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The Leblanc process was an early industrial process for making soda ash (sodium carbonate) used throughout the 19th century, named after its inventor, Nicolas Leblanc.It involved two stages: making sodium sulfate from sodium chloride, followed by reacting the sodium sulfate with coal and calcium carbonate to make sodium carbonate.
An element–reaction–product table is used to find coefficients while balancing an equation representing a chemical reaction. Coefficients represent moles of a substance so that the number of atoms produced is equal to the number of atoms being reacted with. [1] This is the common setup: Element: all the elements that are in the reaction ...
Sodium carbonate (also known as washing soda, soda ash and soda crystals) is the inorganic compound with the formula Na 2 CO 3 and its various hydrates.All forms are white, odourless, water-soluble salts that yield alkaline solutions in water.
The Solvay Process as an example of a cyclic process in chemical industry (green = reactants, black = intermediates, red = products) The Solvay process results in soda ash (predominantly sodium carbonate (Na 2 CO 3 )) from brine (as a source of sodium chloride (NaCl)) and from limestone (as a source of calcium carbonate (CaCO 3 )). [ 8 ]
A chemical equation is the symbolic representation of a chemical reaction in the form of symbols and chemical formulas.The reactant entities are given on the left-hand side and the product entities are on the right-hand side with a plus sign between the entities in both the reactants and the products, and an arrow that points towards the products to show the direction of the reaction. [1]
For example a range from 1.4 to 2.2 Na 2 SO 4 •Na 2 CO 3 is stable as a solid solution. [2] Silvialite can substitute about half its sulfate with carbonate [ 3 ] and the high temperature hexagonal form of sodium sulfate (I) Na 2 SO 4 can substitute unlimited proportions of carbonate instead of sulfate.
At low pH, the following reaction might occur with thiosulfate: S 2 O 2− 3 + 2 H + → SO 2 + S + H 2 O. Some reactions involving certain reductants are reversible at certain pH, thus the pH of the sample solution should be carefully adjusted before performing the analysis. For example, the reaction: H 3 AsO 3 + I 2 + H 2 O → H 3 AsO 4 + 2 ...
For example, sulfuric acid (H 2 SO 4) is a diprotic acid. Since only 0.5 mol of H 2 SO 4 are needed to neutralize 1 mol of OH −, the equivalence factor is: f eq (H 2 SO 4) = 0.5. If the concentration of a sulfuric acid solution is c(H 2 SO 4) = 1 mol/L, then its normality is 2 N. It can also be called a "2 normal" solution.