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Dissociation vs Ionization
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Dissociation vs. Ionization
And a musical chemistry joke...
I showed you a chemistry joke, but
I didn't get much of a reaction.
I was going to do a better one,
but all the good ones argon.
Thank you!
- Most always occurs in water
- The polar water molecules pull apart ionic compounds (usually crystals) fairly easily
- Result is ions suspended in the water
Dissociation is the process of dissolving ionic
compounds into ions.
Ionization is the process of dissolving molecular (covalently bonded) compounds to produce ions.
Examples
NaCl(s) Na+(aq) + Cl-(aq)
Na2SO4 (s) 2 Na+(aq) + SO42-(aq)
(NH4)3PO4 (s) 3 NH4+(aq) + PO43-(aq)
NaOH(s) Na+(aq) + OH– (aq)
- This, too, is also usually always done in water
- However, in this process, the H+ ion leaves the compound to join the H2O
- This results in the ions being left behind, suspended in the water
Examples:
HCl (g) H+(aq) + Cl-(aq)
H2SO4 (g) 2 H+(aq) + SO42-(aq)
- Most molecular compounds will not undergo ionization
- Acids are an exception to this
- Most of what we are working with in class is the ionization of acids in water
HCl(g) + H2O(l) H3O+(aq) + Cl-(aq)
H2SO4 (g) + H2O(l) 2 H3O+(aq) + SO42-(aq)
Because the two are very similar, they are often confused with one another.
- We are working with mostly ionization reactions (acids in water)
- However, we use things such as the reaction's dissociation constant and percent dissociation
- Kinda sketchy
- This comes from the concept that the dissociation constant from water refers to its autoionization
- This is where the two terms become interchanged
- This allows the two terms to be used loosely and interchangeably
- We refer to dissociation when working with acids, although we should technically be calling it ionization
- There is a difference between the two!
Also, these are ions