Chem Chapter 19 Acids and Bases
Terms in this set (47)
Compounds can be classified as acids or bases according to _____ different theories.
An _____ acid yields hydrogen ions in aquesous solution.
An Arrhenius base yields _____ in aqueous solution.
A Bronsted-Lowry acid is a ___ donor.
A Bronsted-Lowry base is a proton ______ .
In the Lewis Theory, an acid is an _____ acceptor.
A Lewis base is an electron-pair ____ .
An acid with one ionizable hydrogen atom is called a _____ acid, while an acid with two ionizable hydrogen atoms is called a _____ acid.
A ____ is a pair of substances related y the gain or loss of a hydrogen ion.
conjugate acid-base pair
A substance that can act as both an acid and a base is called ______ .
Tastes sour and will change the color of an acid-base indicator
An electron-pair donor
A water molecule that gains a hydrogen ion
hydronium ion (H3O+)
Acids that contain 3 ionizable hydrogens
Particle that remains when an acid has donated a hydrogen ion
An electron-pair acceptor
Acids that contain one ionizable hydrogen
Tastes bitter and feels slippery
Particle formed when a base gains a hydrogen ion
Water molecules can _____ to form hydrogen ions (H+) and hydroxide ions (OH-).
The concentrations of these ions in pure water at 25 degrees Celsius are both equal to ____ mol/L.
1.00 x 10^-7
The pH scale, which has a range from ____ , is used to denote the ____ concentration of a solution.
On this scale, 0 is strongly ____ , 14 is strongly ____, and 7 is ____ .
acidic; basic; neutral
Pure water at 25 degrees Celsius has a pH of _____ .
The _____ constant for water has a value of 1.0 x 10^-14
Thus, the product of the concentrations of ____ ions and ____ ions in aqueous solution will always equal 1.00 x
H+ or H3O+; OH-
Aqueous solution in which [H+] and [OH-] are equal
Product of hydrogen ion and hydroxide ion concentrations for water
Ion-product constant for water (Kw)
Solution in which [H+] is less than [OH-]
Reaction in which two water molecules produce ions
The negative logarithm of the hydrogen-ion concentration
Solution in which [H+] is greater than [OH-]
Ratio of the concentration of the dissociated (or ionized) form of an acid to the concentration of the undissociated acid
Acid dissociation constant (Ka)
Bases that dissociate completely into metal ions and hydroxide ions in aqueous solution
Acids that ionize completely in aqueous solution
Bases that do not dissociate completely in aqueous solution
Acids that are only partially ionized in aqueous solution
Ratio of concentration of conjugate acid times concentration of hydroxide ion to the concentration of conjugate base
Base dissociation constant (Kb)
Dissociate means ______
dissolve into ions
In the reaction of an ___ with a base, hydrogen ions and ___ ions react to produce ______ .
acid; hydroxide; water
This reaction, called ____ , is usually carried out by ______ .
The ____ in a titration is the point at which the solution is neutral.
At the ____ point of a titration, the number of equivalents of acid equals the number of equivalents of base.
A ____ is a laboratory method used to determine the concentration an acid or a _____ in solution by performing a ____ reaction with a standard solution.
titration; base; neutralization
At the ____ of the titration, the indicator changes color, which indicates neutralization.
Once neutralized, moles of ____ and moles of ____ are equal.
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