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.

0.00649M

The question is incomplete,


You are told that the first ionization of the sulfuric acid is complete and the second ionization of the sulfuric acid has a constant Ka₂ = 0.012


With that you can solve the question following these steps"


1) First ionization:


H₂SO₄(aq) --> H⁺ (aq) + HSO₄⁻ (aq)

Under the fully ionization assumption the concentration of HSO4- is the same of the acid = 0.01 M

2) Second ionization


HSO₄⁻ (aq) ⇄ H⁺ + SO₄²⁻ with a Ka₂ = 0.012


Do the mass balance:


        HSO₄⁻ (aq)        H⁺        SO₄²⁻

        0.01 M  - x          x            x

Ka₂ = [H⁺] [SO₄²⁻] / [HSO₄⁻]

=> Ka₂ = (x²) / (0.01 - x) = 0.012


3) Solve the equation:

x² = 0.012(0.01 - x) = 0.00012 - 0.012x

x² + 0.012x - 0.0012 = 0


Using the quadratic formula: x = 0.00649


So, the requested concentratioN is [SO₄²⁻] = 0.00649M

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