• 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
6. 6
6
7. 7
7
8. 8
8
9. 9
9
10. 10
10
11. 11
11
12. 12
12
13. 13
13
14. 14
14
15. 15
15
16. 16
16
17. 17
17
18. 18
18

# Experiment to investigate how changing the concentration of hydrochloric acid affects the rate of its reaction with the reactant

Extracts from this document...

Introduction

Experiment to investigate how changing the concentration of hydrochloric acid affects the rate of its reaction with the reactant Aim: Is to investigate how concentration of hydrochloric acid affects the rate of its reaction with the reactant. To decide which reactant I will use for my investigation, I will do preliminary experiments to decide this. Preliminary work I will be doing some different preliminary experiments. The preliminary will allow me to decide which reactants to use for my investigation and how much of that reactant to use in each experiment. Experiment 1a: Which reactant reacts best? 1. Display 3 beakers. In: * Beaker 1 place some chalk * Beaker 2 place some marble chips * Beaker 3 place some strips of magnesium 2. In each beaker pour some hydrochloric acid and observe the reaction. 3. Estimate the rate of the reaction on a scale of 0-5 (0= no reaction, 1= very slow, 2= slow, 3= medium, 4= fast, 5= very fast) I noted down the results, however, I realized that they are too inaccurate for me to base my decisions on them. Therefore, I will set a volume of hydrochloric acid to pour into the beakers and also I will weigh the reactants and make sure they all have the weight. Experiment 1b: Which reactant reacts best? 1. Display 3 beakers. In: * Beaker 1 place 2g of chalk * Beaker 2 place 2g of marble chips * Beaker 3 place 2g of strips of magnesium 2. In each beaker pour 40ml of hydrochloric acid and observe the reaction. 3. Estimate the rate of the reaction on a scale of 0-5 (0= no reaction, 1= very slow, 2= slow, 3= medium, 4= fast, 5= very fast) I noted my results and I will keep these because they are fairly accurate. However, I decided to extend my experiment and test marble chips and magnesium again but in a different form. ...read more.

Middle

However, I want to keep my experiment as fair as possible to get reliable results. * When I use the hydrochloric acid from the bottle I have to take off the lid and put it back on as quickly as possible. This has to be done for two reasons: 1. Hydrochloric acid evaporates 2. Hydrochloric acid decomposes when in contact with sunlight. * Weigh the chalk as accurately as possible because if the concentration of the chalk changes, then there would be another factor affecting the rate of reaction. Remember, I only want the concentration oh hydrochloric acid to affect the rate of reaction. If another factor affects the rate of reaction then my results will not allow me to see how the concentration of hydrochloric acid affects the rate of reaction. * Make sure that the cylinder of chalk used is new and is not cracked or dented. Otherwise, the surface area will affect the rate of reaction. As I have explained earlier, I don't want any other factor to affect the reaction. * When mixing the hydrochloric acid with dilute water, measure the amounts accurately in order to get the correct concentration. If I do not get the correct concentration my results will be incorrect. * When placing the cylinder of chalk into the beaker with hydrochloric acid, I have to do it as softly as possible without creating too much movement within the hydrochloric acid. * When the chalk is placed in the beaker I have to start the stopwatch as soon as possible because I have to start the time as soon as the reaction starts, therefore, I have to do this as quickly as possible for me to get accurate timings. * When doing the experiment I have to turn off the air conditioner. I have to do this for two reasons: 1. The AC affects the readings on the balance and random numbers appear. For me to get correct results I need the balance to function properly. 2. ...read more.

Conclusion

This would reduce the reaction surface of the chalk, lowering the rate of reaction. I should have used pure mineral chalk to avoid this. My results are based on the experiments I have done. My experiments were done following a detailed method I have written and I have also paid much attention to keeping the experiment a fair test. For each concentration, I have repeated the experiment three times and I calculated the average of the results I got for each concentration. The procedure that I have followed convinces me that my results are reliable. However, the fact that other factors were introduced into my experiment, means that my plan and method have to be more detailed in order to get even more accurate results. I would also consider doing more repetitions for each concentration to get an even more accurate average. To obtain more evidence to support my conclusion I could have used a wider range of substrate concentration to make sure there is no limit to the pattern I found in my analysis. Another thing I could have done, was to do more repeats for each concentration, this would make my results more accurate when calculating the average. To extend this investigation I should investigate reactions between hydrochloric acid and other reactants such as magnesium and sodium thiosulphate. This would allow me to see if the concentration does not only affect the reaction with chalk. The reaction between hydrochloric acid and magnesium would be: 2HCL+Mg MgCl2+H2 Hydrogen is released from the reaction. Therefore, I could use the same method to calculate the mass loss. However, if I use a different method, it would allow me to see if the results will be consistent. I would collect the hydrogen gas released in a syringe. I would measure how much hydrogen gas is released in a certain amount of time. This would allow me to calculate rate of reaction and see if concentration affects rate of reaction. ?? ?? ?? ?? Mohamed Maamir ...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

# Related GCSE Patterns of Behaviour essays

1. ## Marble Chips and Hydrochloric Acid.

4 star(s)

90 - 100 - 110 - 120 - 130 - 140 - 150 - 160 - 170 - 180 - From these results we can see that the reaction takes place quickly, within 50 seconds. We were unable to record any further results as the measuring cylinder we used was too small and so filled with the gas quickly.

2. ## Experiment to Investigate the Rate of Reaction between Hydrochloric Acid and Sodium Thiosulphate, with ...

is due to the collision theory, which happens while the reactions take place, which is by 'Increasing the concentration of a substance in solution means that there will be more particles per dm3 of that substance' (www. gcsescience.com). So the more particles there are in the substance 'the more will

1. ## Measuring the Rate of Reaction between Hydrochloric Acid and Calcium Carbonate

Therefore, there will be more collisions every second between the carbonate ions and the H+ ions. Thus, there will be more successful collisions between the atoms and the rate of reaction will increase. Quantitatively, if the concentration of hydrochloric acid is increased, I think the rate of reaction will increase

2. ## Investigate how changing the surface area of Calcium carbonate affects the rate of reaction ...

HYPOTHESIS: I predict that the powdered marble will react faster than the marble chips. This is because increasing the surface area increases the chance of the particles hitting the reactant and allows more particles to react with the reactant at once.

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

Record the amount of gas produced at 10 second intervals. 7. Repeat all of the abovementioned steps once more for more accurate results and take an average of the two results. If there is great variance in the two results, repeat a third time and take an average.

2. ## Investigating the reaction between Marble Chips and Hydrochloric Acid.

The reaction rate did not seem to show any signs of slowing down in the latter stages of the timed reaction, which was an opposite event to that I had predicted. This was almost certainly due to the fact that the experiment was not timed for long enough.

1. ## Effect Of Substrate Concentration On The Activity Of Catalase

These are called fruitful collisions. The fruitful collisions have sufficient energy (activation energy) to break the existing bonds and to form new bonds, which then form the products of the reaction. Increasing the concentration of the reactants and raising the temperature make more collisions and therefore more fruitful collisions which increases the rate of reaction.

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

Even though we couldn’t keep the temperature constant, we noted down the temperature of the solution before and after the experiment. * The range on some of the apparatus wasn’t very good, we could only see how much carbon dioxide was produced to the nearest 10th of 1 cm³ on

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