Chemistry Lesson One – Net Ionic Equations
Published by This is a quick Chem lesson over Net Ionic Equations that should help you make sense of it all.
To find out when a substance will ionize a solution you must first figure out if it is
1. Strong Acids: HCl, HBr, H2SO4, HI, HNO3, HCLO4, HCLO3
2. Strong Bases: Any Hydroxides of 1A and 2A. Example: KOH
3. Soluble Salts Example: NaCl
4. If the solution has NO3, NH4, Group IA metals, C2H3O2, CLO4, CLO3
Cl, Br, I Except with: Pb, Ag, Hg2
SO4 Except with: Pb, Ag, Hg2, Ca, Sr, Ba
If the substance doesn’t fit these rules it isn’t soluble, therefore cannot dissociate
Now you first step is to write out your equation-
Example:
Solutions of iron (II) nitrate and potassium hydroxide are mixed.
Fe(NO3)3 + KOH —-> Fe(OH) + KNO3
After writing this balance the equation and find out if it is gas, liquid, solid, and aqueous
Fe(NO3)3(AQ) + 3KOH(AQ) —-> Fe(OH)(S) + 3KNO3(AQ)
Next, Dissociate aqueous compounds into the total ionic equation and it will look like this
Fe + 3NO3 + 3K + 3OH —-> Fe(OH)3 + 3K + NO3
Now cross out the spectators that are on each side and you will have your net ionic equation
Fe + 3OH —-> Fe(OH)3
Thanks for reading and I hoped this helped you
DEJAY
Liked it
On December 5, 2009 at 6:58 am
I never was any good at chemistry. Interesting article.
On December 8, 2009 at 1:44 pm
I got highest marks in chemistry..
On December 9, 2009 at 7:26 am
ur lookin Einstein…great information
On December 27, 2009 at 2:10 am
This is awesome for any student. I disliked chem. Physics was my strong point. Where were u when I needed you? LOL
On January 19, 2010 at 2:54 pm
Seeking to widen my horizons I’d hoped for the new, however, you seem to be instructing in the standard way of proceeding while interacting as a person with a specialized interest in doing so in a time tested standard format.
On January 26, 2010 at 10:57 am
Thanks for trying to help us understand – I have a headache. LOL