Cu + 4HNO3 ---> 2H2O + 2NO2 + Cu(NO3)2

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After

 In this reaction we added HNO3 to the Cu, and heated it. This dissolved the copper strips and changed the solution to a light blue liquid of Cu(NO3)2. H2O and NO2 also formed, but evaporated into the air. The copper in the end is apart of the blue liquid.

Cu(NO3)2+2NaOH--> Cu(OH)2+2NaNO3

Before

During



After

In this reaction we started with the Cu(NO3)2 and added NaOH. Then took the new solution and put it over a hot plate stirring constantly until the solution changed to a black color. The color change signified that the solution had changed to Cu(OH)2 and NaNO3, which burned off with the heat. The ending copper is the black solid as the bottom of the beaker.

Cu(OH)2-->CuO+H2O

This is a double replacment reaction. This reaction occurs when cations and anions from two different componds mix to form two new compounds. This happens when the new product formed cannot be split into cations and anions, therefore a precipitate forms.

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During

After

In this reaction we poured the Cu(OH)2 into a vacummed filter so that the liquid (H20) seperated from the solid (CuO). The copper ended as a black solid in the filter paper. 

CuO+2HCl-->CuCl2+H2O

In this reaction we took the  solid CuO and added HCl. By doing this we balanced the pH level to 7, changing the color, and forming CuCl2 and H2O, resulting in copper being apart of a green liquid. 

Before

After

3CuCl2+2Na3PO4--->Cu3(PO4)2+6NaCl

This is a double replacment reaction. This reaction occurs when cations and anions from two different componds mix to form two new compounds. This happens when the new product formed cannot be split into cations and anions, therefore a precipitate forms.

In this reaction we took the CuCl2 and added Na3PO4. By doing this Cu3(PO4) was formed into a gel like solution that sunk to the bottom of the beaker, while NaCl floated on top. The ending copper result is apart of the blue gel. 

Before

After

Cu3(PO4)2+3H2SO4--->3CuSO4+2H3PO4

Before

In this reaction we took the filtered Cu3(PO4)2 solid, and put the funnel over our beaker. Next we poured in H2SO4 to dissolve the Cu3(PO4)2 into the beaker. After the compound was all dissolved it created CuSO4 and H3PO4. At the end of this reaction the copper is apart of a light blue liquid. 

After

Zn+CuSO4-->ZnSO4+Cu

Before

This is a single replacement reaction. This reaction occurs because the Zn is more reactive then the Cu and therefore trades places with the Cu to form the compound ZnSO4.

In this reaction Zn strips were added to the CuSO4 to seperate the Cu from the SO4, and get the Cu by itself. Next we stirred and waited for the Zn to dissolve and the solution to become colorless indicating it was done reacting. Once this happened, the solution was filtered again, and taken to a heater so it could dry, and be weighed. The final condition of the copper is a light red powder. 

After

Striving for Accuracy

#1

We carefully measured the 5 mL of NaOH by bending down to eye level so we could accurately see the meniscus and add the needed amount of the NaOH during the first reaction.

#2

We carefully and slowly added the Cu3(PO4)2 through the filter to make sure all the solid remained in the filter, and all the liquid passed through, with no cave ins during the 6th reaction.

#3

During this reaction we had to repeated add H2SO4 through our previously produced solid so that all of the solid would drain into the bottom of the beaker and no copper would be left behind, during the 6th reaction.

#4

During the second reaction we had to carefully and accurately stir the solution while the color shift happened. If we did not do this correctly the solution would have started to pop and we would've gotten dangerous chemicals on us.