• Join over 1.2 million students every month
• Accelerate your learning by 29%
• Unlimited access from just £6.99 per month
Page
1. 1
1
2. 2
2
3. 3
3
4. 4
4
5. 5
5

# Investigation to find out the effect of acid concentration in dilute hydrochloric acid and magnesium ribbon, and how much hydrogen gas is given off.

Extracts from this document...

Introduction

Rates Of Reaction Aim: To find out the effect of acid concentration in dilute hydrochloric acid and magnesium ribbon, and how much hydrogen gas is given off. Prediction: I predict that as the concentration of the hydrochloric acid increases the time taken for magnesium ribbon to dissolve will decrease. Apparatus: Saturated test tube Rubber bung Bowl water Magnesium ribbon Concentrated hydrochloric acid Plastic tube Stopwatch Conical flask Measuring cylinder The concentration of the acid is going to be my only variable. It will vary the time taken for the magnesium ribbon to dissolve into the acid. Other things that I will be using are not going to be varied these are volume of hydrochloric acid and magnesium ribbon. The magnesium ribbon dissolves into the hydrochloric acid because then it collides with the particles inside the hydrochloric acid. Activation energy is minimum amount of energy required for a reaction to take place. For each of the concentrations I use the activation energy will be different. If the activation energy is high then only a small amount of particles will have enough energy to react but if the activation energy is low then a lot more particles can react. The reaction will also be exothermic because it will be giving off heat and hydrogen gas. A change in concentration is a change in the number of particles in a volume. If we increase the volume the particles will collide more because they are crowded. Factors: The factors that could affect the rate of reaction are as follows: Concentration of Acid This could affect the rate of reaction because the higher that concentration of the acid the more particles there are so there is more collision per second. Temperature: If the starting temperature of the acid is different each time then the speed at which the atoms will collide will increase or decrease depending on what the temperature is. ...read more.

Middle

This means they atoms will gain more energy and will collide more frequently per second. Surface Area of Magnesium: If the magnesium has more surface area then more sides are exposed to the acid this means that the time taken for it to dissolves will speed up. Type of Acid: If we changed the acid then the rate of reaction would also change because different acids have different concentrations. The main factor I have chosen is the concentration of the acid. I have chose this because several different concentrations can me made up for my experiment by the lab technicians. Diagram: Method: Firstly I set all my apparatus up correctly in order to proceed with the experiment. An equation for the reaction: Magnesium + hydrochloric acid > magnesium chloride + hydrogen I am going to be using 3 concentrations of hydrochloric acid these are 2 molar, 1 molar and 0.5 molar. I measured the amount of acid in a measuring cylinder then we poured 25cm3 of hydrochloric acid each time to make it a fair test and single piece of magnesium ribbon each time. We placed the saturated test tube full of water in the bowl and measured how much gas was given off every 10 seconds. When we did the experiment we made sure that the stopwatch was started exactly the same time as the magnesium was added to the acid. The reaction ended when the magnesium was dissolved completely. We all wore safety goggles and aprons to protect ourselves from harmful acid. We made sure that we weren't distracted during the experiment so we could get accurate results. Results: The result for the amount of gas produced when magnesium ribbon is dissolved is shown in the tables and graphs below. From my results I can see that the more concentrated hydrochloric acid dissolves the magnesium ribbon quicker than if it was less concentrated. ...read more.

Conclusion

I conclude that if the concentration of the acid is doubled then the amount of gas produced is at least over half if it is not doubled. This is because the ions collide more often in a more concentrated solution. When magnesium was added to the acid it fizzed and hydrogen gas was given off. The solution turned sliver as the magnesium dissolved this is because of magnesium's physical properties. In the process it is the hydrochloric atoms that need the activation energy because they are the ones that are moving and causing the reaction. They react with the magnesium to form a product called magnesium chloride. Evaluation: My method of carrying out the experiment was fairly accurate. This is because I washed out the beakers so they were clean for other concentrations. I measured the same amount of hydrochloric acid each time. I made sure I stopped the stopwatch at the right time. On the other hand it would have been better if I used I new beaker each time so then there wouldn't be any water left at the bottom of the beaker. If I was to do the experiment again I would make sure that all the pieces of magnesium ribbon I used were the same size and that I sandpapered the magnesium to make sure it had a clean surface. I would also make sure that the concentration of the acid was exactly what it was supposed to be. I would like to make the magnesium the variable next time and see what would happen if I used different sizes of magnesium ribbon. However I also did an experiment with sodium thiosulphate and I found out that the time taken for the cross to disappear depends on how concentrated the hydrochloric acid is. I say that the acid to water ratio is bigger this means that there is more acid to water and because of this there are more hydrochloric molecules. The colour of the solution also changed in the sodium thiosulphate experiment as they started to react, it turned into a greenish yellowy colour. ...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 Aqueous Chemistry 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

# Related GCSE Aqueous Chemistry essays

1. ## How much Iron (II) in 100 grams of Spinach Oleracea?

0.0000506 x 1000 = 0.0506 mols dm-3 At a temperature of 60 oc Firstly work out the moles of Potassium Manganate (VII) (aq) in the titration. Moles = Concentration x Volume Moles = 0.01 mol dm -3 x 21.58 cm3 1000 The volume of the average titre is divided by 1000 to change the units from cm3 to dm3.

2. ## The effect of Acid Rain on Seed Germination.

After 10% concentration the average length of the seed's growth dramatically drops, this may be due to the fact that too many enzymes had been denatured and so the growth of the cress was seriously stunted. The cress only grew well at 0% and 10% concentrations of the acid rain

1. ## See how different concentrations of Hydrochloric acid change the rate of reaction with a ...

Ways in which I will record my experiment There is several ways which I could record my experiment, but here are the two which I am planning to do: Amount of gas evolved I could use a gas syringe to collect the gas that will evolve from my experiment.

2. ## Investigating the effect of a chosen factor on the activity of Lipase

Preliminary Experiment: This experiment is to determine the best conditions for testing of the metabolic action of Lipase, and the role of Bile in the process. So it must be done at 40?c, for optimum reaction rate (as theoretically noted).

1. ## Finding out how much acid there is in a solution.

* Swirl the flask with your hand slowly whilst the acid solution is being added to the 25cm� solution drop by drop. This is to make sure that the acid solution is evenly distributed throughout the sodium carbonate solution. Once the solution in the conical flask becomes clear and colourless stop the tap.

2. ## Rate of Reaction between Sodium Thiosulphate and Dilute Hydrochloric acid

Another reason for my bad result could be that I did not wash the equipment (the conicle flask, cylinders) properly which meant that there was still sulphur left in it which therefore affected my result.

1. ## Find out how much acid there is in a solution

* At the same time the conical flask must be rapidly swirled around but making sure that it doesn't bump into the tap. * Look for any changes in the appearance of the Sodium Carbonate solution. * When there is a change in colour, lower the flow of acid solution from the burette tap.

2. ## whether the strength of Hydrochloric acid will affect the speed of the rate of ...

Burette Method Equipment Conical Flask, Bung, Connecting Pipe, Burette, Large Measuring Jug. For this method we first set up the equipment needed to carry out the burette experiment as shown below; The burette method consists of the Magnesium ribbon being put into a conical flask with 50ml of hydrochloric acid

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