Exp 06: Chemical Equations

Your job is to make about a dozen mixtures and determine if a chemical reaction occurs in each mixture. If you observe a reaction you will determine the chemical equation that describes it.

Report your final chemical equation for each: If there is no reaction, show N/R. If there is a reaction, provide the net ionic equation that describes it.

You will use double displacement kinetics and your understanding of precipitation, neutralization, and gas evolution reactions to justify your conclusions.

AB + CD → AD + CB

Exp 06: Chemical Equations

Test #1. Mix 0.1M sodium chloride (NaCl) and 0.1M potassium nitrate (KNO3) solutions.

Test #2. Mix 0.1M sodium chloride (NaCl) and 0.1M silver nitrate (AgNO3) solutions.

Test #3. Mix 1M sodium carbonate (Na2CO3) and 6M hydrochloric acid (HCl) solutions.

Test #4. Mix 3M sodium hydroxide (NaOH) and 6M hydrochloric acid (HCl) solutions.

Test #5. Mix 0.1M barium chloride (BaCl2) and 3M sulfuric acid (H2SO4) solutions.

Test #6. Mix 6M ammonia (NH3) and 3M sulfuric acid (H2SO4) solutions in the hood.

Test #7. Mix 0.1M copper (II) sulfate (CuSO4) and 0.1M zinc nitrate (Zn(NO3)2 solutions.

Test #8. Mix 1.0M sodium carbonate (Na2CO3) and 0.1M calcium chloride (CaCl2) solutions.

Test #9. Mix 0.1M copper(II) sulfate (CuSO4) and 0.1M ammonium chloride (NH4Cl) solutions.

Test #10. Mix 3M sodium hydroxide (NaOH) and 6M nitric acid (HNO3) solutions.

Test #11. Mix 0.1M iron(III) chloride (FeCl3) and 3M sodium hydroxide (NaOH) solutions.

Test #12. Add 1 gram of solid sodium bicarbonate (NaHCO3) to 3 mL of water and shake to dissolve. Then add about 1 mL of 6 M HCl solution, dropwise, using a medicine dropper.

Part A: Test each of the following reactions, record your observations and determine the chemical equation that describes any observed reaction.

Exp 06: Chemical Equations

In the hood you will find dilute solutions of 0.1 M NH4Cl, 0.1 M CuSO4, 3 M NaOH and 6 M HCl.

Test #13. Predict which two of these solutions would produce a precipitate if you mixed them. Test your prediction by combining about 1 mL of each of the two solutions in a test tube. Record the results of your test or tests.

Test #14: Predict which two of these solutions you could mix to produce a gas. Mix the two chosen solutions in a test tube and place a wet piece of red litmus paper at the top of the test tube. If ammonia gas is formed, it will reach the wet litmus paper and turn it blue (ammonia is a weak base). Record your test or tests.

Part B: Design and test a reaction to meet each of the criteria of test #13 and #14, using the solutions provided.

Exp 06: Chemical Equations

Calculations: Use the calculation guide from the experiment description to guide you in determining the chemical equation for each reaction.

Calculations Guide for Experiment:Double Displacement Rxns

Example Test: Mix 0.1M sodium chloride [NaCl] and 0.1M lead nitrate [Pb(NO3)2] solutions.

Balanced Complete Ionic Equation: 2 Na+(aq) + 2 Cl-(aq) + Pb2+ (aq) + 2 NO3- (aq) ➞ 2 Na+(aq) + PbCl2 (s) ↓ + 2 NO3- (aq)

(break all electrolytes into dissociated ions in solution)

Net Ionic Equation: 2 Cl-(aq) + Pb2+ (aq) ➞ PbCl2 (s) ↓

(remove all spectator ions from the ionic equation;if nothing is left write “N/R” for no reaction)

Test #1. Mix 0.1M sodium chloride (NaCl) and 0.1M potassium nitrate (KNO3) solutions.

Test #2. Mix 0.1M sodium chloride (NaCl) and 0.1M silver nitrate (AgNO3) solutions.

Test #3. Mix 1M sodium carbonate (Na2CO3) and 6M hydrochloric acid (HCl) solutions.

Observations:

Upon mixing, a bright yellow solid appeared.

Complete Ionic:

Net Ionic:

Molecular:

Obs:

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Balanced Molecular Equation: 2 NaCl (aq) + Pb(NO3)2 (aq) ➞ 2 NaNO3 (aq) + PbCl2 (s) ↓

(predict the possible products by identifying the AB + CD ➞ AD + CB pattern; look for any non-electrolyte products)

Complete Ionic:

Net Ionic:

Molecular:

Obs:

Complete Ionic:

Net Ionic:

Molecular:

Obs:

You do not need to balance these equations, but

show the state of each reactant and product!

Questions?