Equilibrium Lab application
Lab O6 – Equilibrium Lab Application
Purpose: An introduction to the qualitative aspects of chemical equilibrium. Starting with a reaction at equilibrium, one will change the concentration of various ions present in the equilibrium, and record the states of the changing equilibrium through observation.
Theory:
Equilibrium- the point at which a solution has become perfectly saturated; when their forward and reverse reaction rates are equal
Concentration- a measurement of how much solute is dissolved in a solution, measured in molarity (M)
Reversible reaction-represented by a double arrow, a reaction the works in both the forwards and reverse directions
Closed system- an environment in which nothing in the reaction will be able to escape. Must be part of an actual equilibrium expression
Common Ion- when a substance is added to equilibrium and it has one ion in common, it will most likely affect to equilibrium in one way or another as a precipitate may form
Control dish- the initial equilibrium to which all modified solutions will be compared
Equilibrium Shift- when a system in equilibrium is affected by an external stress, the reactants and products shift to minimize the effects of the stress
Stresses- alterations made to a system in regards to concentration, pressure and volume, temperature or the addition of a catalyst
Materials:
1- 150ml beaker
4- 250ml beakers
0.0020M potassium thiocyanate, KSCN, (aq)
10 drops of Fe(NO3)
Crystals of solid KSCN
Crystals of solid Na2HPO4
Safety goggles
Lab book
Sketch of apparatus:
Procedure:
1. In the first table, write down a description of what KSCN and Fe(NO3)3 look like.
2. Clearly mark the 4 beakers, 1 thru 4, to ensure you know what substance is added to each beaker.
3. Observe a solution of potassium nitrate KNO3. Describe the appearance of the solution in the first table.
4. Put approximately 25 ml of 0.0020M potassium thiocyanate solution, KSCN, in
Purpose: An introduction to the qualitative aspects of chemical equilibrium. Starting with a reaction at equilibrium, one will change the concentration of various ions present in the equilibrium, and record the states of the changing equilibrium through observation.
Theory:
Equilibrium- the point at which a solution has become perfectly saturated; when their forward and reverse reaction rates are equal
Concentration- a measurement of how much solute is dissolved in a solution, measured in molarity (M)
Reversible reaction-represented by a double arrow, a reaction the works in both the forwards and reverse directions
Closed system- an environment in which nothing in the reaction will be able to escape. Must be part of an actual equilibrium expression
Common Ion- when a substance is added to equilibrium and it has one ion in common, it will most likely affect to equilibrium in one way or another as a precipitate may form
Control dish- the initial equilibrium to which all modified solutions will be compared
Equilibrium Shift- when a system in equilibrium is affected by an external stress, the reactants and products shift to minimize the effects of the stress
Stresses- alterations made to a system in regards to concentration, pressure and volume, temperature or the addition of a catalyst
Materials:
1- 150ml beaker
4- 250ml beakers
0.0020M potassium thiocyanate, KSCN, (aq)
10 drops of Fe(NO3)
Crystals of solid KSCN
Crystals of solid Na2HPO4
Safety goggles
Lab book
Sketch of apparatus:
Procedure:
1. In the first table, write down a description of what KSCN and Fe(NO3)3 look like.
2. Clearly mark the 4 beakers, 1 thru 4, to ensure you know what substance is added to each beaker.
3. Observe a solution of potassium nitrate KNO3. Describe the appearance of the solution in the first table.
4. Put approximately 25 ml of 0.0020M potassium thiocyanate solution, KSCN, in