Different Reactions

There were many different reactions that took place in the lab. Here's a look at two important ones

SINGLE REPLACEMENT
There was one single replacement reaction that took place in this lab during step 7, demonstrated by the equation:
                                Zn + CuSO4 -> ZnSO4 + Cu

The driving force of this reaction was the transfer of electrons, through different levels of acitivity seires in the metals present. The copper sulfate solution that we added the zinc to had a higher acivity level than the copper; therefore, the copper was replaced by the zinc in the  bond.

DOUBLE REPLACEMENT

There were also two double replacement reactions that occured in our lab. In step 5, the reaction

                              3CuCl2 + 2NaPO3 -> Cu3(PO4)2 + 2NaCl

In step 4, we also witnessed the double replacement reaction

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

In both reactions, the driving force is the formation of a solid, which in this case is called a precipatate. In these cases, one precipatate was formed when two liquids where put together. In step 5, the precipitate that was formed was the cupric phosphate, because neither the copper, nor the phosphate dissolves in water. However, the sodium chloride remained in its aqueos state, because both elements are soluble. In step 2, nearly the same scenario applies. The product copper hydroxide was formed because neither the hydroxide nor the copper was soluble, while the very soluble nitrate and sodium ions remained dissolved in the solution.

Striving for Acccuracy

Throughout this lab, we demonstated many different techniques of striving for accruacy and craftsmanship.

Lauren demonstrates striving for accuracy by re-reading the directions and constantly stirring the mixture on the hot plate.

Madison shows striving for accuracy by bending down to eye level to measure "accurately."

Here we spend time washing the bits of copper from the left over solid zinc in the solution so that all of our copper is accounted for.

And here we seal the vacume by pushing down on the funnel, preventing the ridges from obstructing the air tight structure.

Part G

The final reation in Part G involves the replacement of copper with zinc. Zinc reacts with the cupric sulfate solution forming zinc sulfate solution and copper. This was a single replacement reaction.

Zn + CuSO4 -> ZnSO4 + Cu

Before starting the reaction, we weighed our filter paper to subtract from our final weight.

We added 2 grams of zinc to the cupric sulfate...

...and waited and stirred and waited and stirred.

We ended up with an ugly gray solution of zinc sulfate and copper at the bottom.

Then very carefully (striving for accuracy) we picked out the remaining zing with plastic tweezers and washed the remains of copper back into the beaker.

Finally, we ended up with our original copper and put the solution through another vacume to isolate the solid copper.

Part F

Part F involves another acid-base neutralization reaction as sulfuric acid dissolves the cupric phosphate to produce a blue cupric sulfate solution and phosphoric acid.

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

First, the solution was heated on low.

Then it was put through another vacume and wash procedure to get rid of the H2O.

Finally, we added the acidic H2SO4 to the cupric phosphate to create a clear blue cupric sulfate solution.

Part E

Part E involves a reaction between the cupric chloride solution and a solution of sodioum phosphate to produce a blue cupric phospate and soduim chloride. This is an example of a double replacement reaction.

3CuCl2 + 2NaPO4 -> Cu3(PO4)2 + 6 NaCl

Measuring out the sodium phosphate!

Here the solid just begins to form between the cupric chloride and sodium phosphate that eventually forms into the cloudy liquid found below.

Part D

The black cupric oxide solid undergoes an acid-base neutralization reaction with aqueous hydrochloric acid to form a green cupric chloride salt solution, and water.

CuO + 2HCl -> CuCl2 + H2O

Here, the black cupric oxide solution was vacumed to extract all of the water and isolate the cupric oxide.

When this was done, HCl was added to the Cupric oxide to create a cupric chloride salt solution.

Part C

 Part C- The blue cupric hydroxide is decomposed with heating into black cupric oxide solid and water. This is an example of a double replacement reaction

Cu(OH)2 + E(heat) à CuO + H2O

After stirring on the hot plate for 3 minutes, the cupric nitrate turned from blue to black and solid copper formed in the solution

Part A

Part A

Copper metal is oxidized by nitric acid to produce a blue solution containing aqueous cupric nitrate and water and nitrogen dioxide, a brown, poisinous gas.

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

During the first 2 minutes of the reaction- the copper has not dissolved and the blue liquid is just beginning to form

The copper is nearly all dissolved and the blue cupric nitrate has formed.