I'm trying to reach a more thorough understanding of what's going on when we calculate equilibrium concentrations and was wanting to understand more what assumptions we make in order to follow through with the calculations. Let me ask off of an example: Consider mixing equal amounts of NH3 and HCl, each having the concentration of α upon mixing. The general way I've seen taught is to assume via being a strong acid that the HCl fully ionizes and causes the following equation to occur: NH3 + H30+ → NH4+ + H2O Then to recognize that NH4+ is a weak acid, so we'll need to set up the reverse equation as an equilibrium to run an ICE problem off of: NH4+ + H2O ←→ NH3 + H30+ Wherein we take the initial concentration of NH4+ to be α, and can use it's Ka to find the final hydrogen ion concentration of the entire solution. Here then are my questions directly: 1) In the first equation, we seem to assume that all the hydrogen ions from HCl jump onto our NH3, thus allowing us to use our initial α concentration also as the initial concentration of NH4+. How so? Could it not be that some hydrogen ions tend to stick around as H30+, thereby reducing the actual concentration of NH4+ to slightly less than α? What knowledge/assumptions do we use to reduce this complexity from our calculations? 2) Are there any other important assumptions we make when working similar equilibrium problems? As I work them myself, I constantly feel like the scenarios are a bit oversimplified (even if I acknowledge they give us answers very proximal to reality). Thanks much!