I have a question about solubility rules and net ionic equations
so for example :
CuSO4+Ba(NO3)2----->BaSO4+Cu(NO3)2 Okay so I know BaSO4 is insoluble while Cu(NO3)is solulable, that means BaSO4 will have a precipitate while Cu(NO3) doesn't. So does that mean the overall equation will have a reaction because one of the two compounds has a precipitate?
IN other words in an equation if both compounds have a precipitate and are insoluble will there be a reaction? what if it's only one compound with a precipitate/is insoluble like the example that I gave above, will there be a reaction? what if they both are soluble/don't have a precipitate will there be a reaction?
Thanks!
The rules I remember for reactions:
1. A rxn will occur if a (a meaning one) ppt forms. It goes without saying that if two ppts form there will be a reaction also.
Your rxn is an example.
2. A rxn will occur if a gas is formed. Example:
2Na + H2O ==> 2NaOH + H2
3. A rxn will occur if a weak electrolyte is formed. Example:
NaOH + HCl ==> NaCl + H2O (H2O is the weak electrolyte; i.e., slightly ionized).
4. Redox reactions occur if the voltage between the two is positive.
Here is why those rules apply. Reactions occur if anything happens to force the equilibrium of the reaction to the right producing more products.
1. Formation of a ppt. The ppt essentially leaves the field of reaction (because it's insoluble), the reverse reaction can't take place because the ppt is not soluble so reactants continue to form ppt until all of the reactants are used. Most of the ppt reactions take place at close to 100%.
2. A gas is formed. This is another case where the gas leaves the field of reaction; therefore, no reverse reaction can take place and the reactants continue to produce more products until all of the reactants are gone.
3. A weak electrolyte is formed. Another case in which the weak electrolyte leaves the field of reaction and the reverse reaction can't continue as well as the forward reaction.
4. Redox. These reactions have their own rules.
Hope this helps.
To determine if there will be a reaction or not, you need to consider the solubility rules and write the net ionic equation.
In the given example, CuSO4 + Ba(NO3)2 -> BaSO4 + Cu(NO3)2, you correctly stated that BaSO4 is insoluble and Cu(NO3)2 is soluble. This means that BaSO4 will precipitate out of the solution, while Cu(NO3)2 will remain in the solution as ions.
To write the net ionic equation, you first need to write the balanced molecular equation: CuSO4 + Ba(NO3)2 -> BaSO4 + Cu(NO3)2. Then, you need to determine the states of the compounds. CuSO4 and Ba(NO3)2 are usually soluble, so they remain as ions in the solution, whereas BaSO4 is insoluble and precipitates out. Cu(NO3)2 remains as ions in the solution.
The net ionic equation only includes the species that are directly involved in the reaction. In this case, the net ionic equation would be: Ba^2+ + SO4^2- -> BaSO4. This equation shows the formation of the insoluble BaSO4 precipitate.
Now, to answer your questions:
1. If both compounds are insoluble, meaning both have precipitates, there will be a reaction. The reaction results in the formation of the insoluble precipitate.
2. If only one compound has a precipitate/is insoluble, there will still be a reaction. The soluble compound will remain in the solution as ions, while the insoluble compound will precipitate.
3. If both compounds are soluble/don't have a precipitate, there will not be a reaction. The compounds will remain dissolved in the solution.
It is important to consult solubility tables to determine the solubility of compounds and identify if a precipitate will form or not.