Definitions of Acids and Bases - High School Chemistry

An acidic solution will always have a hydronium concentration greater than . A basic solution will always have a hydroxide concentration greater than . If the hydroxide concentration is equal to the hydronium concentration, the solution is neutral.

The opposite of the above conditions can also be noted. If the hydronium concentration is less than , then the solution will be basic. An example of this is a solution where the hydronium ion concentration is . Since this value is far less than , this will be a basic solution.

Strong acids and bases dissociate completely into ions when placed in an aqueous solution. In contrast, weak acids and bases do not completely dissociate.

There are only six strong acids: perchloric acid (HClO4), hydroiodic acid (HI), hydrobromic acid (HBr), hydrochloric acid (HCl), nitric acid (HNO3), and sulfuric acid (H2SO4).

There are three primary classifications of acids and bases.

Arrhenius acids yield protons when dissolved in solution, while Arrhenius bases yield hydroxide ions.

Brønsted-Lowry acids are protone donors, while Brønsted-Lowry bases are proton acceptors.

Lewis acids are electron acceptors, while Lewis bases are electron donors.

An acid that dissociates completely in solution is considered a strong acid due to its high Ka value.

The most common Lewis bases are anions, and therefore, have unpaired valence electrons which may be donated to Lewis acids. The concept of donating and/or accepting hydrogens refers to the Bronsted-Lowry definition of acids. A Bronsted-Lowry acid donates hydrogens.

Acids are soluble in water substance, but remember, only water gets the liquid (l) phase label. Since acids are almost always dissolved in water, we use the (aq) subscript at the end of the chemical formula to indicate its phase.

According to the Bronsted-Lowry definition, acids are hydrogen donors.

According to the Bronsted-Lowry definition, bases are hydrogen acceptors.

According to the Arrhenius definition, acids increase the concentration of hydrogen ions in a solution.

According to theArrhenius definition, bases increase the concentration of hydroxide ions in a solution.

According to the Lewis definition, acids are electron pair acceptors.

According to the Lewis definition, bases are electron pair donors.

An amphoteric substance is one that can act either as an acid or a base. Amino acids are good examples of amphoteric substances; they have a carboxylic acid group that can be acidic, and an amino group that can be basic.

Remember: amphoteric means that the substance can act as either an acid or a base. Using the Bronsted-Lowry definition of acids and bases (acids donate hydrogens and bases accept hydrogens) we find that is the only compound that can give up a hydrogen (and be left with ), or accept a hydrogen (and become ).

Acids have hydrogens that can dissociate into solution. In this case, the word "mono" tells us that there is only one potential hydrogen ion in that acid; so only one hydrogen ion can be ionized from that acid. A diprotic acid, such as has two ionizable hydrogens.

Acids have hydrogen ions and balanced charges, "di" tells us that the acid in question has two potential hydrogen ions, which can be ionized and turned into protons (protic). These acids, like can ionize once, yielding then again, yielding .

Acids have hydrogen ions and balanced charges. "Tri" tells us that the acid has three potential hydrogen ions. Once ionized, a hydrogen turns into a proton, hence, protic. An example of a triprotic acid is phosphoric acid

By definition, a polyprotic acid is one that has more than two ionizable hydrogens.