We’re being asked to calculate the pH solution containing 0.1 M weak acid HA at equilibrium and 10 M conjugate base (A-)
Remember that weak acids partially dissociate in water and that acids donate H+ to the base (water in this case). The dissociation of HA is as follows:
HA(aq) + H2O(l) ⇌ H3O+(aq) + A–(aq); Ka = 1.0× 10–1
From this, we can construct an ICE table. Remember that liquids are ignored in the ICE table.
An acid, HA, has a Ka value = 1.0 × 10-1. At equilibrium, a solution of this acid is found to have a concentration, [HA]eq = 0.1 M. If the concentration of the conjugate base is 10 M, what is the pH of the solution?
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