Determine Limiting Reagen Experiment
Investigation 3
Determine the Limiting Reagent
Chemistry
Investigation 3 Limiting Reagents
Aim: To determine the limiting reagent in a reaction.
Hypothesis: if the number of moles of the solutions added together equals the stoichiometry ratio in the balanced equation, then we would not expect a limiting reagent in the reaction.
Independent variable: The number of moles of the reactants
Dependent Variable: The limiting reagent
Constant Variable: The volume of reactants added
Equipment: 2 100 ml beaker 2 measuring cylinders 10 ml of 0.1 molL-1 HCL(aq), NAOH(aq) 20 ml of 0.1 molL-1H2SO4(aq), CuSO4(aq) 30 ml of 0.1 molL-1 Ba(NO3)2(aq) Universal indicator Filter Paper Funnel 4 test tubes
Reaction A-
Method: 1) Measure 10 ml of 0.1 molL-1 of Hydrochloric Acid using a measuring cylinder. 2) Measure 10 ml of 0.1 molL-1 of Sodium Hydroxide solution using another measuring cylinder. 3) Pour the 2 solutions into a 100 ml beaker. 4) Mix the solution using a stirring rod. 5) Add 2 drops of the universal indicator into the solution. 6) Observe any changes to the resulting solution. (colour)
Results/Observations:
The solution turns light purple after adding the universal indicator.
Reaction B-
Method: 1) Measure 10 ml of Ba(NO3)2(aq) and H2SO4(aq). 2) Pour the 2 solutions into a 100 ml beaker. 3) Mix using a stirring rod. 4) Prepare a funnel on top of a 100 ml beaker. 5) Cover the top of the funnel with 3 layers of filter paper. 6) Pour the solution into the funnel. 7) Separate the solution obtained in the beaker into 2 test tubes. 8) Add Ba(NO3)2 into one of the test tubes and H2SO4 into the other. 9) Observe and record any changes.
Reaction C-
Method:
Repeat the method used in Reaction B using Ba(NO3)2 and CuSO4 instead.
Results:
Reaction B- Test tube 1 | Ba(NO3)2 added to the solution from beaker | Precipitate formed | Test tube 2 | H2SO4
Determine the Limiting Reagent
Chemistry
Investigation 3 Limiting Reagents
Aim: To determine the limiting reagent in a reaction.
Hypothesis: if the number of moles of the solutions added together equals the stoichiometry ratio in the balanced equation, then we would not expect a limiting reagent in the reaction.
Independent variable: The number of moles of the reactants
Dependent Variable: The limiting reagent
Constant Variable: The volume of reactants added
Equipment: 2 100 ml beaker 2 measuring cylinders 10 ml of 0.1 molL-1 HCL(aq), NAOH(aq) 20 ml of 0.1 molL-1H2SO4(aq), CuSO4(aq) 30 ml of 0.1 molL-1 Ba(NO3)2(aq) Universal indicator Filter Paper Funnel 4 test tubes
Reaction A-
Method: 1) Measure 10 ml of 0.1 molL-1 of Hydrochloric Acid using a measuring cylinder. 2) Measure 10 ml of 0.1 molL-1 of Sodium Hydroxide solution using another measuring cylinder. 3) Pour the 2 solutions into a 100 ml beaker. 4) Mix the solution using a stirring rod. 5) Add 2 drops of the universal indicator into the solution. 6) Observe any changes to the resulting solution. (colour)
Results/Observations:
The solution turns light purple after adding the universal indicator.
Reaction B-
Method: 1) Measure 10 ml of Ba(NO3)2(aq) and H2SO4(aq). 2) Pour the 2 solutions into a 100 ml beaker. 3) Mix using a stirring rod. 4) Prepare a funnel on top of a 100 ml beaker. 5) Cover the top of the funnel with 3 layers of filter paper. 6) Pour the solution into the funnel. 7) Separate the solution obtained in the beaker into 2 test tubes. 8) Add Ba(NO3)2 into one of the test tubes and H2SO4 into the other. 9) Observe and record any changes.
Reaction C-
Method:
Repeat the method used in Reaction B using Ba(NO3)2 and CuSO4 instead.
Results:
Reaction B- Test tube 1 | Ba(NO3)2 added to the solution from beaker | Precipitate formed | Test tube 2 | H2SO4