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The Bronsted Lowry acid hypothesis is indeed an acid-base reaction theory first proposed in 1923 by Danish chemist Johannes Nicolaus Bronsted and Thomas Martin Lowry. According to the hypothesis, acids and bases interact with one another, with the acid forming its conjugate base and also the base forming its conjugate acid through proton interchange. The Bronsted-Lowry hypothesis is a more advanced variant of the Arrhenius acid-base theory. An acid raises the concentration of Hydrogen ions in an aqueous solution, whereas a base raises the percentage of OH– ions, as per the Arrhenius hypothesis. The Arrhenius theory has a restriction in that it only detects the interaction of an acid and a base during an aqueous phase.
Bronsted Lowry Acid Theory
About the Hypothesis
According to the Bronsted Lowry method, a constituent only acts as an acid in the presence of such a base, but only acts as a base within the absence of an acid. Moreover, once an acidic substance loses one proton, it creates an acidic solution, also known as an acid conjugate base, and when a basic substance obtains a proton, it produces the acid known as base conjugate acid. As a result, the reaction of an acidic chemical like hydrochloric acid and a basic substance like ammonia can be best summed up as:
HCl +NH3⇌NH4++Cl-
The ammonium ion (NH4+) is indeed the acid correspondent of the basic ammonia, while the chloride ion (Cl-) is indeed the base correspondent of hydrochloric acid present in the formula above. Acids include hydroxide ions, ammonium ions, and various saturated metal cations. Bases include phosphorus, acetate, sulphide, carbonate, and halogen ions.
Bronsted Lowry Acid
A material that gives or contributes hydrogen ions throughout a chemical reaction is known as a Bronsted-Lowry acid. The Bronsted-Lowry base, on the other hand, absorbs hydrogen ions. The Bronsted Lowry Acid contributes protons, whereas the base takes them. Amphoteric species would be those who may either give or take protons based on the circumstances.
Each Bronsted Lowry acid transfers its proton to the conjugate base molecule.
HCl (aq) + NH3 (aq)→ NH4+ (aq) + Cl- (aq)
Inside this following process, hydrochloric acid (HCl) contributes a proton on ammonia (NH3), forming an ammonium cation (NH4+) as well as the chloride anion (Cl-). A chloride ion is indeed the conjugate base of hydrochloric acid, which would be a Bronsted-Lowry acid.
Weak and Strong Acids
In the aqueous phase, a strong acid is a substance that entirely disintegrates into component ions. Strong acids include nitric acid and sulfuric acid. With water, it separates into hydronium & nitrate ions. There are no dissolved HNO3 molecules in solutions after the process.
A weak acid, on the other hand, doesn’t entirely dissolve into its component ions. Acetic acid, which would be found in vinegar, is a weak acid. With water, acetic acid partly separates into hydronium & acetate ions.
The Bronsted Lowry Acid Importance
- A Bronsted Lowry acid is a type of chemical that can donate a proton or a hydrocarbon cation.
- A Bronsted Lowry base is a type of chemical that can receive a proton. In other words, it is a species with a single electron pair that can attach to H+.
- After donating a proton, a Bronsted-Lowry acid creates its conjugate base. When a Bronsted-Lowry base receives a proton, it generates the conjugate acid. The chemical formula of the conjugate acid-base pair is identical to that of the initial acid-base pair, with the exception that the acid has one more H+ than the conjugate base.
- Compounds that ionise in water are known as strong acids and bases. Weak acids and bases typically dissolve partially.
- Aqua is amphoteric, as per this hypothesis, and may operate as both a Bronsted-Lowry acid and a Bronsted-Lowry base.
Conclusion
As per the Bronsted Lowry theory, acids and bases react through proton exchange, with the acid creating its conjugate base and the base producing its conjugate acid.
A Bronsted Lowry acid’s importance is that it provides or donates hydrogen ions during a chemical process. Protons are given by the Bronsted-Lowry acid, while they are taken away by the base. Amphoteric species are those that can provide or accept protons depending on the situation.
