CHEMICAL REACTIONS
Chemical Reactions
How do you know that a chemical reaction has taken place? What are the products of a chemical reaction? Can you predict whether or not a chemical change will take place?
Equipment/Materials:
| |microtitration plate |0.1 M Pb(NO3)2 |
| |Beaker |0.1 M HC2H3O2 |
| |magnesium metal |0.1 M KI |
| |zinc metal |0.1 M CuSO4 |
| |copper metal |0.1 M AgNO3 |
| |3 M HCl |0.1 M NaOH |
| |Na2SO3 (solid) |0.1 M NaCl |
| |NaHCO3 (solid) | |
Safety Considerations:
• Wear goggles and aprons at all times in the lab.
• Use caution when smelling any substance. Remember to WAFT!
• Acids are corrosive and can cause severe burns. Be careful!
• Silver nitrate will stain skin and clothing
Procedure:
Mixing of aqueous solutions – mix together 5 drops each of the following solutions and observe:
1. 0.1 M Pb(NO3)2 with 0.1 M KI
2. 0.1 M CuSO4 with 0.1 M NaOH
3. 0.1 M CuSO4 with 0.1 M NaCl
4. 0.1 M AgNO3 with 0.1 M NaCl
5. 0.1 M AgNO3 with 0.1 M KI
Mixing of Powders and Liquids – mix about 0.2 g (a portion about half the size of a paper match head) of each solid with about 5 drops of the liquid specified and observe: WARNING: Concentrated acids are corrosive! If any contact with skin or clothing occurs, immediately wash the area with large amounts of water and then inform your instructor.
6. solid NaHCO3 with HC2H3O2 (CH3COOH)
7. solid Na2SO3 with 3M HCl NOTE: See warning above!
8. solid NaHCO3 with 3 M HCl NOTE: See warning above!
Mixing of Metals and Liquids – Mix a piece of each metal with 8 drops of the liquid specified and observe:
9. zinc metal with 0.1 M CuSO4
10. zinc metal with 3 M HCl NOTE: See warning above!
11. copper metal with 3 M HCl NOTE: See warning above!
12. magnesium metal with 3 M HCl NOTE: See warning above!
13. copper metal with AgNO3
Data Table
|Reaction |Observations |Word Equation |Balanced Chemical Equation |Net Ionic Equation |
|Number | | | | |
|1 | | | | |
|2 | | | | |
|3 | | | | |
|4 | | | | |
|5 | | | | |
|6 | | | | |
|7 | | | | |
|8 | | | | |
|9 | | | | |
|Reaction |Observations |Word Equation |Balanced Chemical Equation |Net Ionic Equation |
|Number | | | | |
|10 | | | | |
|11 | | | | |
|12 | | | | |
|13 | | | | |
Questions:
1. Write a WORD equation that would state what happened for each chemical reaction (use a pencil). Have this approved before moving to step 2
2. Write the balanced chemical equation for each reaction in the space provided, include phase symbols when known. If no reaction occurs, write NR.
3. What things did you observe that indicated a chemical change took place?
3. Using the activity series, look at reactions 9-13 and determine whether or not they “follow the rules”.
4. Using the activity series, determine whether or not the following substances would react. If there is a reaction, write the balanced equation.
Prediction (yes or no)
_________ Zinc and sodium chloride ______________________________________________________________________
_________ Copper and potassium iodide ____________________________________________________________________
_________ Magnesium and copper II sulfate __________________________________________________________________
Extension
1. Use the solubility table to determine the identity of the precipitates that were produced. In the balanced equation, put (s) by the precipitate and (aq) by the other product.
2. Identify the TYPES of reactions that you observed.
3. Write the net ionic equations for all of the reactions.
Predict what will happen when the following reactants are combined. If you think there is a reaction, write out the products. If there will be no reaction, write N.R.
|Reactants |Predictions |
|Pb(NO3)2 with KI | |
|CuSO4 with NaOH | |
|CuSO4 with NaCl | |
|AgNO3 with NaCl | |
|AgNO3 with KI | |
|HC2H3O2 with NaHCO3(s) | |
|Na2SO3(s) with HCl | |
|NaHCO3(s) with HCl | |
|zinc metal with CuSO4 | |
|zinc metal with HCl | |
|copper metal with HCl | |
|magnesium metal with HCl | |
|Copper metal with AgNO3 | |
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