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An acid–base titration is a method of quantitative analysis for determining the concentration of Brønsted-Lowry acid or base (titrate) by neutralizing it using a solution of known concentration (titrant). [1]
When used as an indicator in an EDTA titration, the characteristic blue end-point is reached when sufficient EDTA is added and the metal ions bound to the indicator are chelated by EDTA, leaving the free indicator molecule.
In chemistry, an acid dissociation constant (also known as acidity constant, or acid-ionization constant; denoted ) is a quantitative measure of the strength of an acid in solution.
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Thioglycolic acid with a pK a of 3.83 [7] is an acid about 8.5 times stronger than acetic acid (pK a 4.76): . HSCH 2 CO 2 H → HSCH 2 CO 2 − + H +. The second ionization has a pK a of 9.3:
Murexide (NH 4 C 8 H 4 N 5 O 6, or C 8 H 5 N 5 O 6 ·NH 3), also called ammonium purpurate or MX, is the ammonium salt of purpuric acid.It is a purple solid that is soluble in water. The compound was once used as an indicator reagent. [1]
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