What is pH and pOH?
pH and pOH scale define and measure the acidity and basicity of neutral, acidic, and basic solutions in water based on the relative concentration of hydrogen and hydroxyl ion mainly in chemistry, biology, and soil science. The terms pH and pOH scale are widely used and important for chemical, biological, and soil health measurement by translating the values of the concentration of hydrogen or hydroxyl ion or using pH paper and meter. Sorensen first invented or used the term known as pH scale or chart for measuring the concentration of hydrogen and hydroxyl ion for acid and alkaline solution.
What is pH definition?
According to Sorensen definition, pH (full form potential of hydrogen) is negative of the logarithm of the activity or concentration of hydrogen ion. Therefore, pH = – log aH+. When the solution is very dilute, aH+ = CH+, therefore, pH = – log CH+. The Sorensen definition largely uses in chemistry, biology, and agronomy for the simple mathematical calculation of pH and pOH scale value. Technically we use the instrument like pH paper and pH meter for acid and base determination.
What is pOH in chemistry?
In learning chemistry, the concentration value of hydroxyl ion represents the term known as the pOH in place of pH. Therefore, pOH = – log (COH–). If a solution of pH levels = 1 and the acidity of the said solution go down 100 fold, the pH scale range goes up by two units. In the same way, when hydroxyl ion will go down by two units means pOH values go from 13 to 11.
pH scale range
pH scale range or concentration of H+ ion differentiate neutral, acidic, and basic solutions. The acidity or basicity level defines the pH and pOH scale chart value of the neutral, acidic, or alkaline solution in chemistry.
Acidic, basic, and neutral solutions
pH value of neutral solution
A neutral solution or pure water solution meaning the solution where the concentrations of hydrogen and hydroxyl ions are equal or pH values of acids and bases are equal. Therefore, CH+ = COH– = 10-7 M. From the definition we can write simply, pH = pOH = 7. Therefore, this scale range or level explained that the neutral water solution having the same value of pH and pOH which stand for 7.
pH scale for acids
An acidic solution has the hydrogen ion greater than hydroxyl ion or CH+ > COH–. Therefore from the definition, pH < 7 and pOH > 7. From this equation, an acidic pure water solution pH scale range stands from zero to less than seven, and the pOH range stands from greater than seven to fourteen.
pH range for bases
But in alkaline or basic solution, the concentration of hydrogen less than hydroxyl ion or CH+ < COH–. Therefore, the measures pH range is greater than 7 to 14.
Ionic product of water
Water molecule ionizing weakly to form conjugate acid base pair like hydrogen ion and hydroxyl ion in solution. There will always be a chemical equilibrium between hydrogen and hydroxyl ions in the water solution. Therefore, H2O ⇄ H+ + OH–. Dissociation of water will have its equilibrium constant value, k × CH2O = CH+ × COH–, where CH2O, CH⁺, and COH⁻ = concentrations of water, hydrogen, and hydroxyl ions. But in any dilute aqueous solution, the concentration of water = 55.5 moles/liter, can be taken as a constant. Therefore, k × CH₂O = Kw = CH+ × COH–, where Kw = ionic product of water.
Chemical reactions in which absorbed a specific heat by the system from the surroundings are known as endothermic reactions in thermodynamics. A specific heat or energy (13.7 kcal) is absorbed from the surroundings for the ionization of water. Therefore, according to the Le Chatelier principle, increasing temperature will facilitate higher values of dissociation constant (Kw). The ionic product of hydrogen ion and hydroxyl ion has constant having the value 10-14. Therefore, from the Sorensen pH and pOH definition in chemistry, pH + pOH = 14.
What is the ph of water?
The concentration of hydrogen and hydroxyl ion or pH scale in pure water equal to the ionic product of water. The ionic product of pure water = 10-14 and the concentration of hydrogen ion and hydroxyl ion are the same. Hence, Kw = CH+ × COH– =10-7 × 10-7 = 10-14. Therefore, the above facts describe the pure water solution pH scale level. The pH value for pure equal to 7 because CH+ = COH– = 10-7. This equation shows that the concentration of hydrogen ion and hydroxyl ion are inversely proportional to each other. To maintain constant Kw, if hydrogen ion concentration increases 100 fold then hydroxyl ion decrease 100 fold.
Measurement of pH
For 0.01 m sulfuric acid
Sulfuric acid is a dibasic acid. Normality of sulfuric acid = 2 × molarity of the sulfuric acid solution. Thus the values of 0.1 m and 0.2 N sulfuric acids are the same. Therefore, the pH measurement value for 0.1 M or 0.2 N sulfuric acid = – log (0.2) = 0.699.
For 0.02 M hydrochloric acid
Hydrochloric acid is a strong electrolyte and completely dissociated in the solution. Therefore the measured pH value of 0.02 M hydrochloric acid (HCl) solution = – log (2×10-3) = (3 – log2) = 2.7.
For 0.02 m acetic acid
Acetic acid is a weak organic acid and the concentration of hydrogen ion in 0.02 m acetic acid. Therefore the measured pH value for 0.002 acetic acid (CH3COOH) = – log (CH+) = -log (2 × 10-4) = 3.7.
Negative pH scale
Nitric acid, sulfuric acid, hydrochloric acid in pure water solution are completely dissociated and regarded as an almost equally strong acid. But the mathematical definition or application of pH meter provides the negative scale value when the concentration of hydrogen ion in some content exceeds 1 gm equivalent. Therefore, measure pH and pOH scales value for such polar acid, base, or salt solution avoided because these solutions are not likely to dissociate fully. The absolute concentration of such a strong acid solution is measure in terms of relative molarity rather than the potential of hydrogen or pH scale value.