Alkalinity affects gluten production in kneaded doughs, and also improves browning by reducing the temperature at which the Maillard reaction occurs. Sodium carbonate has several uses in cuisine, largely because it is a stronger base than baking soda ( sodium bicarbonate) but weaker than lye (which may refer to sodium hydroxide or, less commonly, potassium hydroxide). The calcium and magnesium ions form insoluble solid precipitates upon treatment with carbonate ions: Sodium carbonate is a water-soluble source of carbonate. Sodium carbonate is used for removing these ions and replacing them with sodium ions. Hard water usually contains calcium or magnesium ions. It is also a key input for tableware glass manufacturing. Soda–lime glass has been the most common form of glass for centuries. In this way, sodium carbonate is a source of sodium oxide. When these materials are heated, the carbonates release carbon dioxide. Bottle and window glass (" soda–lime glass" with transition temperature ~570 ☌) is made by melting such mixtures of sodium carbonate, calcium carbonate, and silica sand ( silicon dioxide (SiO 2)). This "soda glass" is mildly water-soluble, so some calcium carbonate is added to the melt mixture to make the glass insoluble. Sodium carbonate serves as a flux for silica (SiO 2, melting point 1,713 ☌), lowering the melting point of the mixture to something achievable without special materials. It is used in the manufacture of sodium compounds like borax.It is used in the manufacture of glass, soap, and paper (see § Glass manufacture).It is used for lowering the hardness of water (see § Water softening).It has detergent properties through the process of saponification, which converts fats and grease to water-soluble salts (specifically, soaps). Sodium carbonate is a component of many dry soap powders. As a cleansing agent for domestic purposes like washing clothes. Some common applications of sodium carbonate include: It is one of the few metal carbonates that is soluble in water. Na 2 CO 3 + 10 H 2 O ⟶ Na 2 CO 3 ⋅ 10 H 2 O Soda ash is dissolved in water and crystallized to get washing soda. Sodium carbonate decahydrate (Na 2CO 3♱0H 2O), also known as washing soda, is the most common hydrate of sodium carbonate containing 10 molecules of water of crystallization. with 2.5 units of water per sodium carbonate unit ("pentahemihydrate"). In dry air the decahydrate and heptahydrate lose water to give the monohydrate. The decahydrate is formed from water solutions crystallizing in the temperature range −2.1 to +32.0 ☌, the heptahydrate in the narrow range 32.0 to 35.4 ☌ and above this temperature the monohydrate forms. It is also formed when sodium hydrogencarbonate is heated (calcined) e.g.
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