Write an equation for the Brønsted–Lowry acid–base reaction that occurs when each of the following acids react with water. Show all unshared electron pairs and formal charges, and use curved arrows to track electron movement.
So, here we've got something kind of interesting, right? We've got an ester but guys look at this right here, it's pronated, right? So it means that it's got a lone pair and a positive charge, right? When it likes to have two bonds here, it has three, so it's got a positive charge and really wants to give away that hydrogen, so that's where our water comes in, comes in with its lone pair, grab the hydrogen, kick electrons onto that O and then we end up with our H3C, C double bond O with now two lone pairs, our O down here, with two lone pairs, right? That it exactly the same and then we've got our CH3 and again we have our hydronium, which is going to have a positive charge and one lone pair, totally drawing behind me right now, sorry about that, there it is, Guys if you have any questions feel free to let me know, if not, let's move on.