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GCSE DOUBLE AWARD SCIENCE INVESTIGATION

Title: Investigating how concentration changes the rate of a chemical reaction |

Name: Ryan Bradley |

Class: 12A1 |

What is the aim of this experiment?

To investigate how concentration hydrochloric acid affects the rate of reaction between sodium thiosulphate and hydrochloric acid and water.

P.6a: List all the factors that could have an effect on the results in this investigation?

* Concentration * Temperature * Surface area * Catalyst * Colour of the X * Stirring the mixture * Water in the beaker from washing out beaker

P.6a: P.8a: Explain in detail how each of the factors you named could affect the investigation?

Surface Area: This would affect my investigation because if there was a bigger surface area this means the particles have more room to collide as they are more exposed to head on collisions

Concentration: If I was to increase the concentrations of the hydrochloric acid by too much/ little this will make my results unreliable because the more hydrochloric acid the more successful collisions and this would increase the rate of reaction.

Stirring the mixture: This would affect my investigation because if I was to stir the mixture it would speed up the reaction time as you are creating more collisions meaning the ‘x’ will disappear quicker.

Temperature: If I was to increase the temperature this would affect my investigation because it would mean the particles would gain more energy and this would mean they would collide with a greater force and this would make the rate of reaction faster which would turn the mixture opaque more quickly.

Catalyst: If I was to add to much of the catalyst this would increase the rate of reaction a lot faster and this may affect my investigation and my results would then be unreliable

Colour of the X: This may affect my investigation because if I was change the colour of the ‘x’ on the piece of paper this will leave my results very inaccurate because if I used a lighter coloured ‘x’ it would disappear quicker and if I was to use a darker coloured ‘x’ it would take longer for it to disappear

Water in the beaker from washing out beaker: This may affect my investigation because there may be water in the bottom of my beaker and this may dilute the reactants meaning this will increase their reaction time.

P.6a: Name the factor you intend to vary.
The factor I intend to vary is the concentration of Hydrochloric acid.

P.6b: Explain how you will vary this factor and give the range of values you intend to use.
I will vary the concentration on HCl by obtaining hydrochloric acid from my science teacher and measure out different concentrations of HCl, I used 5cm3 of water each time to dilute the solution for each concentration E.g. 1) 20cm3HCl 5cm3 H20 2) 15cm3 HCl 10cm3 H20

P.6a: What are you going to measure in the experiment?
In this experiment I am going to measure the length of time it takes for the ‘x’ to disappear.

P.6a: Explain how you are going to take the measurement?
I am going to take this measurement by using a digital stop clock so I will be able to time how long it will take for the solution to go opaque and for the ‘x’ to disappear. I will start my clock when I added the concentrations together and they are all in the one beaker, I will then look over the reaction and when the ‘x’ is no longer visible I will stop the stop clock.

P.6b: How many measurements will you take in the experiment?

I am going to make five different concentrations of hydrochloric acid starting with 5cm3 and working my way to 25cm3 increasing the concentration by 5cm3 each time. I will then repeat my investigation 2 times so I can get fairly accurate results.

Prediction

P.6b: State what you think will happen when you change the independent variable?

When I change the independent variable I believe that the reaction time for the solution of hydrochloric acid and thiosulphate solution will be a lot quicker as there will be more molecules when would mean there will be more collisions. I think that when you double the concentration of hydrochloric acid the time taken for the ‘x’ to disappear will also be twice as fast because there will be more successful head on collisions.

P.6b: Explain in detail your prediction?

There are many possible collisions in my experiment and here are a few:

* Hydrogen ions with thiosulphate ions * Hydrogen ions with water molecules * Water molecules with thiosulphate ions * Chlorine ions and thiosulphate ions * Sodium ions with chlorine ions * Chlorine ions with hydrogen ions

The reaction I am looking at is between hydrochloric acid and sodium thiosulphate.
It is a collision between hydrogen ions from the hydrochloric acid and thiosulphate ions from the sodium thiosulphate that can result in a reaction. When these two ions collide with each other head on and fast the reaction will take place for my experiment. I predict that when the hydrochloric acid is more concentrated the ‘x’ on the sheet will disappear quicker as there are hydrogen ions per unit volume to collide with the thiosulphate ions, more collisions between these two mean more successful collisions and a faster reaction and for a reaction to be successful if the hydrogen ions and thiosulphate ions collide fast, head on with sufficient energy.
P.8a: How can you make sure your measurements are as accurate and reliable as possible?

I will make my measurements accurate and reliable as possible by keeping all the factors the same and using the same equipment so it will be the same throughout. I will also measure each volume of solution by using a measuring cylinder and by getting eye level to measure the volume by using the meniscus.

Results template

P.8b: Use the space below to show how you intend to record your results:

Template table: Volume Na2S2O3 (cm3) | Volume HCL (cm3) | Volume H2O (cm3) | Time 1 (sec) | Time 2 (sec) | Average Time (sec) | 25 | 5 | 20 | | | | 25 | 10 | 15 | | | | 25 | 15 | 10 | | | | 25 | 20 | 5 | | | | 25 | 25 | 0 | | | |

Results table: Volume Na2S2O3 (cm3) | Volume HCL (cm3) | Volume H2O (cm3) | Time 1 (sec) | Time 2 (sec) | Average Time (sec) | 25 | 5 | 20 | 30.27 | 28.78 | 29.52 | 25 | 10 | 15 | 18.87 | 19.32 | 19.09 | 25 | 15 | 10 | 17.87 | 16.98 | 17.42 | 25 | 20 | 5 | 12.68 | 13.28 | 12.98 | 25 | 25 | 0 | 11.50 | 10.28 | 10.94 |

Strategy for dealing with results
P.8b: Will you do anything further with your results when they have been recorded – use the space below to show what you intend.

Rate of reaction
(s-1)

Volume of HCl (cm3)

I am going to use my results to create a line graph to show the relationship of direct proportion between the volume of hydrochloric acid and the rate of reaction. I am expecting to find my results as shown and I will then include a line of best fit.

1. Calculate the average time for each concentration by adding the two times and then dividing by 2 1. Calculate the rate of reaction- rate= 1/average time 2. Plot a graph showing the rate v’s concentration

VolumeHCl(Cm3) | AverageTime(Sec) | RateX100(s-1) | Rate (2dp) X100(s-1) | 5 | 29.52 | 3.387534 | 3.39 | 10 | 19.09 | 5.238345 | 5.24 | 15 | 17.42 | 5.740528 | 5.74 | 20 | 12.98 | 7.70416 | 7.70 | 25 | 10.94 | 9.140768 | 9.14 |

Use of suitable equipment

P.4b: List the apparatus you will need to carry out your investigation.

Conical flasks

2 measuring cylinders

2 pippets

Stop clock

Safety goggles

2 beakers

P.2a, P.6a: Draw a diagram to show how you will set up the apparatus.

P.2a, P.6a: Write a step by step method describing how you will carry out your investigation. * First get all the equipment needed for the experiment * Label the beakers and draw and ‘x’ on a piece of paper, this is the marker which helps tell you when the mixture is opaque * Draw out a table for your results showing how much Na2S2O3, HCl and H2O added and how long it take for the ‘x’ to disappear * Put on safety goggles and start experiment * Measure 25cm3 of 0.5 molar Na2S2O3 into a measuring cylinder and get down to eye level to read the bottom of the meniscus and to make the measurement is accurate * Pour this into the conical flask. * place the flask over the piece of paper with the x on it * Then measure 20cm3 of H2O and 5cm3 of 0.5 molar HCl into the other measuring cylinder and add this to the conical flask. * When the HCl and H2O mixture is added, start the stop clock and time how long it takes for the x to disappear. Record your times to 1/100 of a second * Repeat this experiment with the same measurements of chemicals and compare the two times * Clean out your equipment and start again using the same amount and volume of Na2S2O3 throughout the experiment but change the volume of H2O and HCl every time for example for the second experiment have 25cm3 of Na2S2O3 and have 15cm3 of H2O and 10cm3 of HCl and keep reducing the amount of H2O by 5cm3 but increase the amount of HCl by 5cm3 and every time you do an experiment repeat it twice

List any safety precautions you should take. * Wear eye protection * Stand up when doing the experiment * Do not have anything in the way of the experiment

Skill Area O: Obtaining evidence.

* Use your equipment safely to make measurements as accurately as possible. * Make sure you have enough results (at least 5 sets). * Record your results clearly and accurately in the space below. * Consider whether you should repeat any of your measurements.

O.2a | | O.4a | | O.4b | | O.6a | | O.6b | | O.8a | |
Skill Area I: Interpreting and evaluating.
Presentation of results

I.4a, I.6a: How have you presented your results?

I have recorded my results in a table and have included the average time in my table for the two reaction times of each concentration. I have presented my results on a line graph which shows the line of best fit to show the relationship of direct proportion.

Identification of trends and patterns

I.4b: Describe any patterns you can see in your results.

From my results I can see that when I increased the amount of hydrochloric acid the rate of the reaction also increased. This shows on my graph that there is a relationship of direct proportion between the two measurements because as I doubled the concentration of hydrochloric acid the reaction time also increased. I can see from my graph that although my line of best fir does not go directly through my origin it still shows a relationship of direct proportion. Rom my graph and results I can see that there is a strong positive correlation between the rate of reaction and the concentration of hydrochloric acid, from my table I have highlighted my two closest results and were very similar.

Conclusion

I.2a, I.6b: What can you conclude from these results?

From my results I have concluded that when the amount of HCl was increased the rate of reaction was faster and I know this because I have recorded my results which show that when more hydrogen ions were present there was a greater reaction time which meant the time taken for the ‘x’ to disappear was faster. My results also show me there is a relationship of direct proportion between the concentration of hydrochloric acid and the rate of reaction as my graph shows a distinct relationship between the two factors. From my line of best fit I can make out that two of my results did not fit the overall pattern as one of the factors may have affected my investigation. From my investigation I can conclude that there was a relationship on the concentration of hydrochloric acid and the rate of reaction as the majority of my results are on my line of best fir or close to it showing the reliability of my investigation.

I.8b: Does what you have found out agree with the prediction you made?

From what I have found out it does agree with my prediction because when I increased the concentration of hydrochloric acid the faster the reaction time which means that there was more hydrogen ions to collide successfully. When I added 5cm3 of hydrochloric acid the amount of water molecules decreased leaving more of a chance for the collision between the thiosulphate ions and hydrogen ions which would of increased in my results in which it did therefore my prediction I made was correct and I agree that my prediction was correct.

I.6b: Can you explain why you got these results (why this happened)?

I feel that I got these results because I know that when the concentration of HCl increased it means that there was more chance of collision with the Na2S2O3 ions as the H20 ions do not have a big enough density to collide with the thiosulphate ions. I can also explain why this happened because I know that for a successful collision to happen there needs to be a sufficient amount of energy between the hydrogen ions and the thiosulphate ions.

I.6c: Do you think your method was the best way of carrying out this investigation or could it be improved in order to obtain more accurate and reliable results?

I feel that I had made a good reliable attempt at my investigation and I feel it was the best way but it there is room for improvement as I could have recorded the test more than two times, I could of photocopied the paper with the ‘x’ on it and laminate it (so it won’t get damp) to ensure that the ‘x’ was the same throughout my investigation. I could have also changed the molar of the concentration to get more accurate results, I could have also made sure my flask was dry by using a towel to dry it and not to use a heater as this would affect the temperature of the beaker and this factor could affect my investigation. To make sure that my results were reliable I could have repeated the experiment more often for each concentration.

I.8c: Are there any results that do not seem to fit the overall pattern? If so, try to explain why you got these results.

For 10cm3 of hydrochloric acid on my average graph I got 5.24s-1 which was 0.4s-1 of my line of best fit, I may have got these results because I may not haveadded enough concentration of hydrochloric acid as this may affected my results as they may have been more hydrogen ions in the solution. For 15cm3 of hydrochloric acid on my average graph I got 5.74s-1 which was about 0.4s-1 of my line of best fit, I may have got this result because I may not have added to much concentration of hydrochloric acid. For both these results I may not have cleaned out my beaker correctly and there could have been water molecules in the bottom of it meaning it may have diluted the solution. I.8c: How reliable do you think your results are overall, do you think they are good enough to convince someone else that there is a particular relationship between these 2 factors?

I feel that my results are reliable enough for a school experiment, to convince someone that there is a relationship of direct proportion between the concentrations of Na2S2O32-and HCl solutions as my results are fairly accurate and I have completed the investigation under a fair test making sure I had kept all the independent variables the same throughout my test. My line of best fir did not go through the origin but most of my point lie close to my line of best fit showing me that they are accurate. Although some of my points were not on my line of best fit for example, 10cm3 of hydrochloric acid is not on my line of best fit but close to it, 3 other results are on my line of best fit which shows me that there is still some relationship of direct proportion and I think they are accurate and reliable enough to convince someone that there is a relationship between the concentration of hydrochloric acid and the rate of reaction.

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