2.10:
pH
The potential of hydrogen, or pH, refers to a solution's acidity or alkalinity — properties based on the concentration of hydronium ions.
The pH of a solution is the negative logarithm of its hydronium ion concentration. For example, a solution with 1 × 10-5 M hydronium concentration has a pH of 5.
pH values can range from zero to fourteen and are typically depicted in decreasing order of hydronium ion concentration on a pH scale.
Since pH is on a logarithmic scale, a solution of pH 4 has ten times more hydronium ions than a solution with pH 5, which has ten times more hydronium ions than pH 6, and so on.
pH seven is neutral since the water molecules dissociate into equal concentrations of hydroxide and the hydronium ion.
Coffee has an acidic pH due to the high concentration of hydronium ions.
In contrast, a low hydronium concentration, as in milk of magnesia, results in higher pH values.
Substances above a pH of seven are alkaline or basic, while those below are acidic.
2.10:
pH
The potential of hydrogen (pH) is a measure of the acidity or basicity of a water-based solution determined by the concentration of hydronium ions (H3O+). In one liter of pure water at neutral pH, there are 1×10−7 moles of hydronium ions. However, the extensive range of hydronium ion concentrations present in water-based solutions makes measuring pH in moles cumbersome. Therefore, a pH scale was developed to convert moles of hydronium ions into the negative logarithm of the hydronium ion concentration.
The pH of pure water, 7, represents a neutral solution. Most solutions have a pH between 0 and 14, but some solutions, like carborane (with a pH of −18), exceed this. One liter of carborane has 1×1018 moles of hydrogen ions.
As more hydronium ions accumulate, the pH value of a solution falls below 7. Coffee, lemon juice, and gastric acid (digestive juices) are acidic solutions with pHs around 4.5, 2.5, and 1.5, respectively.
Solutions with a pH above 7 are called alkaline, as they have lower hydronium ion concentration. Saltwater and soapy water are examples of alkaline solutions, with pHs of approximately 8 and 12, respectively.
Buffers are solutions that can prevent significant changes to pH. Buffers are critical because most biological functions occur in near-neutral pH conditions, approximately 7.35 to 7.45. For example, blood has an average pH of ~7.4, maintained by a buffer system involving carbonic acid (H2CO3), bicarbonate ions (HCO3–), and carbon dioxide (CO2).
Bicarbonate is also used to buffer chyme as it moves from the stomach to the small intestine. Without it, the acidity of the digested food would damage the lining of the intestine.