Acids Bases and Buffers - 5 Flashcards
Define a Bronsted-Lowry acid
Proton donor
Define a Bronsted-lowry base
Proton acceptor
Define Lewis acid
Electron pair acceptor
Define Lewis base
Electron pair donor
What ion causes a solution to become acidic
Oxonium ion
What causes a solution to become alkaline
-OH
Write an equation for the ionisation of water
2H20 —> H+ + OH-
Define strong acid
Dissociate completely in water
Name 3 strong acids
Hydrochloric acid
Sulphuric acid
Nitric acid
Define weak acids
Acids that only partially dissociate
Name 2 weak acids
Methanoic acid
Any organic acid
What is the symbol of acid dissociation constant
Ka
Write the acid dissociation constant expression
Ka = [H+] [A-] / [HA]
What does a larger Ka value mean
Larger the Ka - greater the extent of dissociation
Write the equation used to convert Ka into pKa
pKa = -log(Ka)
Write the equation used to convert pKa into Ka
Ka = 10^-pKa
What is the relation ship between pKa and the strength of an acid
Smaller the pKa, the stronger the acid
Write the equation used to convert concentration into pH
pH = -log[H+]
Write the equation used to convert pH into h+ conc
[H+] = 10 ^ -pH
Write the equation used to calculate [H+] of weak acids
[H+] = √(Ka * [HA])
Write the expression for the ionic product of water
Kw = [H+] [OH-]
What is the units for Kw
mol2 dm-6
What is the value of Kw at 298K
1 x10^-14
What physical factors affect Kw
Only temperature
