Reaction 7-Cupric Sulfate to Copper

Zn(s) + CuSO4(aq) --> Cu(s) + ZnSO4(aq)

Put a few chunks of mossy zinc into the solution and allow to bubble away the blue. BLUE=BAD! When it's colorless, the excess zinc must be dissolved. To do this, add 2 M H2SO4 in one-ml portions. Keep adding until no more gas bubbles are produced. Allow red copper to settle. Filter the copper, let it sit. Weigh copper in filter paper. Subtract weight of filter paper.

Zinc, zinc, zinc it up!

Zinc bubbling away the blue.

Our liquid was finally clear rather than blue, with our copper in the bottom.

Sarah was making sure we didn't lose our copper by sucking it up from the table with a clean pipette!

This reaction is defined as single replacement because the SO4 goes from being attached to the Cu to instead the Zn through the reaction. The driving force is transfer of electrons, so it is a redox reaction and the Cu is formed as a solid because the CuSO4 dissolves away all the Zn.

Reaction 6-Cupric Phosphate to Cupric Sulfate

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

Dissolve solid by pouring 12 ml of 2 M H2SO4. Wash filter into beaker with distilled water until it is white.

ON THE MONEY! $$$

Anna was making sure we had the perfect amount of H2SO4 by measuring it to the bottom of the meniscus.

Reaction 5-Cupric Chloride to Cupric Phosphate

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

Neutralize solution with 8 M NaOH until liquid becomes cloudy. Add 6 M HCl until cloudiness disappears. The pH should be about 7. Add 15 ml 0.3 M Na3PO4. Allow precipitate to settle. Heat solution until it barely shows signs of boiling. Filter it, leave precipitate in funnel overnight.

Cloudy!

Clear!

Fascinated by precipitate!

Also making sure that a precipitate was created by adding a few extra drops of Na3PO4.

Hot, hot, hot!

We like Cupric Phosphate!

Reaction 4-Cupric Oxide to Cupric Chloride

CuO(s) + HCl(aq) -> CuCl2(aq) + H2O(l)

Put funnel with filter paper in beaker. Dissolve solid by pouring 8 ml 6 M HCl into funnel. Keep repeating until all of solid is dissolved into a green liquid.

Measure that HCl!

Make sure the filter paper turns all white!

We used a small amount of distilled water to clean all of the green color off of the filter in order to have correct results.

This reaction is a double replacement reaction. The driving force is formation of water. Water was formed because the oxygen combined with the hydrogen to form the compound.

Reaction 3-Cupric Hydroxide to Cupric Oxide

Cu(OH)2(s) --> CuO(s) + H2O(l)

Add distilled water until it reaches 100 ml in the beaker. Heat mixture until it turns black-ish. Filter it.

Thanks for being precise, Anna!

Anna added the perfect amount of distilled water by bringing the meniscus up to the 100 ml line on the beaker!

It changed colors!

We love chemistry!

Reaction 2-Cupric Nitrate to Cupric Hydroxide

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

Add 5 ml 8m NaOH to solution. Allow precipitate to settle. Test acidity of the liquid, should turn paper blue, so liquid is basic.

ACCURATE! :)

Sarah was accurate by getting down on eye level with the graduated cylinder and measuring the exact amount of NaOH.

PRECIPITATE! ;)

This is a double replacement reaction. The NO3 switches from the Cu to the Na and the OH switches from the Na to Cu. The reaction forms a precipitate (or solid), which is its driving force. This solid was formed because together, Na and NO3 are insoluble.

Reaction 1-Copper to Cupric Nitrate

Cu(s) + 4HNO3(aq) --> Cu(NO3)2(aq) + 2H2O(l) + 2NO2(g)

Add 5 ml 8 M Nitric Acid to the original copper sample in the beaker. Heat it gently. Dilute with 10 ml distilled water.

On the right level with the cylinder and beaker to be 100% sure of our results.

In the process of heating up...