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Calcium oxide (formula: Ca O), commonly known as quicklime or burnt lime, is a widely used chemical compound. It is a white, caustic , alkaline , crystalline solid at room temperature . The broadly used term lime connotes calcium-containing inorganic compounds , in which carbonates , oxides , and hydroxides of calcium, silicon , magnesium ...
Besides the simple oxide CaO, calcium peroxide, CaO 2, can be made by direct oxidation of calcium metal under a high pressure of oxygen, and there is some evidence for a yellow superoxide Ca(O 2) 2. [16] Calcium hydroxide, Ca(OH) 2, is a strong base, though not as strong as the hydroxides of strontium, barium or the alkali metals. [17]
Calcium-alpha-ketoglutarate (C 5 H 4 CaO 5 •H 2 O) is a special form mineral calcium that can be used to restore calcium concentration level in the blood back to normal. Calcium-alpha-ketoglutarate binds excess phosphate and pass it as a waste, re-establishing normal balance of calcium and phosphate in the body.
A strong base is a basic chemical compound that can remove a proton (H +) from (or deprotonate) a molecule of even a very weak acid (such as water) in an acid–base reaction. Common examples of strong bases include hydroxides of alkali metals and alkaline earth metals, like NaOH and Ca(OH)
Calcium oxalate is a combination of calcium ions and the conjugate base of oxalic acid, the oxalate anion. Its aqueous solutions are slightly basic because of the basicity of the oxalate ion. The basicity of calcium oxalate is weaker than that of sodium oxalate, due to its lower solubility in water.
Aqueous buffer solutions will react with strong acids or strong bases by absorbing excess H + ions, or OH − ions, replacing the strong acids and bases with weak acids and weak bases. [13] This has the effect of damping the effect of pH changes, or reducing the pH change that would otherwise have occurred.
An example of a weak base is ammonia. It does not contain hydroxide ions, but it reacts with water to produce ammonium ions and hydroxide ions. [4] The position of equilibrium varies from base to base when a weak base reacts with water. The further to the left it is, the weaker the base. [5]
Calcium lactate has insufficient acid-neutralizing capacity caused by its weak base formation. The lactate ion (C 3 H 5 O 3 −) is the conjugate base of lactic acid, which is a weak acid. When calcium lactate dissolves in water, it releases lactate ions that can slightly increase the pH of the aqueous solution.