Barium chloride formula

Barium Chloride (BaCl₂) is an inorganic salt that is composed of Barium cations (Ba⁺) and Chloride anions (Cl⁻). It is also named Barium dichloride or Barium Muriate. It is a white solid chemical compound which is soluble in water, it is hygroscopic, and provides a frail yellow-green colour when put to a flame. BaCl₂ is the chemical formula of Barium Chloride. Barium salts are widely used in the industry. The sulfate is applied in white paints, especially for external use. Barium chloride is toxic in nature. Structure of Barium Chloride BaCl₂ The chemical formula of Barium Chloride is BaCl₂, and the molar mass of Barium Chloride is 208.23 g mol⁻¹. This salt is formed by one Barium cation (Ba²⁺) and one Chloride anion (Cl⁻). The crystals can be cubic fluorite or orthorhombic. Its chemical structure can be formulated as below, in the common representations applied for organic molecules. Cl⁻ Cl⁻ Ba²⁺ Preparation of Barium Chloride Hydrochloric acid (concentrated) 180 ml is diluted with 440 ml of water and emptied in a porcelain evaporating dish. The solid Barium Carbonate in tiny portions is added and mixed after. If Barium Carbonate is added too quickly, the mixture will churn out of the dish. After Barium Carbonate is added, and the solution becomes neutral to litmus, the mixture is ignited to boiling. If Barium Carbonate comprises iron as an impurity, it can be excluded by adding 3g of Barium Peroxide and boiling the solution gently for 5 minutes. The Barium Chloride hot s...

• العربية • Azərbaycanca • تۆرکجه • Català • Čeština • Deutsch • Ελληνικά • Español • Esperanto • Euskara • فارسی • Français • 한국어 • हिन्दी • Bahasa Indonesia • Italiano • ქართული • Қазақша • Latviešu • Magyar • Македонски • Bahasa Melayu • Nederlands • 日本語 • Norsk bokmål • Oʻzbekcha / ўзбекча • Polski • Português • Română • Русский • Simple English • Slovenčina • Slovenščina • Српски / srpski • Srpskohrvatski / српскохрватски • Suomi • Svenska • தமிழ் • తెలుగు • ไทย • Türkçe • Українська • Tiếng Việt • 吴语 • 中文 Chemical compound Barium chloride is an 2. It is one of the most common BaCl 2·2H 2O, which are colourless crystals with a bitter salty taste. It has limited use in the laboratory and industry. Preparation [ ] On an industrial scale, barium chloride is prepared via a two step process from BaSO 4 + 4 The second step requires reaction between BaS + 2 HCl → BaCl 2 + H 2S or between BaS + CaCl 2 → CaS + BaCl 2 In place of HCl, BaCl 2·2H 2O) can be crystallized as colorless crystals. Barium chloride can in principle be prepared by the reaction between Ba(OH) 2 + 2 HCl → BaCl 2 + 2 H 2O BaCO 3 + 2 HCl → BaCl 2 + H 2O + CO 2 Structure and properties [ ] BaCl 2 crystallizes in two forms ( PbCl 2) structure, whereas the cubic CaF 2) is stable between 925 and 963 °C. Ba 2+ ion for Ba 2+ is 8 in the fluorite structure BaCl 2 is subjected to pressures of 7–10GPa, it transforms to a third structure, a Ba 2+ increases from 9 to 10. In aqueous solution BaCl 2 behaves as a simple [...

Precipitation Reaction A precipitation reaction is a reaction that yields an insoluble product—a precipitate—when two solutions are mixed. We described a precipitation reaction in which a colorless solution of silver nitrate was mixed with a yellow-orange solution of potassium dichromate to give a reddish precipitate of silver dichromate: \[AgNO_3(aq) + K_2Cr_2O_7(aq) \rightarrow Ag_2Cr_2O_7(s) + KNO_3(aq)\tag\] Thus precipitation reactions are a subclass of exchange reactions that occur between ionic compounds when one of the products is insoluble. Because both components of each compound change partners, such reactions are sometimes called double-displacement reactions. Two important uses of precipitation reactions are to isolate metals that have been extracted from their ores and to recover precious metals for recycling. Video: Mixing Potassium Chromate and Silver Nitrate together to initiate a precipitation reaction (Equation 4.2.1). While chemical equations show the identities of the reactants and the products and gave the stoichiometries of the reactions, but they told us very little about what was occurring in solution. In contrast, equations that show only the hydrated species focus our attention on the chemistry that is taking place and allow us to see similarities between reactions that might not otherwise be apparent. Let’s consider the reaction of silver nitrate with potassium dichromate. When aqueous solutions of silver nitrate and potassium dichromate are mix...

• Experimental Physico-chemical Properties • Experimental Melting Point: 963 °C Alfa Aesar 963 °C OU Chemical Safety Data (No longer updated) 963 °C Alfa Aesar 1764-1766 °F (962.2222-963.3333 °C) Wikidata 1765 °F (962.7778 °C) Wikidata 961 °C Kaye & Laby (No longer updated) • Experimental Boiling Point: 2840 °F (1560 °C) NIOSH 1560 °C OU Chemical Safety Data (No longer updated) 2839-2841 °F / 760 mmHg (1559.4444-1560.5556 °C / 760 mmHg) Wikidata 2840 °F / 760 mmHg (1560 °C / 760 mmHg) Wikidata 37.5 °C / 150 mmHg (86.5023 °C / 760 mmHg) Kaye & Laby (No longer updated) 1560 °C / 760 mmHg Kaye & Laby (No longer updated) • Experimental Solubility: 35.7% w/w in 20?C water Kaye & Laby (No longer updated) 37-39 g/100g Wikidata 38% NIOSH 38.0 g/100g Wikidata 58.8% w/w in 100?C water Kaye & Laby (No longer updated) slightly soluble in HCl Kaye & Laby (No longer updated) slightly soluble in HNO3 Kaye & Laby (No longer updated) very slightly soluble in ethanol Kaye & Laby (No longer updated) • Experimental Density: 3.097 g/mL Alfa Aesar 3.9 g/mL Alfa Aesar 3.86 g/l Wikidata 3.097 g/mL / 24 °C Kaye & Laby (No longer updated) 3.917 g/mL / 20 °C Kaye & Laby (No longer updated) • Miscellaneous • Appearance: white granular crystalline powder OU Chemical Safety Data (No longer updated) White, odorless solid. NIOSH • Stability: Stable. OU Chemical Safety Data (No longer updated) • Toxicity: Inorganic Compound; Barium Compound; Household Toxin; Industrial/Workplace Toxin; Synthetic Compound ...

Barium is listed under Group 2A of So we have Barium as #Ba^(+2)# Now let's move to Chloride. Don't bother looking at the table, because it is not listed. Chloride is an ion of Chlorine, which is from Group 7A and we know anything in that column has a charge of -1. So Chlorine has gained an electron and becomes Chloride. Note that this is an anion and has a negative charge. You can see how easy it was to change the name, you just change the suffix to -ide. So we have Chloride as #Cl^-# We're not finished though! The charges do not balance! To balance it we simply add another Chloride so that you have two negatives balancing the two positives. You'll write it as #Cl_2#. Now they balance; you have one barium #Ba^(+2)# and two chloride #Cl^-# #Cl^-# The final formula is written as #BaCl_2#. Hope that helps!

Figure 1: structure of barium chloride It is one of the most water soluble barium salts. Like other barium salts, it is toxic and imparts a yellow-green coloration to a flame. It is also hygroscopic. There are several methods of production of barium chloride, one of them is by the action of hydrochloric acid in barium carbonate: 2HCl + BaCO 3 → BaCl 2 + CO 2 + H 2 OR Another method of producing barium chloride is by heating a mixture of barium sulfate, carbon and barium chloride. BaSO 4 (S) + 4C (s) → BaS (s) + 4CO (g) BaS (s) + CaCl 2 → BaCl 2 + CaS Physical and chemical properties Barium chloride are crystals, orthorhombic in their anhydrous and monoclinic form in their dihydrated form, white without a characteristic aroma (National Center for Biotechnology Information., 2005). Their appearance is shown in figure 2. Figure 2: appearance of barium chloride The compound has a molecular weight of 208.23 g / mol for its anhydrous form and 244.26 for its dihydrate form. It has a density of 3.856 g / ml for the anhydrous form and 3.098 g / ml for the dihydrate form. Its melting and boiling point is 963 ° C and 1560 ° C respectively. Barium chloride is very soluble in water, whereby 35.8 grams of compound can be dissolved in 100 ml of solvent (Royal Society of Chemistry, 2015). Neighborhood chloride may react violently with BrF 3 And 2-Furan percarboxylic acid in its anhydrous form (CAMEO, 2016). Reactivity and hazards Barium chloride is extremely poisonous and toxic. Ingestion...