Aqueous reactions

Lab #4: Aqueous Reactions
Introduction:
In this experiment we studied the two different types of aqueous chemical reactions, double replacement and single replacement. In a double replacement reaction one or both of the products is an insoluble ionic compound or otherwise known as a precipitate; or a non-electrolyte; or a gas. In a single replacement reaction there is typically a metal and an ionic compound consisting of a metal cation and a non-meatl anion. Singel replacement ractions occur when the reacting element is more active, whihch means it is more likely to lose electrons than the product element. There was two parts to this experiment, in Part A we mixed various aqueous solutions of ionic compounds and observed if a reaction occurred or not. A reaction occurred if a precipatate was formed, a gas was evolved, or a non-electrolyte was produced. In Part B of this experiment we mixed various metals with aqueous solutions and acid and observed the results. Then we determined the activity order of the metals used based upon our results.
Data Sheet:
Part A:
Reaction #1A:
Na2CO3(aq) + HCL(aq)(0.5m)  H2CO3(g) + 2NaCl(l) H2O(l) + CO2(g) + 2NaCl(l)
Observations:
There was a formation of a gas and the liquid was clear.
Reaction #2A:
Na2CO3(aq) + NaCl(aq)  Na2CO3(aq) + NaCl(aq)
Observation:
No reaction was observed.
Reaction#3A:
Na2CO3(aq) + CaCl2(aq)  2NaCl(aq) + CaCO3(s)
Observations:
The solution turned white and cloudy which is evidence that a perticipate was formed.
Reaction #4A:
NaOH(aq) + HCl(aq)(0.5m)  H2O(l) + NaCl(aq)
Observations:
A clear gas was formed.
Reaction #5A:
NaOH(aq) + Mg(NO3)2(aq)  2 NaNO3(aq) + Mg(OH)(s)
Observations:
The solution turned slightly cloudy.
Reaction #6A:
Na2SO4(aq) + BaCl2(aq)  Na2Cl2(l) + BaSO4(s)
Observations:
The solution turned white and cloudy.
Reaction #7A:
Na2SO4(aq) + Cu(NO3)2(aq)  CuSO4(aq) + 2NaNO3(aq)
Observations:
The solution was slightly tinted blue due to the copper, but it