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"McFarland High School may refer to: *McFarland High School (Wisconsin), in McFarland, Wisconsin *McFarland High School (California), in McFarland, California "
"Drake (2016 population: ) is a village in the Canadian province of Saskatchewan within the Rural Municipality of Usborne No. 310 and Census Division No. 11. The village lies west of Highway 20, approximately south of its intersection with the Yellowhead Highway. History Drake incorporated as a village on September 19, 1910. Demographics In the 2016 Census of Population conducted by Statistics Canada, the Village of Drake recorded a population of living in of its total private dwellings, a change from its 2011 population of . With a land area of , it had a population density of in 2016. In the 2011 Census of Population, the Village of Drake recorded a population of , a change from its 2006 population of . With a land area of , it had a population density of in 2011. Economy Drake is mostly a farming community, supported by the crops and livestock of the surrounding farms. However, several successful large-scale businesses, Drake Meat ProcessorsDrake Meat Processors and Bergen IndustriesBergen Industries were founded in and operate from the village, keeping it from becoming a loose connection of farms. Education The local school, Drake Elementary School, is used by elementary-aged students from Drake (as well as surrounding areas without their own school, such as Lockwood). After Grade 8, students go to the nearby Lanigan Central High School to complete their secondary education. Despite decreasing enrollment, DES finds strong support in the community; however, recent changes to the school division structuring across Saskatchewan have left its long-term future in doubt. Sports Drake is home to the 2018 Senior Saskatchewan Hockey Association Provincial C, Long Lake Hockey League champions the Drake Canucks. Notable people Home of former National Hockey League player Robin Bartel. See also * List of communities in Saskatchewan * Villages of Saskatchewan References External links * Villages in Saskatchewan Usborne No. 310, Saskatchewan Division No. 11, Saskatchewan "
"Barium chlorate, Ba(ClO3)2, is a white crystalline solid, the barium salt of chloric acid. It is an irritant and toxic, as are all soluble barium compounds. It is sometimes used in pyrotechnics to produce a green color. It also finds use in the production of chloric acid. Reactions =Synthesis= Barium chlorate can be produced through a double replacement reaction between solutions of barium chloride and sodium chlorate: :BaCl2 \+ 2 NaClO3 → Ba(ClO3)2 \+ 2 NaCl On concentrating and chilling the resulting mixture, barium chlorate precipitates. This is perhaps the most common preparation, exploiting the lower solubility of barium chlorate compared to sodium chlorate. The above method does result in some sodium contamination, which is undesirable for pyrotechnic purposes, where the strong yellow of sodium can easily overpower the green of barium. Sodium-free barium chlorate can be produced directly through electrolysis: :BaCl2 \+ 6 H2O → Ba(ClO3)2 \+ 6 H2 It can also be produced by the reaction of barium carbonate with boiling ammonium chlorate solution: :2 NH4ClO3 \+ BaCO3 \+ Q → Ba(ClO3)2 \+ 2 NH3 \+ H2O + CO2 The reaction initially produces barium chlorate and ammonium carbonate; boiling the solution decomposes the ammonium carbonate and drives off the resulting ammonia and carbon dioxide, leaving only barium chlorate in solution. The green seen in this firework is produced by barium chlorate and barium nitrate =Decomposition= When exposed to heat, barium chlorate alone will decompose to barium chloride and oxygen: :Ba(ClO3)2 → BaCl2 \+ 3 O2 =Chloric acid= Barium chlorate is used to produce chloric acid, the formal precursor to all chlorate salts, through its reaction with dilute sulfuric acid, which results in a solution of chloric acid and insoluble barium sulfate precipitate: :Ba(ClO3)2 \+ H2SO4 → 2 HClO3 \+ BaSO4 Both the chlorate and the acid should be prepared as dilute solutions before mixing, such that the chloric acid produced is dilute, as concentrated solutions of chloric acid (above 30%) are unstable and prone to decompose, sometimes explosively. Commercial uses Barium chlorate, when burned with a fuel, produces a vibrant green light. Because it is an oxidizer, a chlorine donor, and contains a metal, this compound produces a green color that is unparalleled. However, due to the instability of all chlorates to sulfur, acids, and ammonium ions, chlorates have been banned from use in class C fireworks in the United States. Therefore, more and more firework producers have begun to use more stable compound such as barium nitrate and barium carbonate. Environmental Hazard Barium chlorate is toxic to humans and can also harm the environment. It is very harmful to aquatic organisms if it is leached into bodies of water. Chemical spills of this compound, although not common, can harm entire ecosystems and should be prevented. It is necessary to dispose of this compound as hazardous waste. The Environmental Protection Agency (EPA) lists barium chlorate as hazardous. References Barium compounds Inorganic compounds Chlorates Pyrotechnic oxidizers Pyrotechnic colorants Oxidizing agents "