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The compound consists of separate tetrahedral ammonium cations and octahedral [PtCl 6] 2− anions.It is usually generated as a fine yellow precipitate by treating a solution of hexachloroplatinic acid with a solution of an ammonium salt. [2]
Ra + 2H 2 O → Ra(HO) 2 + H 2. The reaction of radium oxide and water can also generate radium hydroxide, and the reaction releases a lot of heat: [citation needed] RaO + H 2 O → Ra(HO) 2. The compound can also be prepared by reacting radium nitrate with NaOH in solution. [citation needed]
The standard Gibbs free energy of formation (G f °) of a compound is the change of Gibbs free energy that accompanies the formation of 1 mole of a substance in its standard state from its constituent elements in their standard states (the most stable form of the element at 1 bar of pressure and the specified temperature, usually 298.15 K or 25 °C).
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.
A metal ion in aqueous solution or aqua ion is a cation, dissolved in water, of chemical formula [M(H 2 O) n] z+.The solvation number, n, determined by a variety of experimental methods is 4 for Li + and Be 2+ and 6 for most elements in periods 3 and 4 of the periodic table.
It is defined as the energy released with the formation of 1 mole of water. When a reaction is carried out under standard conditions at the temperature of 298 K (25 degrees Celsius) and 1 atm of pressure and one mole of water is formed, the heat released by the reaction is called the standard enthalpy of neutralization (ΔH n ⊖).
The density of the solution is 1.093 g/mL at 5% concentration, [22] and 1.21 g/mL at 14%, 20 °C. [23] Stoichiometric solutions are fairly alkaline, with pH 11 or higher [8] since hypochlorous acid is a weak acid: OCl − + H 2 O ⇌ HOCl + OH −. The following species and equilibria are present in NaOCl/NaCl solutions: [24] HOCl(aq) ⇌ H ...
The same equation relating the concentrations of acid and base applies. The concept of neutralization is not limited to reactions in solution. For example, the reaction of limestone with acid such as sulfuric acid is also a neutralization reaction. [Ca,Mg]CO 3 (s) + H 2 SO 4 (aq) → (Ca 2+, Mg 2+)(aq) + SO 2− 4 (aq) + CO 2 (g) + H 2 O