binder and solvents.
Sources: Barium nitrate may be prepared from nitric acid or ammonium nitrate and barium carbonate, which is available from ceramic supply stores.
6.7 Barium sulfate:
Formula: BaSO4
Description: Barium sulfate is used as a high-temperature oxidiser in some ****l based green color compositions.
Hazards: Unlike many other barium compounds, barium sulfate is not very poisonous due to its low solubility in water.
Sources: Barium sulfate may be precipitated from a solution of a soluble barium salt, such as barium nitrate or chloride, and a sulfate. Magnesium and potassium sulfate are both cheaply available as fertilizer and are convenient to use. The precipitated barium sulfate is a very fine powder which may be rinsed by repeated washings with hot water, settling and decanting. A final washing in the filter with acetone or ethanol will allow it to dry quickly. Do not use sulfuric acid to precipitate barium sulfate as this may result in the inclusion of acid droplets in the precipitated particles which can lead to spontaneous ignition of some mixtures.
6.8 Boric acid:
Formula: H3BO3
Description: Boric acid is a white powder which is used as an additive to compositions containing aluminum or magnesium and a nitrate. The ****l powder can reduce the nitrate to an amide which will react with the ****l powder in a very exothermic reaction that can lead to spontaneous ignition of the composition. This process is often accompanied by a smell of ammonia and is most likely to occur with wet compositions. Addition of a few percent boric acid can often prevent this reaction from taking place since it neutralizes the very basic amides forming ammonia and a borate. It is also advisable to avoid using a water soluble binder for these composition. Using red gum or shellac with alcohol or nitrocellulose lacquer is safer.
Hazards: Boric acid is not particularly toxic or dangerous.
Sources: Boric acid is cheaply and in kilogram quantities available from ceramic supply shops. It is also sold in many drug stores at a somewhat higher price, but since only small quantities are needed the price is not really important.
6.9 Calcium sulphate:
Formula: CaSO4.x H2O where x= 0, 2, 3 or 5
Description: The trihydrate is commonly known as plaster of paris. The dihydrate occurs as a mineral known as gypsum . Calcium sulphate can be used as a high temperature oxidiser in orange color compositions. Excellent strobe compositions can be made with it.
Hazards: Calcium sulphate is not particularly toxic or dangerous.
Sources: Plaster can be used as is in strobe compositions, but is better to remove the water which is easily accomplished by heating.
6.10 Dextrin:
Formula: mixture of polysacharides
Description: Dextrine is one of the most commonly used binders in pyrotechincs as it is very cheap and readily available. It is water soluble and can produce rock hard stars.
Hazards: Colophonium is not particularly toxic or dangerous.
Sources: Dextrine is easily prepared from starch. Potato and corn starch will both work fine. The starch is spread out on a sheet in a layer about 1 cm thick and placed in the oven. The oven is then heated to 220°C for several hours. The dextrine will turn slightly yellowish brown. One way to check if all the starch has been converted is to dissolve a small sample in boiling hot water and add a drop of KI3 solution. A blue color indicates presence of starch, which means the conversion hasn't completed yet. KI3 solution is conveniently prepared by dissolving a crystal of elemental iodine in a potassium iodide solution.
6.11 Ethanol:
Formula: CH3CH2OH
Description: Ethanol is used as a solvent. Red gum and shellac, two common binders both dissolve in ethanol well. Ethanol/water mixtures are also often used since the ethanol increases the 'wetness' of the water (it reduces the surface tension of the water) and reduces the solubility of common oxidisers.
Hazards: Ethanol is flammable and volatile. Ethanol vapour is heavier than air and spreads over the ground. Provide adequate ventilation when working with ethanol.
Sources: Chemically pure ethanol can be quite expensive due to increased tax, unless it is used for laboratory purposes. Denaturated alcohol (usually a mixture of ethanol and methanol) has been made undrinkable and therefore a lot cheaper. It can be used for pyro purposes. Some types of denaturated alcohol exist with other chemicals mixed in besides methanol to make it undrinkable and recognisable as such (colorants etc). I have no idea what these extra additives are and wheter they can cause problems in compositions. I have been using 'spiritus' (a well known type of denaturated alcohol in the Netherlands) for several years without problems.
6.12 Iron:
Formula: Fe
Description: Iron powder is used for spark effects, mainly in fountains and sparklers. It produces golden yellow branching sparks. Not every iron alloy will work equally well. Iron alloys with a high carbon content generally work best. Stainless steel will produce hardly any sparks.
Hazards: Iron needs to be protected before use in pyrotechnic compositions. Otherwise it will corrode and render the composition useless or even dangerous. Iron containing compositions are generally best kept dry and not bound with water soluble binders. Iron can be coated with linseed or tung oil. The latter was used in ancient China (and may still be used shellac, two common binders​

 

[معمر القذافى]

gaseous ammonia or aqueous ammonium hydroxide. Filter the solution to collect the crystals of ammonium perchlorate, recrystallize them from water, and dry at 110 °C until a constant weight is obtained.
6.40-3 barium perchlorate:
Ba(ClO4)2 melting point
505 °C molecular mass
336.27 g/mol density
3.681 g/mL
Anhydrous barium perchlorate is prepared by heating a mixture of solid barium chloride and nitrosyl perchlorate, or by heating a mixture of barium carbonate and ammonium perchlorate.
6.40-4 cadmium perchlorate:
Cd(ClO4)2 melting point
290 °C molecular mass
311.30 g/mol
Anhydrous cadmium perchlorate can be prepared by mixing together cadmium nitrate with anhydrous perchloric acid and 100% nitric acid.
6.40-5 calcium perchlorate:
Ca(ClO4)2 melting point
220 °C molecular mass
238.98 g/mol
Anhydrous calcium perchlorate can be prepared by heating a mixture of 100 g of calcium carbonate with 235 g of ammonium perchlorate. Ammonium carbonate will be evolved as a gas, leaving behind pure calcium perchlorate.
6.40-6 cobalt perchlorate:
Co(ClO4)2 molecular mass
257.83 g/mol density
3.327 g/mL
The hexahydrate of cobalt perchlorate can be prepared by dissolving calcium carbonate, or calcium oxide, in aqueous perchloric acid. Evaporation of the solution yields crystals of cobalt perchlorate.
6.40-7 copper perchlorate:
Cu(ClO4)2 melting point
82.3 °C molecular mass
262.43 g/mol density
2.225 g/mL
Anhydrous copper perchlorate is prepared by heating in vacuum at 200 °C a mixture of nitrosyl perchlorate and your choice of either copper monoxide, copper dichloride, or copper nitrate. It can also be prepared by reacting copper powder with nitrosyl perchlorate in an organic solvent.
6.40-8 hydrazine diperchlorate:
N2H4.2HClO4 melting point
191 °C molecular mass
232.97 g/mol density
2.21 g/mL
Hydrazine diperchlorate, or HDP, can be prepared by reacting equimolar amounts of aqueous barium perchlorate with hydrazine sulfate. Filter to remove the precipitate of barium sulfate, and evaporate the filtrate on a water bath to yield crystals of HDP.
6.40-9 iron perchlorate:
Fe(ClO4)2 melting point
explodes molecular mass
254.75 g/mol
Iron perchlorate is prepared by reacting 70% perchloric acid with iron sulfide, or iron sulfate, followed by evaporation of the solution. Heat the solution very gently to evaporate, strong heating can cause an explosion.
6.40-10 lead perchlorate:
Pb(ClO4)2 melting point
83 °C molecular mass
406.09 g/mol density
2.6 g/mL
The trihydrate of lead perchlorate can be prepared by dissolving lead carbonate in aqueous perchloric acid and evaporation the solution until crystals appear.
6.40-11 lithium perchlorate:
Li(ClO4)2 molecular mass
205.84 g/mol
The trihydrate of lithium perchlorate can be prepared by reacting lithium sulfate with barium perchlorate in solution, then evaporating the solution to yield the crystals. It can also be prepared by reacting lithium carbonate with aqueous perchloric acid.
6.40-12 magnesium perchlorate:
Mg(ClO4)2 melting point
224-520 °C molecular mass
223.21 g/mol density
2.21 g/mL
The hexahydrate of magnesium perchlorate can be prepared by dissolving pure magnesium oxide in dilute perchloric acid. Evaporate the solution until fumes appear, then cool. Filter to collect the crystals of magnesium perchlorate that should have formed, and recrystallize them from water.
6.40-13 manganese perchlorate:
Mn(ClO4)2 melting point
explodes molecular mass
253.84 g/mol
The hexahydrate of manganese perchlorate can be prepared by dissolving manganese hydroxide, or manganese carbonate, in dilute perchloric acid. Evaporate the solution until crystals appear.
6.40-14 mercury perchlorate:
Hg(ClO4)2 molecular mass
399.49 g/mol
Anhydrous mercury perchlorate can be prepared by adding a solution of perchloric acid in trifluoroacetic acid to and mercury salt in trifluoroacetic acid. Carefully evaporate the solution until crystals form.
6.40-16 nickel perchlorate:
Ni(ClO4)2 melting point
explodes molecular mass
257.61 g/mol density
3.4 g/mL
The hexaammoniate of nickel perchlorate can be prepared by adding a solution of 14 g of sodium perchlorate in 50 mL of water to a solution of 23.8 g of nickel dichloride and 5.4 g of ammonium chloride in 120 mL of water. Slowly add with stirring 60 mL of concentrated ammonium hydroxide. Cool this mixture for 4 hours with a salt-ice bath, then filter to collect the crystals of the perchlorate.
6.40-17 nitryl perchlorate:
NO2ClO4 melting point
135 °C molecular mass
161.45 g/mol
Nitryl perchlorate can be prepared by distilling anhydrous perchloric acid, allowing the distillate to drip onto a large excess of dry dinitrogen pentoxide chilled to -80 °C (yes that's negative) and some nitromethane. The mixture is allowed to warm to room temperature, then kept under vacuum for 48 hours to remove any volatile contaminants.
6.40-18 potassium perchlorate:
KClO4 melting point
588 °C molecular mass
138.55 g/mol density
2.53574 g/mL
Potassium perchlorate is prepared by slowly adding 50 mL of concentrated sulfuric acid to 2-5 g of potassium chlorate. The addition is slow to avoid explosion. Alternately, nitric acid, phosphoric acid, or chromium trioxide can be used instead of sulfuric acid. It can also be prepared by mixing potassium chloride and nitrosyl perchlorate in solid form and heating. A residue of potassium perchlorate will be left behind.
6.40-19 silver perchlorate:
AgClO4 melting point
486 °C molecular mass
207.32 g/mol density
2.806 g/mL
Anhydrous silver perchlorate can be prepared by adding anhydrous perchloric acid to a solution of a silver salt dissolved in trifluoroacetic acid. It can also be prepared by dissolving silver oxide in aqueous perchloric acid and evaporating the solution until crystals appear.
6.40-20 sodium perchlorate:
NaClO4 melting point
473 °C molecular mass
122.44 g/mol density
2.5298 g/mL
The monohydrate of sodium perchlorate can be prepared by dissolving sodium carbonate in a slight excess of dilute perchloric acid. Evaporate some of the solution, then cool to 50 °C. The solid can be centrifuged, collected, and dried at 250 °C. The anhydrous can be obtained by recrystallizing from water above 53 °C.
6.40-21 strontium perchlorate:
Sr(ClO4)2 melting point
decomposes molecular mass
286.52 g/mol density
2.973 g/mL
The monohydrate of strontium perchlorate can be prepared by dissolving pure strontium nitrate in an excess of perchloric acid, and neutralizing the acid with strontium carbonate. Centrifuge to collect waste solids, and chill the liquid until crystals of the perchlorate appear.

6.40-22 titanium tetraperchlorate:
Ti(ClO4)4 molecular mass
445.70 g/mol
Anhydrous titanium tetraperchlorate can be prepared by mixing 8 moles of anhydrous perchloric acid with 1 mole of titanium tetrachloride at -10 °C.
6.40-23 uranyl perchlorate:
UO2(ClO4)2 melting point
90 °C molecular mass
469.0 g/mol
The hexahydrate of uranyl perchlorate can be prepared by dissolving ordinary hardware store brand uranium trioxide in 40% perchloric acid. Concentrate the solution on a water bath then chill to yield yellow crystals of the perchlorate.
6.40-24 zinc perchlorate:
Zn(ClO4)2 melting point
106 °C molecular mass
264.27 g/mol density
2.252 g/mL
The hexahydrate of zinc perchlorate can be prepared by mixing solutions of zinc sulfate and barium perchlorate, filtering off the precipitate of barium sulfate, and evaporating the solution until crystals appear. It can also be prepared by zinc oxide, or zinc carbonate, in aqueous perchloric acid and evaporating the solution until crystals appear.​

 

[معمر القذافى]

Acétone : diluant : Supermarché
Acide chlorhydrique : Acide chlorhydrique à 30% : Supermarché
Acide nitrique : Nettoyage de plaques : Imprimerie/magasin photo
Acide sulfurique : Acide de batterie : Supermarché/magasin d'auto
Alcool éthylique : Alcool éthylique à 95% : Supermarché
Ammoniac : Ammoniac (clair, pour nettoyage de vitre) : Supermarché
Carbone : Charbon de bois : Supermarché
Cellulose(coton) : Coton médical : Pharmacie
Chlorate de soude : Désherbant total : Rayon jardinage
Dextrine : Fusée : Amidon cuit
Eau distillée : Eau déminéralisée : Supermarché
Eau oxygénée : décoloration/désinfection : pharmacie
Glycérine : : pharmacie
Huile minérale : Cuisine : Supermarché
Iode : : Pharmacie
Magnésium : Allumeur : Camping
Mercure : Thermomètre à mercure : Supermarché
Nitrate d'ammonium : Amonitrate (engrais) : Jardinage/agriculture
Nitrate de sodium : Engrais : Rayon jardinage
Oxyde de fer : Rouille : Fer rouillé/droguerie
Permanganate de Potassium : Désinfectant : Pharmacie
Peroxyde d'hydrogène : Eau oxygénée : Pharmacie
Poudre sans fumée : Poudre à fusil : Armurerie
Saccharose : Sucre en poudre : Supermarché
Soufre : Jardinage : Rayon jardinage

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[tom14cat]

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