Chapter 15 - Acids and Bases

Soren Sorensen

In 1909, ________ created a more practical metric termed pH.

Digestion

________ is facilitated by a lower pH (high acidity) of gastric juices, while higher pH blood is required to transport oxygen.

conjugate acids

Bases that are stronger than OH− react to OH− and their ________ with water.

Manganese

________ (VII) oxide (Mn2O7) and chromium (VI) oxide (CrO3) are two well- known examples of metal oxides that react with water to form acids.

Oxide ion

________ (O2),- for instance, is a stronger base than OH- and therefore reacts completely like this with water: − (aq) + H2O (l) par 2OH− | O2− (aq) (aq)

Salt

________ that contains an alkaline metal ion or an alkaline earth metal ion (excluding Be2+)

Na2CO3

The reactions between acidic oxides and the basic oxides and acids are similar to normal acid- based reactions as salt and water are the products: CO2 (g) 2NaOH (aq) ________ (aq) H2O (l) salt water base acidic oxide.

Ammonia

________ is a weak base.

H3O+

________ is the most potent and aqueous acid possible.

chloride ion

The ________ (Cl−), for example, is the conjugate base from HCl acid.

pH

The ________ of a solution with a pH meter is measured in the laboratory.

Ka

Where ________, the acid ionization constant, is the acid ionization equilibrium constant.

conjugate base

Its ________ has no measurable strength if an acid is strong.

OH−ion

The ________ is the most powerful base in aqueous solution.

Lewis acid

A(n) ________ is an atom or molecule that can receive two electrons.

Acid ionization

________ constitutes an important category of aqueous solution chemical balance.

H3O+

Acids that are stronger than ________ react to ________ and its conjugate bases by water.

Salts

________ are powerful electrolytes that break down fully into ions when exposed to water.