Prediction
I predict that adding copper sulphate to catalase will slow down the rate at which hydrogen peroxide is broken down into water and oxygen. There will therefore be more oxygen produced when copper sulphate is not present. I believe this because copper sulphate will act as a non-competitive inhibiter in the reaction.
I predict that the reaction will not continue when the concentration of hydrogen peroxide is increased at the end of the experiment. This is because copper sulphate contains the heavy metal ion Cu2+. Heavy metal ions act as irreversible inhibitors (as stated in the ‘Scientific Knowledge’ above).
Aim
To find out the effect copper sulphate has on the activity of catalase.
Apparatus
- Stand and clamp
- Side arm flask
- Basin
- Water
- Stop clock
- Burette
- 5 x beaker
- 3 x 20ml syringe
- Knife
- Ruler
- Ceramic tile
- OHP pen
- Chipping machine
Reagents
- 60ml 0.5 mol copper sulphate solution
- 60ml water
Method
Begin by gathering all apparatus together, as listed on the previous page. Set up the equipment as shown in the diagram below. Fill the basin and the burette with water. Turn the burette to vertical with the opening submerged in the water contained in the basin. Clamp the measuring cylinder in this position. Position the side arm flask so that the end of the arm is directly beneath the opening of the measuring cylinder.
Use the chipping machine to produce potato chips. Cut the chips into 1cm3 pieces using the knife, ruler and ceramic tile. Place 5 potato cubes in the side arm flask. With a syringe put 20ml copper sulphate into a beaker, and using a different syringe, add 20ml of hydrogen peroxide to the copper sulphate. Pour the contents of the beaker into the side arm flask, and start the stop clock at the same time. Place a stopper in the top of the flask to prevent oxygen escaping. Measure the level of oxygen in the burette straight after putting in the stopper. The action of pushing the stopper down into the top of the flask will displace air in the flask and air will be forced through the side arm and up the burette. This air displaced by the stopper must not be measured as oxygen produced by the reaction. Record the volume of oxygen produced every 20 seconds for the following 3 minutes. Carry out two replications of this test. Repeat this process five more times but each time add a different concentration of 20ml of copper sulphate solution to the 20ml of hydrogen peroxide. The five other concentrations are: 0.4mol, 0.3mol, 0.2mol, 0.1mol, and 0mol. The diagram below shows the preparation of the six different copper sulphate solution concentrations. Use different syringes to measure the various liquids.
- The first contains 20ml of 0.5 mol copper sulphate solution.
- The second contains 16ml of copper sulphate solution and 4ml of water to create a solution with a copper sulphate concentration that is 80% of the first or a 0.4mol copper sulphate concentration.
- The third contains 12ml of copper sulphate solution and 8ml of water to create a solution with a copper sulphate concentration that is 60% of the first or a 0.3mol copper sulphate concentration.
- The fourth contains 8ml of copper sulphate solution and 12ml of water to create a solution with a copper sulphate concentration that is 40% of the first or a 0.2mol copper sulphate concentration.
- The fifth contains 4ml of copper sulphate solution and 16ml of water to create a solution with a copper sulphate concentration that is 20% of the first or a 0.1mol copper sulphate concentration.
- The fifth contains 0ml of copper sulphate solution and 20ml of water to create a solution with a copper sulphate concentration that is 0% of the first or a 0mol copper sulphate concentration.
Lastly, to test whether or not copper sulphate acts as a reversible inhibitor, add five 1cm3 pieces of potato, 20ml of hydrogen peroxide and 20ml of 0.5mol copper sulphate solution to the flask. Leave the reactants together until no more oxygen is being produced. Then add a further 20ml of hydrogen peroxide and see if any more oxygen is produced. Repeat this process twice. If no oxygen is produced after hydrogen peroxide is added for the second time then copper sulphate must be an irreversible inhibitor.
It is important to use a burette as it will measure to the nearest mm3 how much oxygen is produced. This is more accurate than just counting the number of oxygen bubbles produced. Bubbles may vary in size and it would be easy to make an error counting the bubbles (particularly at the beginning of the reaction when the rate at which bubbles are produced is highest) than reading off the volume of oxygen in the burette. Using a stop clock will help to ensure a fair accurate test as time can be recorded accurately to the nearest 1/100 second. As stated in the ‘Scientific Knowledge’ temperature, pH and enzyme and substrate concentration have an effect of the rate of reaction. To ensure a fair test these factors will be kept constant. The only variable will be the concentration of inhibitor (copper sulphate solution). To keep the substrate concentration constant, and accurately vary the concentration of the inhibitor the two substances will be measured using syringes. Measuring amounts of liquids is done more accurately with syringes than with measuring cylinders as long as care is taken not to create air bubbles in the syringe. Air bubbles could cause the liquid in the syringe to appear to have a larger volume than it really does. This could lead to an incorrect amount of liquid being measured and create anomalous results. To keep the amount of enzyme constant a potato chipper will be used to cut the potato chips into chips of the same size. It is important to use the same potato for all the chips as the amount of catalase in different potatoes may vary.
Safety
Hydrogen peroxide is poisonous so great care should be taken when handling it.
- Those handling the substance should wear rubber gloves and wash their hands thoroughly afterwards to prevent poisoning themselves or others.
- Safety spectacles to prevent any risk of an eye injury.
- Work with the liquids whilst standing up. Never sit down. Standing up enables one to move quickly if there is a spillage.
- When the experiment has been completed always thoroughly wash the equipment used. Wipe down benches so that they are clean surfaces.
Table 1. A table to show the values (in cm3) read from the burette
Table 2. A table to show the amount of oxygen produced when a further 20ml of hydrogen peroxide was added to the inactive reaction
Table 3. A table to show the values (in cm3) read from the burette collected from a separate investigation
Table 4. A table to show the mean amount of oxygen produced (in cm3, to 2 d.p.) from a separate investigation
Key for graphs
0.0mol copper sulphate concentration
0.2mol copper sulphate concentration
0.4mol copper sulphate concentration
0.6mol copper sulphate concentration
0.8mol copper sulphate concentration
1.0mol copper sulphate concentration
Graph 1. A graph to show the mean amount of oxygen produced for copper sulphate concentrations (ranging from 0mols to 1mols) over time
Graph 2. A graph to show the mean amount of oxygen produced for copper sulphate concentrations (ranging from 0.2mols to 1mols) over time
Graph 3. A graph to show the mean amount of oxygen produced, when the copper sulphate solution concentration was zero, over time. This graph is included as an example of how the initial rate of reaction was calculated by working out the gradient of the line at 30 seconds.
23.4/50=0.468 cm3/sec
0.468*60=28.08cm3/min
Graph 4. A graph to show the estimated rate of reaction against the concentration of copper sulphate solution (for concentrations ranging from 0mols to 1mols)
Graph 5. A graph to show the estimated rate of reaction against the concentration of copper sulphate solution (for concentrations ranging from 0.2mols to 1mols)
Analysis
Graph 1 clearly shows that more oxygen is produced when copper sulphate is absent from the reaction. Within one minute there was, on average, 23.5cm3 of oxygen produced when there was no copper sulphate. But when a copper sulphate solution, with a concentration of only 0.2mols, was present in the reaction, on average only 1.27cm3 of oxygen were produced in one minute. This is a difference of 22.23cm3 of oxygen.
Graph 1 shows that not only does the presence of copper sulphate creates a large drop in oxygen production, but an increase in its concentration further lowers the amount of oxygen produced. This is shown more clearly on Graph 2 were the scale is larger. Progressively less oxygen is produced and at slower rates, as the copper sulphate solution concentration becomes greater. This is true for all but one of the concentrations. For the copper sulphate concentration of 0.4mols the average amount of oxygen produced between 10 and 20 seconds was extraordinarily high; on average 0.6cm3 of oxygen was produced in those 10 seconds. The reason the average amount of oxygen produced was relatively high is due to one anomalous result. This anomaly occurred when the copper sulphate concentration was 0.4mols in test repeat 2. Between 10 and 20 seconds the reading on the burette dropped from 49.0cm3 to 47.7cm3.
Graph 4 shows that the rate of reaction between hydrogen peroxide and catalase is dramatically decreased by the addition of copper sulphate. The rate of reaction drops from 28.08cm3 of oxygen produced per minute to 2.01cm3 of oxygen produced per minute as the concentration of copper sulphate solution is increased from 0mols to 0.2mols. The rate of reaction gradually decreases as the concentration of copper sulphate is increased. This decrease in rate of reaction is shown more clearly in Graph 5 where the scale is larger. When the copper sulphate concentration was 0.2mols the rate of reaction was 1.8cm3 of oxygen produced every minute, when the copper sulphate concentration was 0.6mols the rate of reaction was 1.32cm3 of oxygen produced every minute and when the copper sulphate concentration was 1.0mols the rate of reaction was just 1.03cm3 of oxygen produced every minute. The decrease in reaction rate was not rapid as the copper sulphate concentration was stepped up from 0.2mols through to 1.0mols but a significant drop can clearly be seen. The same anomaly as mentioned in the previous paragraph is responsible here for an increase of the rate of reaction when the copper sulphate concentration is increased form 0.2mols to 0.4mols. As it is an obvious anomaly it is disregarded and not taken into account by the curve of best fit.
Conclusion
As has been shown in the ‘Analysis’ when copper sulphate concentration is increased the rate at which catalase breaks down hydrogen peroxide into oxygen and water is decreased. Therefore the ‘Prediction’ is correct. The reason for this has been explored in the ‘Scientific Knowledge’. Copper sulphate acts as a non-competitive inhibitor to catalase. What happens is that the Cu2+ ions in copper sulphate combine with the catalase molecule with the allosteric site on the catalase molecule. This alters the structure of the catalase molecule. This has an effect on the shape of the active site so that the hydrogen peroxide molecules are unable to bind to the catalase molecule. The result is that hydrogen peroxide is not broken down into oxygen and water, the rate of reaction is reduced. This is shown in Figure 4 where the enzyme is catalase, the substate is hydrogen peroxide and the non-competitive inhibitor is copper sulphate. Copper sulphate must act as a non-competitive inhibitor to catalase because, as stated in the ‘Scientific Knowledge’ non-competitive inhibitors will always reduce the rate of reaction even if substrate concentration is high. The rate of reaction was reduced even though concentration of the hydrogen peroxide (the substrate) was high.
The investigation also shows that copper sulphate acts as an irreversible inhibitor to catalase. On the three occasions that a further 20ml of hydrogen peroxide was added to the reactants after reaction had stopped, no more oxygen was produced. As stated in the ‘Scientific Knowledge’ irreversible inhibitors bind permanently to the enzyme’s allosteric site so that the active site is permanently altered in structure and therefore will not function.
Evaluation
The experimental procedures used worked well in that they have produced results that clearly show the prediction to be correct. Since good curves of best fit were produced, the data appears reliable. Equipment used in the investigation helped to produce reliable evidence. For example syringes, to make the measurements of liquids more accurate, a stop clock to accurately measure time to the nearest 1/100 of a second and a burette to measure the oxygen produced to the nearest mm3.
But the procedures used did create an anomalous result, as identified in the ‘Analysis’. Reasons for this sudden increase in oxygen production are most likely due to a combination of the following reasons: the temperature within the room may have increased causing the enzyme and substrate molecules to vibrate more rapidly so that the substrate entered the active sites more often and with more energy making it easier for the bonds to be broken leading to an increase in rate of reaction; when the potato chips were cut into cubes the cuts made with the knife may not have created flat faces on the cube causing it to be larger than 1cm3 leading to an increase in the amount of enzyme present in the reaction so more active sites would have been available for the substrate to slot into and more oxygen will have been produced; the measurement on the burette may have been recorded too late giving more time for oxygen to have been produced; the table on which the experiment was being carried out on may have been knocked causing the contents of the flask to shake leading to more collisions between enzyme and substrate molecules so that more substrate molecules enter the active sites and with a greater amount of energy making it easier for the bonds to be broken leading to more oxygen being produced; the concentration of copper sulphate may been lower than 0.4mols. The less inhibitor present, the less active sites are distorted and the more oxygen is produced; the hydrogen peroxide concentration may have been greater than was intended. The more substrate molecules there are around, the more often a catalase active sites can bind with one leading to an increase in the rate at which hydrogen peroxide was broken down into oxygen.
One way that the experiment could be improved would be to carry it out in a room in which the temperature was always constant. This would prevent the rate of reaction being increased if the room temperature did the same or decrease if the temperature fell. Temperature variation was not great enough in the experiment to have a significant enough effect on the results to alter the final conclusions drawn. Room temperature would only have varied by plus or minus 2°C. This would only have changed the rate of reaction enough to have varied the burette reading by plus or minus 0.5mm3.
Other sources of error were caused by human inaccuracies. For instance inaccurate measuring of potato chip size, time and of the various liquids used will have had some effect on the validity of the results. Human error would only have been responsible for a the size of a potato cube being out by approximately plus or minus 2mm3, the timing could only have been inaccurate by plus or minus 1 second and the measurements made of liquids could only have been incorrect by about plus or minus 1ml. These inaccuracies are only large enough to have altered the results by plus or minus 1mm3 and will therefore not have had a large enough effect to change the conclusions made.
To help eliminate the effect of human error on the results the tests could be repeated for more than three times. Using the results from a larger number of repeat tests to calculate averages would minimize the effect of mistakes such as inaccurate timing and measuring.
To provide additional evidence to support the conclusion the experiment could be repeated with a larger variation in inhibitor concentration. In particular using concentrations of copper sulphate solution lower than 0.2mols to lessen the large gap between the amount of oxygen produced when copper sulphate is and is not present. As well as using lower substrate concentrations the substrate and enzyme concentrations could be increased. This would lead to a greater production of oxygen and make the volume measurements more accurate.