Prepration of buffer solutions of acetic acid and sodium acetate and its pH
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The pH of the mobile phase (eluent) is adjusted to improve component separation and to extend the column life. This pH adjustment should involve not simply dripping in an acid or alkali but using buffer solutions, as much as possible. Good separation reproducibility (stability) may not be achieved if buffer solutions are not used.
A buffer solution is prepared as a combination of weak acids and their salts (sodium salts, etc.) or of weak alkalis and their salts. Common preparation methods include: 1) dripping an acid (or alkali) into an aqueous solution of a salt while measuring the pH with a pH meter and 2) making an aqueous solution of acid with the same concentration as the salt and mixing while measuring the pH with a pH meter. However, if the buffer solution is used as an HPLC mobile phase, even small errors in pH can lead to problems with separation reproducibility. Therefore, it is important to diligently inspect and calibrate any pH meter that is used. This page introduces a method that does not rely on a pH meter. The method involves weighing theoretically calculated fixed quantities of a salt and acid (or alkali) as shown in the table below. Consider the important points below.
Denoting Buffer Solutions
A buffer solution denoted, "100 mM phosphoric acid (sodium) buffer solution pH = 2.1," for example, contains phosphoric acid as the acid, sodium as the counterion, 100 mM total concentration of the phosphoric acid group, and a guaranteed buffer solution pH of 2.1.
Maximum Buffer Action Close to the Acid (or Alkali) pKa
When an acetic acid (sodium) buffer solution is prepared from 1:1 acetic acid and sodium acetate, for example, the buffer solution pH is approximately 4.7 (near the acetic acid pKa), and this is where the maximum buffer action can be obtained.
Buffer Capacity Increases as Concentration Increases
The buffer capacity of an acetic acid (sodium) buffer solution is larger at 100 mM concentration than at 10 mM, for example. However, precipitation occurs more readily at higher concentrations.
Beware of Salt Solubility and Precipitation
The salt solubility depends on the type of salt, such as potassium salt or sodium salt. Salts precipitate out more readily when an organic solvent is mixed in.
In addition, avoid using buffer solutions based on organic acids (carboxylic acid) as much as possible for highly sensitive analysis at short UV wavelengths. Consider the various analytical conditions and use an appropriate buffer solution, such as an organic acid with a hydroxyl group at the α position (see Supplement) to restrict the effects of metal impurity ions. (J.Ma,Y.Eg)
The pH of the mobile phase (eluent) is adjusted to improve component separation and to extend the column life. This pH adjustment should involve not simply dripping in an acid or alkali but using buffer solutions, as much as possible. Good separation reproducibility (stability) may not be achieved if buffer solutions are not used.
A buffer solution is prepared as a combination of weak acids and their salts (sodium salts, etc.) or of weak alkalis and their salts. Common preparation methods include: 1) dripping an acid (or alkali) into an aqueous solution of a salt while measuring the pH with a pH meter and 2) making an aqueous solution of acid with the same concentration as the salt and mixing while measuring the pH with a pH meter. However, if the buffer solution is used as an HPLC mobile phase, even small errors in pH can lead to problems with separation reproducibility. Therefore, it is important to diligently inspect and calibrate any pH meter that is used. This page introduces a method that does not rely on a pH meter. The method involves weighing theoretically calculated fixed quantities of a salt and acid (or alkali) as shown in the table below. Consider the important points below.
Denoting Buffer Solutions
A buffer solution denoted, "100 mM phosphoric acid (sodium) buffer solution pH = 2.1," for example, contains phosphoric acid as the acid, sodium as the counterion, 100 mM total concentration of the phosphoric acid group, and a guaranteed buffer solution pH of 2.1.
Maximum Buffer Action Close to the Acid (or Alkali) pKa
When an acetic acid (sodium) buffer solution is prepared from 1:1 acetic acid and sodium acetate, for example, the buffer solution pH is approximately 4.7 (near the acetic acid pKa), and this is where the maximum buffer action can be obtained.
Buffer Capacity Increases as Concentration Increases
The buffer capacity of an acetic acid (sodium) buffer solution is larger at 100 mM concentration than at 10 mM, for example. However, precipitation occurs more readily at higher concentrations.
Beware of Salt Solubility and Precipitation
The salt solubility depends on the type of salt, such as potassium salt or sodium salt. Salts precipitate out more readily when an organic solvent is mixed in.
In addition, avoid using buffer solutions based on organic acids (carboxylic acid) as much as possible for highly sensitive analysis at short UV wavelengths. Consider the various analytical conditions and use an appropriate buffer solution, such as an organic acid with a hydroxyl group at the α position (see Supplement) to restrict the effects of metal impurity ions. (J.Ma,Y.Eg)
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