Experiment_606_Double Displacement Reactions_1_2_3
- Page ID
- 303068
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Student Name |
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Laboratory Date: Date Report Submitted: |
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Student ID |
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Experiment Number and Title |
Experiment 606: Double Displacement Reactions
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Experiment 606: Double Displacement Reactions
Section 1: Purpose and Summary
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Carry out double displacement reactions involving different aqueous solutions.
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Identify reactions that form precipitates, evolve gases, and increase temperature after mixing.
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Predict whether a double displacement reaction will occur between two solutions.
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Write molecular, complete ionic, and net ionic equations.
In this experiment, students will combine two aqueous solutions and determine whether a reaction occurs. Based on solubility rules, students will predict whether a double displacement reaction will occur from a given set of aqueous solutions. The students will then carry out the reaction to confirm their prediction.
Section 2: Safety Precautions and Waste Disposal
Safety Precautions:
Use of eye protection is recommended for all experimental procedures.
Waste Disposal:
While you are doing the experiment, collect your reaction mixtures into a waste beaker.
When you are finished with the experiment, pour the contents of the waste beaker (liquid waste only) into the inorganic waste container in the fume hood. Rinse water from the beaker does not need to be captured, just the bulk material.
Section 3: Procedure
Each reaction in this experiment involves mixing two aqueous solutions in a test tube. Clean, rinse with laboratory water, and dry fourteen (14) test tubes. Label each test tube with the reaction mixture. Set on a test tube rack.
To determine whether a reaction occurs or not, observe any bubble formation (gas evolution) in the solution, formation of a solid (precipitate), or increase in temperature of the reaction mixture. Bubble formation is due to the formation of a gaseous product. If the solution becomes cloudy, this is evidence for the formation of fine, suspended solid particles of the precipitate.
Part 1: Observing double displacement reactions
Obtain about 1 mL (approximately 20 drops) each of the indicated solutions in a test tube. Record your observations. Write the molecular, complete ionic, and net ionic equations for the reaction. If no observable change is noted, write ‘no reaction’ on the reactant side of the equation; no need to write the complete ionic and net ionic equations.
Do one reaction at a time to avoid mixing up of solutions. It is important not to mix up droppers (if used) to avoid contamination of reagents. This may also lead to ‘false positive’ observations.
NOTE: All solutions are at a concentration of 0.1 Molar (moles per liter) unless otherwise indicated*.
Observations:
Molecular equation:
Complete ionic equation:
Net ionic equation:
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Observations:
Molecular equation:
Complete ionic equation:
Net ionic equation:
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Observations:
Molecular equation:
Complete ionic equation:
Net ionic equation:
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NOTE: Add one drop of phenolphthalein indicator separately to the sodium hydroxide and hydrochloric acid before mixing. Mix in a specific sequence.
4.1. Transfer ½ of the sodium hydroxide to the hydrochloric acid. (Excess hydrochloric acid) 4.2. Transfer the rest of the sodium hydroxide to the hydrochloric acid. (Equal amounts) 4.3. Add an additional 1-2 mL of sodium hydroxide to the hydrochloric acid. (Excess sodium hydroxide)
Observations:
Molecular equation:
Complete ionic equation:
Net ionic equation:
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Observations:
Molecular equation:
Complete ionic equation:
Net ionic equation:
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Observations:
Molecular equation:
Complete ionic equation:
Net ionic equation:
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Observations:
Molecular equation:
Complete ionic equation:
Net ionic equation:
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Observations:
Molecular equation:
Complete ionic equation:
Net ionic equation:
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Observations:
Molecular equation:
Complete ionic equation:
Net ionic equation:
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NOTE: Add one drop of phenolphthalein indicator separately to the sodium hydroxide and nitric acid before mixing. Mix in a specific sequence.
10.1. Transfer ½ of the sodium hydroxide to the nitric acid. (Excess nitric acid) 10.2. Transfer the rest of the sodium hydroxide to the nitric acid. (Equal amounts) 10.3. Add an additional 1-2 ml of sodium hydroxide to the nitric acid. (Excess sodium hydroxide)
Observations:
Molecular equation:
Complete ionic equation:
Net ionic equation:
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Observations:
Molecular equation:
Complete ionic equation:
Net ionic equation:
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Observations:
Molecular equation:
Complete ionic equation:
Net ionic equation:
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Part 2: Predicting double displacement reactions
SOLUBILITY RULES for IONIC COMPOUNDS
1. Group 1 metal compounds (also called alkali metal compounds), acetates, nitrates, and ammonium compounds are all soluble.
2. Hydroxides of alkali metals and NH4+1, Ca+2, Sr+2, and Ba+2 are soluble. All others are insoluble.
3. All halides (chlorides etc.) are soluble except for those containing Ag+1, Pb+2, and Hg2+2.
4. Most sulfates are soluble, except for BaSO4, SrSO4, Ag2SO4, PbSO4, and CaSO4.
5. Most phosphates, carbonates, chromates and sulfides are insoluble (except those of the Group 1
metals and ammonium ion).
6. In addition, all acids (compounds that form an ionized H+, HCl, H2SO4, HI, etc.) are soluble!
You have the following solutions available in the lab: NH4Cl, NaOH, HCl, and CuSO4.
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3. Compounds tested:
Observations:
Net ionic equation:
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Compounds tested:
Observations:
Net ionic equation:
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Notes: