Question

Why is pH important in living things?

Answer 1

pH is a scale used in chemistry to describe the acidity or basicity of an aqueous solution. Acidic solutions (those containing a larger concentration of ${{H}^{+}}$ ions) have a lower pH than basic or alkaline solutions. The pH scale is logarithmic, indicating the concentration of hydrogen ions in a solution in inverse order. Because the pH formula approximates the negative of the base 10 logarithm of the molar concentration of hydrogen ions in the solution, this is the case. pH is defined as the negative of the base 10 logarithm of the ${{H}^{+}}$ ion's activity.

Complete answer:
At $25\text{ }{}^\circ C$ , acidic solutions have a pH less than 7, while basic solutions have a pH greater than 7. At this temperature, pH 7 solutions are neutral (e.g. pure water). The pH neutral value changes with temperature, becoming lower than 7 as the temperature rises. For highly strong acids, the pH value can be less than 0 and for very strong bases, it can be more than 14.
Acid–base homeostasis is a process in which the pH of cellular compartments, bodily fluids, and organs is strictly controlled. Acidosis, which is defined as an acid excess in the body with a pH below 7.35, is the most frequent disease in acid–base balance. Alkalosis is the polar opposite of acidosis, in which the blood pH is abnormally high.
The pH of blood is typically somewhat basic, measuring 7.365. In biology and medicine, this number is referred to as physiological pH. Plaque can produce an acidic environment in the mouth, which can lead to tooth decay due to demineralization. Enzymes and other proteins have a pH range where they can denature and become denatured.
pH is significant because enzymes that catalyse life's chemical processes require a particular pH to function properly. Biochemicals such as proteins can also be denatured and rendered non-functional if the pH is substantially elevated or reduced, resulting in cell death.
The typical blood pH in humans is 7.4, which is somewhat basic. This guarantees that the cells' surroundings are kept at the appropriate pH level so that their biomolecules and enzymes may operate properly.

Note:
The pH scale may be traced back to a collection of standard solutions whose pH has been agreed upon internationally. The potential difference between a hydrogen electrode and a standard electrode, such as the silver chloride electrode, is measured in a concentration cell with transference to derive primary pH standard values. A glass electrode with a pH metre, or a color-changing indicator, can be used to determine the pH of aqueous solutions. pH measurements are useful in chemistry, agronomy, medicine, water treatment, and a variety of other fields.