Importance Of Acid Base Chemistry

INTRODUCTION OF ACID BASE REACTION

Acids and bases play a essential role in chemistry because, with the exclusion of redox reactions, each chemical reaction can be categorized as an acid-base reaction.

Practical use of acid base chemistry

Acid-base chemistry is central to us on a practical level as well, outside of laboratory chemical reactions. Our bodily functions, going from the microscopic transport of ions through nerve cell membranes to the macroscopic acidic digestion of food in the stomach, are all lined by the principles of acid-base chemistry. Homeostasis, the temperature and chemical equilibriums in our bodies, is preserved by acid-base reactions. For example, fluctuations in the pH, or concentration of hydrogen ions, of our blood

Lavoisier made-up that all acids must comprise oxygen, and this idea was combined in the names used for this element in the various languages; the English oxygen, from the Greek oxys (sour) and genna (production); the German Sauerstoff, literally acid material; and the Russian kislorod, from kislota (acid). Succeeding the discovery that hydrochloric acid confined no oxygen, Sir Humphry Davy about 1815 first known that the key element in acids was hydrogen. Not all substances that hold hydrogen, however, are acids, and the first really reasonable definition of an acid was given by Justus von Liebig of Germany in 1838. According to Liebig, an acid is a compound having hydrogen in a form in which it can be replaced by a metal. This definition held the field for about 50 years and is still deliberated essentially correct, though somewhat outmoded. At the time of Liebig’s proposal, bases were still stared solely as substances that neutralized acids with the production of salts, and nothing was known about the constitutional features of bases that enabled them to do

Mixing acids and bases can cancel out or neutralize their thrilling effects. A substance that is neither acidic nor basic is neutral.

The pH scale processes how acidic or basic a substance is. The pH scale series from 0 to 14. A pH of 7 is neutral. A pH less than 7 is acidic. A pH greater than 7 is basic.

The pH scale is logarithmic and as a result, each whole pH value below 7 is ten times more acidic than the next higher value. For example, pH 4 is ten times more acidic than pH 5 and 100 times (10 times 10) more acidic than pH 6. The same grasps true for pH values above 7, each of which is ten times more alkaline (another way to say basic) than the next lower whole value. For example, pH 10 is ten times more alkaline than pH 9 and 100 times (10 times 10) more alkaline than pH 8. PH SCALE

The pH scale is used to overgrown solutions in terms of acidity or basicity (alkalinity). Since the scale is depends on pH values, it is logarithmic, meaning that a change of 1 pH unit resembles to a ten-fold change in H+^+ start superscript, plus, end superscript ion concentration. The pH scale is often said to range from 0 to 14, and most solutions do fall within this range, while it’s possible to get a pH below 0 or above 14. Anything below 7.0 is acidic, and anything above 7.0 is alkaline, or