Question- Enough of a monoprotic acid is dissolved in water to produce a 0.0124 M solution. The pH of the resulting solution is 6.24. Calculate the Ka for the acid.
In this case, the inital 10-7 M H from water is not negligible. If [H ]iniital = 10-7 and [H ]final = 5.8 × 10-7, by how much did the concentration change? What does that say about how much A- was produced?
Give your answer with short explanation