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Express each concentration value as the ratio c/c 0, where c 0 is the concentration in a [hypothetical] standard state, with a numerical value of 1, by definition. [19] Express the concentrations on the mole fraction scale. Since mole fraction has no dimension, the quotient of concentrations will, by definition, be a pure number.
For instance, HCl titrated with NaOH of approximately the same concentration will replace H + with an ion (Na +) of the same charge at the same concentration, to keep the ionic strength fairly constant. Otherwise, a relatively high concentration of background electrolyte can be used, or the activity quotient can be computed. [2]
C A is the analytical concentration of the acid and C H is the concentration the hydrogen ion that has been added to the solution. The self-dissociation of water is ignored. A quantity in square brackets, [X], represents the concentration of the chemical substance X. It is understood that the symbol H + stands for the hydrated hydronium ion.
The solvent (e.g. water) is omitted from this expression when its concentration is effectively unchanged by the process of acid dissociation. The strength of a weak acid can be quantified in terms of a dissociation constant , K a {\displaystyle K_{a}} , defined as follows, where [ X ] {\displaystyle {\ce {[X]}}} signifies the concentration of a ...
The dissociation constant has molar units (M) and corresponds to the ligand concentration [] at which half of the proteins are occupied at equilibrium, [6] i.e., the concentration of ligand at which the concentration of protein with ligand bound [] equals the concentration of protein with no ligand bound []. The smaller the dissociation ...
In part because of its high polarity, HCl is very soluble in water (and in other polar solvents). Upon contact, H 2 O and HCl combine to form hydronium cations [H 3 O] + and chloride anions Cl − through a reversible chemical reaction: HCl + H 2 O → [H 3 O] + + Cl −. The resulting solution is called hydrochloric acid and is a strong acid.
HCl + NaOH → NaCl + H 2 O. Acidimetry is the specialized analytical use of acid-base titration to determine the concentration of a basic (alkaline) substance using standard acid. This can be used for weak bases and strong bases. [8] An example of an acidimetric titration involving a strong base is as follows: Ba(OH) 2 + 2 H + → Ba 2+ + 2 H 2 O
Another method which can be used to produce solutions up to 10% concentration is by the use of cation exchange resins and a soluble salt such as NaClO 3, where the Na+ cation will exchange with H+. [2] Another method is the heating of hypochlorous acid, producing chloric acid and hydrogen chloride: [citation needed] 3 HClO → HClO 3 + 2 HCl