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The tables below provides information on the variation of solubility of different substances (mostly inorganic compounds) in water with temperature, at one atmosphere pressure. Units of solubility are given in grams of substance per 100 millilitres of water (g/(100 mL)), unless shown otherwise. The substances are listed in alphabetical order.
The following chart shows the solubility of various ionic compounds in water at 1 atm pressure and room temperature (approx. 25 °C, 298.15 K). "Soluble" means the ionic compound doesn't precipitate, while "slightly soluble" and "insoluble" mean that a solid will precipitate; "slightly soluble" compounds like calcium sulfate may require heat to precipitate.
Sodium hydroxide, also known as lye and caustic soda, [1] [2] is an inorganic compound with the formula NaOH. It is a white solid ionic compound consisting of sodium cations Na + and hydroxide anions OH −. Sodium hydroxide is a highly corrosive base and alkali that decomposes lipids and proteins at ambient temperatures and may cause severe ...
‡ Second column of table indicates solubility at each given temperature in volume of CO 2 as it would be measured at 101.3 kPa and 0 °C per volume of water. The solubility is given for "pure water", i.e., water which contain only CO 2. This water is going to be acidic. For example, at 25 °C the pH of 3.9 is expected (see carbonic acid).
A consequence of this is that concentrated solutions of sodium hydroxide have high viscosity due to the formation of an extended network of hydrogen bonds as in hydrogen fluoride solutions. In solution, exposed to air, the hydroxide ion reacts rapidly with atmospheric carbon dioxide, acting as an acid, to form, initially, the bicarbonate ion.
Sodium aluminate is manufactured by the dissolution of aluminium hydroxide (Al(OH) 3) in a caustic soda (NaOH) solution. Aluminium hydroxide can be dissolved in 20–25% aqueous NaOH solution at a temperature near the boiling point. The use of more concentrated NaOH solutions leads to a semi-solid product.
For example, at room temperature, in a 1-molar solution of acetic acid, only 0.001% of the acid are dissociated (i.e. 10 −5 moles out of 1 mol). Electron-withdrawing substituents, such as -CF 3 group , give stronger acids (the p K a of acetic acid is 4.76 whereas trifluoroacetic acid, with a trifluoromethyl substituent , has a p K a of 0.23).
or by reacting sodium hydroxide with chloral hydrate. C 2 HCl 3 (OH) 2 + NaOH → CHCl 3 + HCOONa + H 2 O. The latter method is, in general, preferred to the former because the low aqueous solubility of CHCl 3 makes it easier to separate out from the sodium formate solution, by fractional crystallization, than the soluble NaCl would be.