Question

Equilibrium Chemistry:

Assume that aqueous concentrations equal activities, and that reactions take place at 25 degrees celsius.

a). Consider the following reaction in a dilute solution:

O₂ (g) = O₂ (aq) K_eq=1.386*10^-3

The concentration of dissolved oxygen (O₂ (aq)) in wastewater is 10^-4 M. Assume that the activity of gaseous oxygen (O₂ (g)) equals the partial pressure in the atmosphere (P_O2 = 0.203 atm). Will O₂ (g) dissolve or evolve from the wastewater if T=25 degrees celsius?

b.) The mineral strontianite is strontium carbonate (SrCO₃). Its solubility product is 10^-8.8. The solubility product is the equilibrium constant for this reaction:

SrCO₃ (s) = Sr²⁺ (aq) +CO₃^2- (aq) K_eq = 10^-8.8

How much Sr²⁺ in mol/L would be present in solution at equilibrium if the CO₃^2- concentration is 3*10^-4 M?

Answer 1