NaCl (aq) + HCl (aq) --> NaCl (s) + HCl (aq)
How does this reaction happen? Are there other acids that can perform a similar reaction?
2Na (s) + 2H2O(l) --> H2 (g) + 2NaOH (aq)
Is sodium metal a base in this reaction? why?
Co(H2O)6 (aq) + 4Cl (aq) --> CoCl4 (aq) + 6H2O (l)
Why shouldn't this reaction be conducted in school laboratories?
Please help, none of this makes sense to me...especially the first two
How does this reaction happen? Are there other acids that can perform a similar reaction?
2Na (s) + 2H2O(l) --> H2 (g) + 2NaOH (aq)
Is sodium metal a base in this reaction? why?
Co(H2O)6 (aq) + 4Cl (aq) --> CoCl4 (aq) + 6H2O (l)
Why shouldn't this reaction be conducted in school laboratories?
Please help, none of this makes sense to me...especially the first two
-
NaCl (aq) + HCl (aq) --> NaCl (s) + HCl (aq)
How does this reaction happen? Are there other acids that can perform a similar reaction?
==============
No. This reaction is nonsense. NaCl is soluble in water.
2Na (s) + 2H2O(l) --> H2 (g) + 2NaOH (aq)
Is sodium metal a base in this reaction? why?
============
This is not an acid/base reaction using Arrhenius theory. Nor is it an acid/base reaction using the Bronsted-Lowry theory, since Na is not an proton acceptor. In the Lewis theory, a base is an electron pair donor and an acid is an electron pair acceptor. Doesn't work either since Na ends up as Na+ ions and not bonded to any other element.
Co(H2O)6 (aq) + 4Cl (aq) --> CoCl4 (aq) + 6H2O (l)
Why shouldn't this reaction be conducted in school laboratories?
==============
Why not? I have run this lab with my AP chemistry students many times. Cobalt can be nasty, but only if you drink it or rub it on your skin. The Cl should be Cl- and it comes in the form of concentrated HCl, but this is done dropwise and really poses the only risk, which can be minimized.
How does this reaction happen? Are there other acids that can perform a similar reaction?
==============
No. This reaction is nonsense. NaCl is soluble in water.
2Na (s) + 2H2O(l) --> H2 (g) + 2NaOH (aq)
Is sodium metal a base in this reaction? why?
============
This is not an acid/base reaction using Arrhenius theory. Nor is it an acid/base reaction using the Bronsted-Lowry theory, since Na is not an proton acceptor. In the Lewis theory, a base is an electron pair donor and an acid is an electron pair acceptor. Doesn't work either since Na ends up as Na+ ions and not bonded to any other element.
Co(H2O)6 (aq) + 4Cl (aq) --> CoCl4 (aq) + 6H2O (l)
Why shouldn't this reaction be conducted in school laboratories?
==============
Why not? I have run this lab with my AP chemistry students many times. Cobalt can be nasty, but only if you drink it or rub it on your skin. The Cl should be Cl- and it comes in the form of concentrated HCl, but this is done dropwise and really poses the only risk, which can be minimized.