silver perchlorate 7783-93-9 AgF silver fluoride 7775-41-9 AgF2 silver difluoride 7775-41-9 AgI silver iodide 7783-96-2 AgIO3 silver iodate 7783-97-3 AgMnO4 silver permanganate 7783-98-4 AgN3 silver azide 13863-88-2 AgNO3 silver nitrate 7761-88-8 Ag2O silver oxide 1301-96-8 AgONC silver fulminate 5610-59-3 AgSNC silver thiocyanate 14104-20-2 Ag2C2 silver acetylide 7659-31-6 Ag2CO3 silver(I) carbonate 534-16-7 Ag2C2O4 silver oxalate 533-51-7 Ag2Cl2 silver(II)
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chemical and physical changes. Materials: * * Hot plate * Water * Salt * Evaporating dish * Candle * Matches * Ammonium hydroxide * Watch glass * Phenolphthalein * Paper towel * Cornstarch * Iodine * Cup * Alka-Seltzer tablet * Pipet * Milk * Vinegar * Copper II sulfate * Lead II nitrate Safety: * Goggles were worn. * Aprons were worn. * Lab station was cleaned up directly following experiments. * Hands were
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http://foricseandbeyond.blogspot.in/ DE’S FOUNDATION BISTUPUR‚ JSR ACTION OF HEAT ON CHEMICAL COMPOUNDS “Analytical chemistry -I” http://foricseandbeyond.blogspot.in/ metal oxide “Oxides of metals are generally stable to heat and they are considered to be most stable form of compound found in nature.” Oxides of potassium‚sodium‚calcium‚magnesium‚ aluminum ‚ zinc‚iron‚lead and copper are stable to heat uO C PbO Zn O http://foricseandbeyond.blogspot.in/ MERCURIC OXIDE
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mol) iron(III) nitrate solution (0.1 mol) copper(II) sulfate solution (0.1 mol) iron(II) sulfate solution (0.1 mol) What to do 1 Draw a cross on a piece of paper and put it underneath a 100 cm3 measuring cylinder‚ or use the cross from part 2‚ so it can be seen when looking down the cylinder. 2 Pour 50 cm3 of sodium thiosulfate solution into the measuring cylinder. 3 Pour 50 cm3 of iron(iii) nitrate solution in the second measuring cylinder. 4 Carefully pour the iron(iii) nitrate solution into the
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surrounded by six nitro ligands [1]. This compound is used as a qualitative test for potassium and ammonium ions (so long as certain other cations are not present) [1]. Potassium and ammonium are insoluble in water‚ while sodium is [1]. Hence‚ the potassium and ammonium salts are precipitated as a yellow solid. AIM To prepare sodium hexanitrocobaltate (III) from pure potassium-free sodium nitrite‚ cobalt nitrate hexahydrate‚ 50% acetic acid and 95% ethanol. THEORY In this practical‚ the nitrite ions
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Q. 1. What do you observe when ammonia gas is bubbled through red litmus solution? Q. 2. Write an equation for solutions of ammonium chloride and sodium hydroxide are heated. Q. 3.(i) What is the purpose of Haber’s Process ? (ii) Name the gaseous inputs of the Haber’s Process and state the ratio by volume in which the gases are mixed. (iii) What is done to increase the rate of reaction in the Haber Process ? (iv) Give two different ways by which the product can be separated from the reactants
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would be negative. During a chemical reaction‚ which consists of breaking and creating bonds‚ heat is either absorbed or released. In this lab‚ the reaction uses the disassociation of an ionic compound ammonium nitrate shown in the equation #1 below into ions. In order to disassociate ammonium nitrate into ions‚ energy is required. Both NH4 and NO3 are always soluble‚ therefore the ionic compound disassociates completely. Through equation #2‚ heat absorbed or released can be measured. In equation #2
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Discussion for Experiment 1 (Basic Laboratory Operations and Identification of a compound : Chemical Properties) In the first experiment‚ the precision of instrument was studied by measuring the mass of water for several times. The result shows that the mass measurement of the balance is precise since the masses of water in six trials are somewhat close. The reason that the masses of water in each trial are not identical may come from the high sensitivity of the balance that keep fluctuating due
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Recommended maximum (ppm) | Chloride | 20 | 400 | Sulfate | 8 | 400 | Nitrate | 0.4 | 10 | Fluoride | 1 | 1.7 | Sodium | 10 | 300 | Calcium | 9 | 200 | Aluminium | 0.2 | 0.2 | * The concentration of sodium (Na+) and chloride (Cl-) ions are important indicators of the salinity of a water system‚ and also affect the taste of water * Magnesium and calcium ions are indicators of water hardness * Phosphate and nitrate ions need to be monitored to prevent eutrophication of a water system
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History of Explosives and Blasting In the US and Canada alone‚ blasters use more than 6 billion pounds of explosives and 75 million detonators per year. Coal mining accounts for two-thirds of consumed explosives of which more than 80% of it is ANFO. Today‚ sophisticated explosive materials and new technologies are being utilized to improve the quality of life for all of us. Computers are used to: drill‚ log and monitor blastholes — automate blending and delivery with bulk trucks — determine bench
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