In this lesson, we will learn how to use dissociation constants to find the equilibrium concentrations of undissociated acids and bases.
Q1:
A 1.00 L stock solution is prepared by dissolving 1.00 mole of a monoprotic acid in water. The 𝐾a value of the acid is 0.050. When calculating [H]+ 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 [H]+ relative to the true value.
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