Making Insoluble Salts by Precipitation. Aim: to observe what happens when two solutions are mixed and to use the data obtained to establish rules of solubility for a number of salts.

Results:

Equations:

1))

1):  2Ag(NO)3(aq) + Na2SO4(aq) => Ag2SO4(s) + 2NaNO3(aq)

2Ag(aq) + SO4(aq) => Ag2SO4(s)

2):Zn(NO3)2(aq) + Na2CO3(aq) => ZnCO3(s) + 2NaNO3(aq)

Zn (2+) + CO3 (2-) => ZnCO3(s)

3): 2NH4NO3(aq) + Na2SO4(aq) => (NH4)2SO4(s) + 2NaNO3(aq)

2(NH4) + SO4 → (NH4)2SO4 

4):2AgNO3(aq) + NaCl(aq) => Ag2Cl(s) + 2NaNO3(aq)

2Ag (+) + Cl (2-) => Ag2Cl(s)

5):2AgNO3(aq) + Na2CO3(aq) => Ag2CO3(s) + 2NaNO3(aq)

2Ag(+) + CO3(2-) => Ag2CO3

2))

1. Zn(NO3)2(aq) + Na2SO4(aq) => ZnSO4(aq) + 2NaNO3(aq)
2. 2Ag(NO3)3(aq) + 3NaSO4(aq) => Al2(SO4)3(s) + 6NaNO3(aq)

Conclusion:

During this experiment we have become familiar with two type of solutions. One a precipitate solution, the other a clear solution. Either of these states could be coloured.

In conclusion, we can see that the salts that seem to dissolve the most, are Chloride, Bromine, Sodium Potassium, Ammonium, Calcium and Iodide, as they have solutions which are mostly found clear and colourless, most likely meaning that these salts formed by these elements are going to be more soluble then the other salts.

The other salts forming coloured and precipitated solutions, are most likely going to be less soluble, then the other these salts.