<p>Hello, guys!</p>
<p>Is a dissociation of ionic compounds to its individual ions considered as the decomposition reaction? Are both acid and base ionic molecules?</p>
<p>Also is burette more precise than the graduated cylinder in general?</p>
<p>My textbook (Chang 10th edition) defines decomposition reactions as a subset of redox reactions, so I wouldn’t think so. I’m not sure what you mean your second question, but if you look at the structure of many acids and bases you’ll see that several are covalent molecules. Burettes are certainly more precise than most graduated cylinders.</p>
<p>No. NaCl (aq) can be found as Na+ and Cl- in a solution. It isn’t the decomposition of NaCl, though, because it’s still considered as NaCl. The ionic compounds are just breaking themselves up into parts, like ripping paper. The parts are still considered as the said ionic compound, just like the ripped paper is still considered paper. Dissociation is just a physical change. Decomposition is a chemical one… I hope this makes sense. </p>
<p>As for acids and bases being ionic compounds, yes they are always. Arrhenius definition says that all acids and bases dissociate to produce OH- and H+ IONS. So, obviously, they must all be ionic. </p>
<p>Also, burettes are more precise than graduated cylinders. They are made to be that way… Specifically for measuring small amounts.</p>
<p>:)</p>
<p>@myraven11
I’m not so sure about all acids and bases being ionic compounds. You seem to define an ionic compound by what it does, not by the structure of the compound itself. This has some problems - not all ionic compounds dissociate in water (hence why you need the solubility rules). In addition, several organic acids fail to meet various criteria needed for ionic compounds - the oxygen and hydrogen atoms in acetic acid, for example, are held together by covalent bonds. It doesn’t form a crystal lattice. And this definition cannot account for some Lewis acids.</p>
<p>@aldfig0
If you read the OP, you’ll see that the question asked was about the difference between ionic dissociation and decomposition. When I mentioned NaCl and other ionic compounds, it was to provide an EXAMPLE. A correct one at that. Idk who was talking about crystal lattices and solubility rules… That’s very irrelevant to this discussion. </p>
<p>And what are you talking about? Even if H+ and OH- ions don’t apply, all Lewis acids still have to accept electrons. They consist of ions… Therefore they’re ionic. 
</p>
<p>Thanks for trying though!</p>