Worksheet: Concentrations from Ionization Constants
In this worksheet, we will practice using dissociation constants to find the equilibrium concentrations of undissociated acids and bases.
When dealing with acid and base solutions, when is it necessary to use equilibrium calculations to accurately determine equilibrium concentrations?
- AIn nonaqueous systems
- BWhen the temperature is not
- COnly at very low concentrations
- DWhen a strong acid or base is involved
- EWhen a weak acid or base is involved
A 1.00 L stock solution is prepared by dissolving 1.00 mole of a monoprotic acid in water. The value of the acid is 0.050. When calculating at equilibrium, a student assumes that the change in concentration of the undissociated acid is negligible. Calculate to 2 significant figures the percentage error in the calculated value of relative to the true value.