syre base kemi
Write the products of the following acid-base reactions:
(a) CH3OH + H2SO4 <--> ?
(b) CH3OH + NaNH2 <--> ?
(c) CH3NH3 + Cl- + NaOH <--> ?
- I do not necessarily need the solutions but what I REALLY need help in is understanding why one reactant is more acidic/basic than the other or even how I would calculate this. I actually have the textbook solutions already BUT I don't undeerstand how the book got to these answers.
(a) The solutions manual provided this to me:
CH3OH (Stronger Base) + H2SO4 (Stronger Acid) <--> CH3OH2+ (Weaker Acid) + HSO4- (Weaker Base)
My first questions from come from seeing this solution:
1. How do I determine which one is base/acid between the reactants? Both Methanol and Sulfuric acid has lone pairs and Hydrogen atoms, so why is Sulfuric acid the one to give up the H+. How did you determine, comparing to Methanol, that Sulfuric Acid was the one to give up the H+ vs the Methanol?
2. When the H+ moved from Sulfuric Acid to Methanol, why would it attach to Methanol vs just being a floating H+ ion in the products side?