in saline water there are h+ ions.
2006-08-29 01:17:14 · 7 answers · asked by RAHUL 1 in Science & Mathematics ➔ Chemistry
Hi there...
Rusting is an example of a corrosion reaction. All metals will corrode, but only iron takes part in rusting
The higher the mass gain, the more iron oxide (rust) is added to the iron. This means the conditions for rusting are best if oxygen, water and salt are present.
2006-08-29 01:23:46 · answer #1 · answered by Chiya 2 · 0⤊ 0⤋
it's faster in saline water. as for why: when iron rusts the flowing reactions happen: (the numbers in the parenthesis are the charge of the ions)
Fe -> Fe(+3) + 3e
H2O + 4e + O2 -> O(2-) + 2OH(-1)
the first one happens on the surface of the iron and the second one where air and water are in contact. in a saline water the presentation of ions will make the electron transfer easier so the iron will rust faster.
2006-08-29 01:29:32 · answer #2 · answered by CH4 3 · 0⤊ 0⤋
It rusts more in the saline water not because there are more H ions, but because the particles of salt hit the steel and damage it and therefore increase the surface on which oxygen and iron can react to create rust.
2006-08-29 01:23:14 · answer #3 · answered by Bax 2 · 0⤊ 0⤋
saline water does NOT have more H+ ions. for example, a solution of NaCl is saline water...
the iron does rust faster, due to more reactions that mostly involve the Cl- ion that attacks directly the iron, in presence of oxygen and water
2006-08-29 01:37:54 · answer #4 · answered by andreicnx 3 · 0⤊ 0⤋
no there is not H+ ions in saline! it's NaCl dissolved in water. Water stays bonded, but the Na+ and Cl- are solvated by the water. there can be other things in saline, but normally saline is just a salt solution.
2006-08-29 07:06:41 · answer #5 · answered by shiara_blade 6 · 0⤊ 0⤋
faster in saline water...
don't know why....but there is probably a link with the h+ions
2006-08-29 01:21:22 · answer #6 · answered by ycaruss y 3 · 0⤊ 1⤋
Doesn't saline have salt in it?
2006-08-29 01:23:23 · answer #7 · answered by suz' 5 · 0⤊ 0⤋