1

Splash proof googles must be worn at all times! No food or drinks are allowed in the laboratory. Cover skin as much as possible; no open-toed shoes allowed. If you break any glassware inform your instructor immediately. Do not try to pick up the glass yourself. If a chemical spill occurs inform your instructor immediately. Do not try to clean up the spill, we have a special kit to clean up spills. At the end of each lab session clean the equipment and lab station for the next student. ASU policy- NOTHING goes down the drain!! Ask before you mix anything! One mistake and…. 2

3

Obtain 0.500g of copper wire weigh on a triple beam scale and placed in the bottom of a flask. Use mole to mole conversion to determine amount of 6 M HNO 3 (aq) and 6 M NaOH (aq). Use gram to gram conversion to determine amount of 2 M H 2 SO 4 (aq) and zinc. Pour 6 M HNO 3 (aq) into the flask under a fume hood After reaction takes place the reaction will be a light blue liquid and form Cu(NO 3 ) 2 (aq). Place flask into ice bath, slowly add 6 M NaOH (aq) Add Cu(NO 3 ) 2 (aq) until a solid forms at the bottom of the flask forming Cu(OH) 2 (s). Set up a filtration system, allow filtered solid to dry. Weigh solid and place solid back into flask. 4

Pour 2 M H 2 SO 4 (aq) into flask. Swirl flask until solid dissolves forming Cu 2 (SO) 4 (aq). Weigh out zinc on a triple beam scale and add to flask. Caution! Adding zinc will cause solution to be warm to the touch and bubble. Be cautious when handling! Add 3 M HCl (aq) into the flask and swirl the flask. Repeat until solution is a transparent colorless solution. Using the filtration system filter the solution and a solid should form. Allow the solid to dry and rinse solid with acetone to remove any impurities. Remove solid and place on a filter paper and weigh your solid on a triple beam scale. Observe your solid, if any black copper is present remove it and reweigh your solid. Use the percent yield equation to determine the amount of copper you recovered. To see an example of the copper cycle lab go to: What is a Copper Cycle?What is a Copper Cycle? 5

Solid copper reacts with aqueous nitric acid (HNO 3 (aq)) Cu (s) + 4HNO 3 (aq) Cu(NO 3 ) 2 (aq) + 2NO 2 (g) + 2H 2 O (l) Aqueous copper (II) nitrate reacts with aqueous sodium hydroxide (NaOH (aq)) Cu(NO 3 ) 2 (aq) + 2NaOH (aq) Cu(OH) 2 (s) + 2NaNO 3 (aq) Solid copper (II) hydroxide reacts with aqueous sulfuric acid (H 2 SO 4 (aq)) Cu(OH) 2 (s) + H 2 SO 4 (aq) CuSO 4 (aq) + 2H 2 O (l) Aqueous copper (II) sulfate reacts with solid zinc CuSO 4 (aq) + Zn (s) ZnSO 4 (aq) + Cu (s) Solid zinc reacts with aqueous hydrochloric acid (HCl (aq)) Zn (s) + 2HCl (aq) ZnCl 2 (aq) + H 2 (g) 6

7

8

9

Materials: (2) 250mL Beakers (2) 25mL Cylinders Approximately 1g of HCl (aq) 1g of NaHCO 3 (s) 1g of “unknown” Weighing paper Triple Beam Balance Scale 10

Measure out approximately 25mL HCl (aq) Measure out approximately 1g of NaHCO 3 (s) Mix HCl (aq) and NaHCO 3 (s) in a 250mL beaker. Once reaction stops weigh the mixture. Repeat three times for accuracy. Trial of HCl Mass Of NaHCO 3 Mass of Acid Mass After Reaction Mass of CO 2 Theoretical Mass of CO 2 Percent Error g24.55 g24.54 g0.982 g0.509 g93.9% g24.51 g24.67 g0.806 g0.506 g59.3% g24.50 g24.66 g0.840 g0.524 g60.3% 11

12

13

Measure out approximately 14g H 2 SO 4 (aq) Measure out approximately 1g of NaHCO 3 (s) Mix H 2 SO 4 (aq) and NaHCO 3 (s) in a 250mL beaker. Once reaction stops weigh the mixture. Repeat three times for accuracy. Trial Of H 2 SO 4 Mass Of NaHCO 3 Mass of Acid Mass After Reaction Mass of CO 2 Theoretical Mass of CO 2 Percent Error g13.195g13.234g0.950g0.518g83.4% g12.452g12.410g1.042g0.524g98.85% g12.820g12.480g1.337g0.522g % 14

15

Measure out approximately 25mL HCl (aq) Measure out approximately 1g of “unknown” Mix HCl (aq) and “unknown” in a 250mL beaker. Once reaction stops weigh the mixture. Repeat three times for accuracy. Trial of “Unknown” Mass of “Unknown” Mass of Acid Mass After Reaction Mass of CO 2 Mass of NaHCO 3 Percent Mass Composition 11.00g24.23g24.619g0.611g0.683g68.3% g24.09g24.459g0.631g0.705g70.5% g23.07g24.414g0.656g0.733g73.3% 16

17

18

It does not take a chemists to do chemistry. Following along with a procedure and using basic algebra anyone can do it and that includes YOU! Just remember to follow the lab safety rules! Think a chemistry major is not for you? Do these experiments plus more by taking CHM 113 at ASU and meet a general course requirement! Interested in chemistry? Check out the Department of Chemistry and Biochemistry at ASU! Department of Chemistry and Biochemistry 19