Question

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.

Hints

[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.

Hints

[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.

Hints

[HSO4−] =

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