Chapter 10: Acids and Bases
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An Arrhenius acid dissociates to form ____.
H+ ions
An Arrhenius base dissociates to form ____.
OH-
A Bronsted acid ____________ H+
donates
A Bronsted base ____________ H+
accepts
Bronsted-Lowry acids and bases always occur in pairs because the definitions requires what?
The transfer of a proton from the acid to the base, aka conjugate acid-base pairs
A conjugate acid is ____.
a base with a hydrogen ion added to it in the reverse reaction, it is the H+ donor, thus it is an acid
A conjugate base is ____.
an acid with a hydrogen ion removed from it in the reverse reaction, it accepts H+, thus it is a base.
An ____________ species is one that reacts like an acid in a basic environment and like a base in an acidic environment.
amphoteric
In the Bronsted-Lowry sense, an amphoteric species can either gain or lose a proton, making it ____________ as well
amphiprotic
The partially dissociated conjugate base of a ________________ acid is usually amphoteric, e.g. HSO4-. The ____________ of certain metals, e.g. Al, Cr, Pb, Zn, are also amphoteric.
polyvalent; hydroxides
Complex amphoteric molecules include amino acids that have a ____________ intermediate with both cationic and anionic character.
zwitterion
Acids formed from anions with names that end in -ide have the prefix ________ and the ending ____.
hydro- -ic
Acids formed from oxyanions are called oxyacids. If the anion ends in -ite (less oxygen), then the acid will end in ________. If the anion ends in -ate (more oxygen), then the acid will end with ____ acid.
-ous acid -ic acid
What is the only thing that can affect Kw?
temperature! just like any other equilibrium constant
At temperatures above 298 K, Kw will increase. Why?
The autoionization reaction is endothermic
Strong acids and bases do what in aqueous solutions?
Completely dissociate
What do weak acids and bases do in aqueous solutions?
They partially dissociate
The smaller the Kb or Ka, the (stronger/weaker) a base or acid is.
weaker
Electronegative elements positioned near an acidic proton increase acid strength how?
they pull electron density out of the bond holding the acidic proton - this weakens proton bonding and facilitates dissociation
Acids and bases may react with each other to form a salt and often (not always) water. This is a ____________ reaction.
neutralization
In acid-base titrations, the equivalence point is reached when what?
the # of acid equivalents present equals the number of base equivalents, or vice versa
THe point at which the indicator changes to its final color is not the equivalence point, but rather the ____________
endpoint
Main differences between strong acid vs weak acid titration with strong base?
• initial pH is greater • strong acid has steeper/sudden rise in pH • equivalence point is greater than 7
Why do weak acid strong base titrations have pH > 7?
produces a weak conjugate base and even weaker conjugate acid - this means there are more OH- than H3O+