Further details, are given in the IUPAC recommendations. The reading from a second standard buffer solution is then adjusted using the "slope" control to be equal to the pH for that solution. To calibrate the electrode, it is first immersed in a standard solution, and the reading on a pH meter is adjusted to be equal to the standard buffer's value. Two or more buffer solutions are used in order to accommodate the fact that the "slope" may differ slightly from ideal. It is calibrated against buffer solutions of known hydrogen ion ( H +) activity proposed by the International Union of Pure and Applied Chemistry ( IUPAC). A combined glass electrode has an in-built reference electrode. In practice, a glass electrode is used instead of the cumbersome hydrogen electrode. pH = − log ( a H + ) ≈ − log ( ) \, the "Nernstian slope". The pH scale is logarithmic and inversely indicates the activity of hydrogen ions in the solution. ![]() ![]() Acidic solutions (solutions with higher concentrations of hydrogen ( H +) ions) are measured to have lower pH values than basic or alkaline solutions. It is a scale used to specify the acidity or basicity of an aqueous solution. In chemistry, pH ( / p iː ˈ eɪ tʃ/ pee- AYCH), also referred to as acidity, historically denotes "potential of hydrogen" (or "power of hydrogen").
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