Chapter 14 - Acids and Bases

H2O

H2O

________ is never included because it is assumed to be constant.

covalent oxide

The reaction between a(n) ________ and water to form a Bronsted-Lowry acid can be defined as a Lewis acid- base reaction.

O¬X bond

If the ________ is ionic, the compound will produce a basic solution in water.

pH scale

The ________ is a compact way to represent solution acidity.

H¬O¬X

A compound containing the ________ group will produce an acidic solution in water if the O¬X bond is strong and covalent.

Kw

________ is the ion- product constant for water.

Calcium hydroxide

________, Ca(OH)2, often called slaked lime, is widely used in industry because it is inexpensive and plentiful.

Salts

________ that contain: Cations of strong bases and anions of strong acids produce neutral solutions.

Acids

________ were first recognized as a class of substances that taste sour.

hydroxide salts

Strong bases are ________, such as NaOH and KOH.

net effect

The ________ is to both polarize and weaken the O- H bond; this effect becomes more important as the number of attached oxygen atoms increases.

alkaline earth hydroxides

The ________ are not very soluble and are used only when the solubility factor is not important.

hydroxide ions

A base does not have to contain ________.

Arrhenius

________ postulated that acids produce hydrogen ions in an aqueous solution, while bases produce hydroxide ions.

Conjugate base

________: Everything that remains of the acid molecule after a proton is lost

polyprotic

A ________ acid has more than one acidic proton