Why, when an ammonia solution is titrated with a strong acid, the #pH# remains relatively constant up to the addition of a stoichiometric quantity of the acid?
Because you have described formation of a buffer solution.........
This is seen from the well-known buffer equation, the which we may represent as:
In this ammoniacal scenario, the free base is the uncharged species, the ammonia, and the ammonium acid is charged:
Many students have difficulties with the logarithmic function. I do not suggest that you do. But I can encourage you and others not to be intimidated when you see a
Back in the day, before the advent of electronic calculators, students (and scientists, and engineers, statisticians, and economists) would routinely use log tables to do calculations that a calculator would these days render trivial.