• Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month

How much concentration of sodium thiosulphate (Na2S2O3) affects the rate of reaction when tested with Hydrochloric acid (HCL).

Extracts from this document...

Introduction

Background Information Chemical reactions happen at widely different rates. The weathering of buildings and statues caused by acid rain is very slow, but the reactions that take place when a firework explodes are very fast. Most reactions take place at a rate somewhere between the firework explosion, which is almost instant. Finding out how quickly reactions take place and understanding why they happen at the rate they do is very important to the chemist. Speeding up useful reactions and slowing down harmful ones can be important in industrial production processes, and in activities such as preserving buildings or foodstuffs. The use of domestic refrigerators and freezers, as well as cold storage by wholesalers, in transit and in shops, makes modern methods of feeding large populations possible by slowing down the speed at which foods decay. The chemical reactions that take place in the human body happen at extremely slow rates when they are unaided. ...read more.

Middle

The rate at which carbon dioxide is evolved can be followed by attaching a gas syringe to a test tube in which the reaction is occurring and noting the volumes at fixed time intervals. By sampling the reaction mixture and the concentration of one of the components of the reaction mixture (either reactants or products) at regular intervals, the concentration of the reaction mixture can be estimated by titration. An example is the acid-catalysed hydrolysis of an ester such as ethyl ethanoate, CH3COOC2H5 + H2O � CH3COOH + C2H5OH. The reaction mixture is titrated at intervals against a standard solution of sodium hydroxide; there is a constant concentration of acid present as catalyst, so as the reaction progresses, more alkali is required due to the formation of ethanoic acid. In some reactions, electrical conductivity can be measured, as this changes as the reaction proceeds. For example, during the alkaline hydrolysis of bromoethane, C2H5Br + OH- � C2H5OH + Br-, the conductivity decreases because the fast-moving hydroxyl (OH�) ...read more.

Conclusion

I will change the Na2S2O3 solution from 0.2ml to 0.4ml, 0.6ml, 0.8ml, and finally 1ml in separate experiments). Using two measuring cylinders pour 0.5ml of HCL into one of the cylinders and the first amount of Na2S2O3 Into the other cylinder. 3. Draw an X symbol onto a clear sheet of paper. 4. Put the flask onto the paper and empty both of the cylinders into the flask and start the stop clock. 5. Repeat this experiment with all of the other concentrations of Na2S2O3 three times. Results: HCL Concentration (ml) Na2S2O3 Concentration (ml) 1st time (seconds) 2nd time (seconds) 3rd time (seconds) Average 0.5 0.2 30 31 32 31 0.5 0.4 23 22 25 23.5 0.5 0.6 10 11 14 12 Conclusion: My prediction was correct. As I added more Na2S2O3 the reaction speeded up and was shorter with the more Na2S2O3 I used. In my first experiment my average time of the X disappearing was 31 seconds and in my second concentration the time was only 23.5 seconds (average) and in my last experiment it the average was only 12 seconds. Harvinder Singh 11GK Harvinder Singh 11GK ...read more.

The above preview is unformatted text

This student written piece of work is one of many that can be found in our GCSE Patterns of Behaviour section.

Found what you're looking for?

  • Start learning 29% faster today
  • 150,000+ documents available
  • Just £6.99 a month

Not the one? Search for your essay title...
  • Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month

See related essaysSee related essays

Related GCSE Patterns of Behaviour essays

  1. Marked by a teacher

    In my investigation I am going to look at how concentration affects the rate ...

    3 star(s)

    All collisions will make a reaction in the experiment but not all collisions are successful, the rate of reaction depends on the number of successful collisions per second, which is directly proportional. The two things that are colliding in the collision are the hydrogen ions from the acid and the thiosulphate ions.

  2. Investigating the effect of temperature on the reaction between Sodium Thiosulphate (Na2S2O3) and Hydrochloric ...

    With a larger amount of Na2S2O3 than HCl the experiment should have happened slower not faster. After further trials I discovered that: Water 40mls Na2S2O3 10mls HCl 5mls gave me an adequate starting time of approximately 3:00 - 3:30 minutes at 20�C.

  1. The Rates of Reaction Between HCl and Na2S2O3.

    To work out the rate of reaction, I will inverse (1/time taken) the time it takes for the reaction to finish then I will multiply the time by 1000. This will give me my rate of reaction. I will then repeat the experiment increasing the concentration of the HCl by 1cm� and decreasing the H2O concentration by 1cm�.

  2. Investigate how concentration of hydrochloric acid (HCL) affects its reaction with calcium carbonate (CaCO3).

    I felt this was a suitable number of readings as it was not too many and not too few. Analysis If you turn to my next page you will see my graph. The graph shown on the last page shows the volume of CO2 gas produced (cm3) against time (seconds).

  1. Free essay

    Close Your Eyes

    and "how long had she been unconscious for?" it just made me more and more worried and I couldn't take it. I looked down at myself and realised I was only in my boxers, I wanted to go in the ambulance with Louise so I raced upstairs, shoved some clothes on and ran back down again.

  2. Rates of Reaction- Hydrolysis of Urea by Urease

    A pH range of 4, 5, 6, 7 and 8 were trialled in order to demonstrate a diverse range of outcomes. Each pH was trialled four times. Firstly, a ph of 4 was trialled. The experiment was first organised by preparing the apparatus and materials.

  1. Reaction between sodium thiosulphate solution (Na2S2O3) and dilute hydrochloric acid (HCl)

    But if the acid is more concentrated there are more H+ ions thus there is a greater chance of a successful collision occurring. At the start there are plenty of H+ ions and atoms of the other reactant, but during the reaction they get used up.

  2. How does the concentration of HCl affect the rate of reaction with CaCO3?

    27.20 27.10 26.90 33.20 N/A 27.07 60.00 0.45 24.00 25.00 0.75 32.10 31.90 31.90 N/A N/A 31.97 60.00 0.53 24.00 25.00 1.00 35.30 34.20 34.50 N /A N/A 34.67 60.00 0.58 24.00 25.00 1.25 41.20 40.90 41.00 40.60 35.60 41.03 60.00 0.68 24.00 25.00 1.50 45.10 45.20 44.90 40.30 N/A

  • Over 160,000 pieces
    of student written work
  • Annotated by
    experienced teachers
  • Ideas and feedback to
    improve your own work