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

How the Concentration of Acid in a Solution affects the Rate of Reaction

Extracts from this document...

Introduction

Investigation into: How the Concentration of Hydrochloric Acid in a Solution affects the Rate of Reaction Aim: This experiment was to observe how the concentration affects the rate of reaction between chemicals. The two chemicals used in our experiment were Sodium Thiosulphate and Hydrochloric Acid. Introduction: The rate of reaction is basically the speed of how fast the reaction occurs between two reactants. You measure this speed in seconds, and have to set an achieving limit, which is a standard point of the reaction where a change is noticed and that is where the time must be recorded. A reaction is the simply the collision of the particles in two different substances (reactants). This essay is about writing how we observed the chemical reaction we carried out. Now here's the bit where the story gets interesting... My Prediction: My prediction is that: as long as the chemicals react in the same amount as was set, the speed of the reaction will be faster as the concentration (molarity) of the Hydrochloric Acid is increased. I predicted this because generally, when something has a higher concentration, it reacts quicker than when it has a lower concentration. This theory is ~ "Increasing the concentration increases the rate of reaction". This is because when there are more particles present, there is more collision between the particles; this increases the rate of reaction. ...read more.

Middle

The concentrations of the Hydrochloric Acid were 1M, 1.5M, 2M, 2.5M and 3M. We did the experiment with each concentration 5 times to be totally accurate. Then, carefully, we put away the chemicals and we washed the apparatus that needed to be washed, and cleared up. This is an important part of an experiment as the "health and safety" policy is essential. Without carefully putting away the apparatus, the irritant chemicals and glass tubes could be harmful, and may be fatal. Results Table: Concentration Of Hydrochloric Acid (Mole) Time taken in reaction. 1stTime (mins) Time taken in reaction. 2ndTime (mins) Time taken in reaction. 3rdTime (mins) Time taken in reaction. 4thTime (mins) Time taken in reaction. 5thTime (mins) Average Time (mins) 1M 3.24 1.14 1.18 1.14 2.48 1:08:72 1.5M 1.08 1.02 1.05 1.13 1.13 1:00:82 2M 1.05 1.07 1.10 1.03 1.10 1:00:70 2.5M 1.06 1.07 1.03 1.06 1.08 1:00:60 3M 1.00 1.05 1.00 1.03 1.02 1:00:20 (Graph for table of results attached on next page) Conclusion: There are a few areas I want to cover in the conclusion about this experiment. The patterns I noticed occurring as the reaction continued were related to the variable reactant. The pattern was that when we added Acid with more concentration to the Sodium Thiosulphate, the reaction was faster. This means that the slowest reaction was when Sodium Thiosulphate reacts with Hydrochloric Acid with a molarity of 1M; and the fastest reaction was when Sodium Thiosulphate reacts with Hydrochloric Acid with a molarity of 3M. ...read more.

Conclusion

So there was no mix of molarity. That was a sensible idea to gain reliable results. The thing that concerned me was the results ~ We were unsure at what point to note the time, so the first set of outcomes were slightly dodgy. This confusion was first revealed when the cross underneath the conical flask failed to totally fade. So then we randomly stopped the time when we got fed up of waiting, and after that, we stopped the time when the some parts of the cross were not entirely visible. This made the outcomes similar to the pattern, and the "increasing concentration" theory made proved itself true in the practical. We could have also used computer sensors for timing which would have given us more accurate results. Also, repeating this experiment as many times as possible would lead to better results and a stronger conclusion. There are many different experiments that we could carry to investigate the rate of reaction. Some of these are: * Varying the temperature * Applying pressure * Increasing surface area of the particles * Using a catalyst My overall comment for this experiment is that: Despite using accurate but imperfect equipment, my practical was a complete success and matched the theory that "the rate of reaction is directly proportional to the concentration of the reactants. ?? ?? ?? ?? ~ Syed Jafri ~ 11 East ~ Chemistry Coursework ~ Page 1 of 7 ...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

Here's what a teacher thought of this essay

3 star(s)

This report is not very well structured and does not follow the scientific standard required. The only reason it achieved three stars is the reliability of the data collected. There are more specific improvements and strengths suggested throughout.

Marked by teacher Cornelia Bruce 17/04/2013

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

    Marble Chips and Hydrochloric Acid.

    4 star(s)

    This is something that we will bear in mind during our investigation. Conclusion of Pre Investigation The results of our pre investigation show us that using 30cm� of acid provides a steady reaction with whatever the concentration. Using a volume below this does not create a reaction within the allocated

  2. Marked by a teacher

    Chemistry Coursework - How the concentration effects the rate of reaction between sodium thiosulphate ...

    I kept everything a close as possible to my preliminary test as I think it went vary well. There seemed to be no error and it all ran rather smoothly. I decided there was no real reason to keep the temperature results as this was not part of my experiment

  1. The effects of caffeine on reaction time

    Overall while looking at the tables it is seen that ther is a difference in the reaction times. It is almost halved which does show some effect of caffeine on the reaction time. To further test the reliability and accuracy I carried out a statistical test: Z test for matched samples.

  2. Investigation on how long a candle burns under a glass beaker.

    The factors that I will change are the size of the glass beakers ONLY. Everything else will be kept the same. We are aiming to measure how long the candle burns for. To make my experiment safe, we will be wearing goggles throughout the whole experiment, and we will make as less mess as possible.

  1. Factors Affecting the Rate of Catalytic Decomposition of Hydrogen Peroxide.

    is not supposed to be doing so * Unclean equipment - if the equipment was not fully clean it would make some of the chemicals react before the experiment, and therefore there would be less mass loss due to some of the particles having already collided with eachother * The

  2. The reaction between Sodium Thiosulphate and Hydrochloric Acid.

    Chemical reactions take place when reacting particles collide with an amount of energy greater than or equal to the activation energy. The next diagram shows what the activation energy of a reaction looks like when represented on a graph. As you can see, the graph goes up before it starts to come down.

  1. To investigate the effect of the concentration of nitric acid on the rate of ...

    A reliable solution would be to place the conical flask in a thermostatically-controlled water bath. This means that one can set a desired fixed temperature (e.g. room temperature 25�C) for the water and the thermostat of the water bath will use a method called a feedback loop to compare the desired temperature to the actual temperature of the water.

  2. Studying the reaction between zinc and copper (2) sulphate solution.

    Using the same polystyrene cup was another thing which may have contributed to not entirely trustworthy results as although the cup was cleaned after each experiment it would have been more reliable to use a new cup each time, as it may not have been completely cleaned out of all traces of zinc.

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