in acid-catalyzed reaction,there are some books show the acid catalyst as H+ and there are some show it as H3O+ .Are they the same?
Short=yes they are. Long version Traditionally, acids were defined to be compounds that produce H+ ions when dissoved in water (Arrhenius theory). But this definition is limited to acids that can be dissolved in water. Br?nsted-Lowry then formed a definition which states that acids are compounds which donates a protons or H+ ions. If u think about it, a H+ ion is practically a proton. a proton with no electron outer shell is far too reactive to stay in its current state. thus it will form a bond with H2O to form H3O+ Because of this, acid catalysts are supose to be H3O+ instead of H+. But since it is more convinient to use H+, the form of writing H+ remained instead....... and yes...... the scientists were lazy......
H+ is the ion contained in acids.... When acids are dissolved in water (H+)+(H2O)=H3O+ Both are the same......
Sort of. If the reaction is under aqueous conditions (any water is included in the reaction), then yes, H+ = H3O+. This is because free protons present (H+) will be coordinated generally to molecules of water [thus H2O + H+ =H3O+ ]. But there are reaction conditions where water is not present, but an acid catalyst is still possible. In these cases, the acid catalyst may frequently be indicated as simply H+. Either way, the function in most of your reaction mechanisms is basically the same, whether indicated as H+ or H3O+ -- and that's to protonate molecules (Lewis or Bronsted bases) with H+. Concentrated sulfuric acid would be an example of a mostly-anhydrous (no water) strong proton/acid source (H+). Hydrochloric acid (HCl) frequently is available as an aqueous solution, even concentrated HCl is an aqueous solution of HCl. HCl itself is a gas under ambient conditions... but it has solubility in water and thus is conveniently sold frequently as an aqueous solution (which could be represented as H3O+)
