mcfaker123

Hello, I have been reading about the acid-base equilibrium in water. I dont understand what my book explains however. The theory may be information lacking(in my opinion). Because Ive read it so many times I just decided to rewrite everything exactly from my book! I also "rewrote" 2 examples after the theory. I am also confused about what they try to accomplish in the examples. I figure they try to set up the reaction of the acid-base equilibrium in water. In the second example they marked H3O+ & OH- in red, I dont know what that means though. Then next to "simplified" they let H3O+ react with NH3. How do I know whether H3O+ reacts with NH3 or with OH-? And why is it H3O+ that reacts with NH3 and not for example Cl- that reacts with H20 or NH4+? Im really confused with this material in my book & cant get out of it no matter what. Can anyone please help me? Thanks in advance! Theory: Example 1: Example 2:

Hello, Ive been seeing it everywhere" NAOH is a strong base". But in order for it to be strong, it has to meet the requirements which are: -The Kb of the reaction must be high. This means that base strenght is not determined by the dissociation % of a substance. Now I ve seen a lot of books say " NaOH is a strong base because it dissociates completely in water" But the dissociation of NaOH in water is not the same reaction as mentioned above right?So this is not a requirement for it to be a strong base! Can anyone help me out please because im stuck. Thanks in advance!

Hello, I have seen 2 kind of "lewis notations" for molecules, I will give an example: Is there anyone on this forum who is well familiar with the second notation? I Dont see any formal charge next to the S and other 2 O's, does that mean that the formal charges of S and the 2 O's are zero? Now if that is true im very confused then, because the first notation has 2+ as formal charge for S!! How is that possible? Im really confused here, could someone please help me out? Thanks in advance!!