unit 5-Acids, bases & buffers Flashcards
(26 cards)
What is a Bronsted-Lowry acid?
Proton donor.
What is a Bronsted-Lowry base?
Proton acceptor.
What is a Lewis base?
Accepts electron pair.
What is a Lewis acid?
Donates electron pair.
What is a monobasic acid?
When one mole of an acid donates one mole of H+ ion to a base.
What is a dibasic acid?
An acid that donates two H+ ions to a base.
What is a tribasic acid?
An acid that donates three H+ ions to a base.
What differs in the reaction when an acid donates more than one proton to a base? Why?
On the second substitution the reaction becomes reversible because the acid becomes weaker after losing a proton.
What are conjugate acid-base pairs?
A set of two species that can transform into each other by the gain or loss of a proton.
How would you calculate [H+]?
[H+]= 10^-pH
How would you calculate pH?
-log10[H+]
For strong acids, what does [HA] equal?
[HA]=[H+]
What is Ka used for?
Weak acids that don’t fully dissociate.
What is the expression for Ka?
Ka= [H+][A-] / [HA]
What does it mean if an acid has a large Ka value?
There is a large extent of disassociation meaning that it is a strong acid.
How would you calculate pKa?
pKa= -log10Ka
How would you calculate Ka from pKa?
Ka=10^-pKa
In weak acids, what is [H+] equal to?
[H+]=[A-]
For weak acids, what is the equation for Ka?
Ka= [H+]^2 / [HA]
Why is water neutral?
[H+]=[OH-]
What is the expression for Kw?
Kw=[H+][OH-]
What are the units of Kw?
mol^2dm^-6
What are the expressions of pOH?
pOH=-log10[OH-]
[OH]=10^-pOH
What does a low pKa value mean about the strength of the acid?
Strong acid.
