To learn how to calculate ion concentrations in an aqueous solution of a strong diprotic acid.
Sulfuric acid, H2SO4, is a strong acid. Its complete dissociation in aqueous solution is represented as
H2SO4?H++HSO4?
A HSO4? anion can dissociate further by
HSO4??H++SO42?
but the extent of dissociation is considerably less than 100%. The equilibrium constant for the second dissociation step is expressed as
Ka2=[H+][SO42?][HSO4?]=0.012
Part A
Calculate the concentration of H+ ions in a 0.010 M aqueous solution of sulfuric acid.
Express your answer to three decimal places and include the appropriate units.


[H+] = 
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Part B
Calculate the concentration of SO42? ions in a 0.010 M aqueous solution of sulfuric acid.
Express your answer to four decimal places and include the appropriate units.


[SO42?] = 
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Part C
Calculate the concentration of HSO4? ions in a 0.010 M aqueous solution of sulfuric acid.
Express your answer to two significant figures and include the appropriate units.


[HSO4?] = 
1.0x10^2M solution of H2SO4.
Sulfuric acid is a strong acid for it's first dissociation, which
means it will dissociate completely to give us H+ and HSO4. HSO4
will also disassociate, but not completely. We will find out how
much:
initial species in solution: 1.0x10^2M H+, 1.0x10^2M HSO4,
H2O.
Since the initial concentration of SO4 2 is 0, we know that the
equilibrium will progress in the forward direction. Let X equal the
change in concentration.
.....................................
HSO4.................<>. H+....................+ SO4
2
Initial concentration........1.0x10^2........
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