Solution-Equilibrium concentrations using equilibrium

Equilibrium concentrations using equilibrium constant

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Reference no: EM132650853

Describe equilibrium reactions and be able to calculate equilibrium concentrations using equilibrium constant expressions and the ICE method.

There are 3 questions; each worth 5 points each. Show all of your work for full credit.

i) A weak monoprotic acid has a Ka = 1.8 x 10-5. The generic equation is:

HA(aq) + H2O(l) ↔A-1(aq) + H3O+1(aq)

If the initial concentration of HA is 0.222 M, determine the equilibrium concertation of all three aqueous species at equilibrium.

ii) 0.200 moles of HA was put into solution and it came to equilibrium. The final A-1(aq) and H3O+1(aq) concentrations at equilibrium were 1.65 x 10-4 M. Determine the Kc.

iii) The Ka for a strong acid is 1 x 103. If 0.345 moles of HA is dissolved in 1 liter of water, then what will be the final concentration of A-1(aq)?

Reference no: EM132650853

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Equilibrium concentrations using equilibrium constant

Reference no: EM132650853

Reference no: EM132650853

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