Net Reactions or Net Ionic Equations are just a simplified version of a reaction involving the forming of a precipitate. Note: A net Ionic Equation can only occur if one of the products in a double replacement reaction is a solid.
A Net Ionic Equation is written using the following steps:
1. Write, predict and balance the complete reaction with state subscripts written in.
2. If a solid is formed, write out the complete equation separating all ions from one another except the ones forming the solid with the charges and state subscripts written in.
3. Cross out any ions found on both sides of the equation.
4. Write out the remaining ions and compounds in a reaction.
Example:
| Step 1: |
| ___BaCl2 (aq) | + | ___Na2CO3 (aq) |  | ___BaCO3 (s) | + | _2__NaCl (aq) |
| Step 2: |
| _Ba2+(aq) | + | 2Cl - (aq) | + | 2Na +(aq) | + | CO3 2-(aq) | | ___BaCO3 (s) | + | 2Na +(aq) | + | 2Cl- (aq) |
Ba 2+ (aq) | + | CO32- (aq) | | BaCO3(s) |
In order to tell whether or not a chemical reaction can occur, one must determine the solubility of the products.
Use the following link to determine whether or not a compound or soluble or not / barely soluble.
http://dl.clackamas.edu/ch105-03/solubili.htm
If one of the products is not or barely soluble then a precipitate or solid forms meaning that a reaction has occurred.
If both the products are soluble meaning they are aqueous then a reaction has not occurred.
Examples:
| NaOH | Fe2S3 | MgSO4 | PbCl2 | Ba(NO3)2 | MgCO3 |
| soluble | insoluble | soluble | insoluble | soluble | insoluble |
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