Double Displacement Reactions

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  1. Title:

Double Displacement Reactions

  1. Purpose:

To gain a better understanding of the typical reaction of the addition of two binary compounds, and how the reaction of those two compounds can be predicted.

  1. Variables:

➔Dependent Variable:

Reagents given, hence the solutions we make from these reagents, and the standard solubility rules.

➔Controlled Variables:

        The two reagents which we will react together at each trial.

➔Independent Variable:

Whether the reagents will create a precipitate or not, which depends on the reagents combined.

  1. Hypothesis:

If the compound is containing mettle and is added to a compound that is also containing mettle. The two mettles will change places and then something in the equation will precipitate out of the solution. The majority of the elements will not precipitate and none will have a whole solution of precipitant. All will have some form of ion solution that we are left over from the chemical reaction.

  1. Materials:
  • Compounds
  • AgNO3
  • BaCl2
  • Na2CO3
  • K3PO4
  • KBr
  • Zn(NO3)2
  • K2CrO4
  • Fe2Cl3
  • NaOH
  • MgCl2
  • NaCl2
  • NaC2H3O2
  • (NH4)2SO4
  • Al(NO3)3
  • Pb(NO3)2
  • Cu(NO3)2
  • Ca(NO3)2
  • Equipment
  • Distilled Water
  • Dropper
  • 16 - 10 ml flasks
  • 10 ml graduated cylinder
  • Solubility chart
  • Balance
  • Transparency
  • Marking pen
  • Masking tape
  • Stirring rod

  1. Procedure:
  1. Prepare 1 molar solutions of given reagents:
  1. Calculate amounts to combine of given reagents. Complete the following for all 16 reagents:
  1. As you need 5 ml of solution, begin with this amount
  2. Multiply by the molar amount which you wish to use for the reactions.
  3. Multiply by the molecular mass of the given compound.
  4. This will give you the amount, in grams, of the molecule for which you are calculating.
  1. Create 1 molar reagents. Complete the following for each reagent:
  1. Mark 16 - 10 ml flasks with masking tape showing the content, showing each of the 16 reagents – one for each flask.
  2. Measure out the amount, which you calculated in the Part a, of the reagent.
  3. Place this mass of the reagent into the flask which is marked with the reagent.
  4. Measure out 5 ml of distilled water in the 10 ml graduated cylinder, and place this water in the flask with the reagent.
  5. Stir the reagent so as to combine it completely.
  1. Combine given reagents.
  1. Grid a transparency so that each reagent has a chance to react with every other reagent. Also make a data chart to write in the data which you will collect.
  2. Complete the following for each solution:
  3. Take one to two drops of the solution and place it in all the boxes which are marked on your grid transparency.
  4. After all solutions have been combined, write in your data chart whether a precipitant has formed, and if so, describe the precipitant; describe the composition of the solution.
  1. Evaluate results:
  1. Write the balanced equations for each of the reactions which occurred in this experiment.
  2. Use solubility rules to determine if a precipitant has formed in each reaction.

  1. Data Collection:

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  1. Data Prossing and Presentation:

A. Stoichiometry Calculations Regarding Molarity

  1. AgNO3

.0102 H20 × 1mol/1L × 169.9 g/ 1 mol = 1.1699 g AgNO3

  1. BaCl2

.0102 H20 × 1mol/1L × 208.736 g/ 1 mol = 2.08736 g BaCl2

3.  Na2CO3

.0102 H20 × 1mol/1L × 105.988g/ 1 mol = 1.05988 g Na2C03

  1. K3PO4

.0102 H20 × 1mol/1L × 195.995 g/ 1 mol = 1.95995 g K3PO4

  1. KBr

.0102 H20 × 1mol/1L × 119.002 g/ 1 mol = 1.19002 g KBr

  1. Zn (NO3)2 ...

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