How long does it takes a strip of magnesium to dissolve in a solution of water and acid
Introduction
I am aiming to find out how long it takes for a strip of magnesium, to dissolve, in a solution of water and acid.
Variables
Ø Concentration of acid
Ø Length of Magnesium
Ø Temperature of water
Ø Temperature of acid
Ø Amount of acid
Ø Size of conical flask
Ø Time taken
Fair test
The variable I will change is the concentration of acid. I will keep the length of the magnesium the same, as with the temperature of the water, amount of acid, size of conical flask and time taken. To make it a fair test.
Plan – Safety
Put safety goggles on
Equipment list
Ø Conical flask
Ø Stop watch
Ø 2 molar acid
Ø Magnesium strips
Ø Measuring cylinder
Instructions
1) Firstly I collected all my equipment
2) Measure 50ml of acid into a measuring cylinder
3) Pour acid into conical flask
4) Cut off a piece of magnesium (5cm)
5) Put the piece of magnesium into the conical flask and start the stop watch
6) Watch the reaction take place, and when all of the magnesium dissolves, stop the clock
7) Record the time in your table
8) Repeat this process twice
9) Repeat the whole process for the different concentrations of acid.
Prediction
GRAPH
I predict that the higher concentration of acid, the faster the magnesium strip will dissolve. In the higher concentration acid there will be a higher number of hydrochloric acid particles, in the same volume. This will result in more collisions, which therefore speeds up the rate of reaction, which will cause the magnesium to dissolve quicker. GRAPH
Conclusion
I have found out, by looking at my graph and results table, that the higher the concentration of acid, the faster the magnesium will dissolve. This happens because more collisions are happening in the same volume.
This is caused by more hydrochloric acid particles being added to the solution. Evaluation
As you can see on my graph, there are no anomalous results. This clearly shows that all of my results were reliable.
The quicker the tablets will dissolve because there will be more water. particles to collide with. So the rate increases. * If the amount of tablets being used is increased for the same amount of water, i.e. as concentration increases, rate will increase. increase as well because there will be more collisions between particles.
We began this investigation by suiting up in lab aprons and goggles, we then gathered our materials, found a lab station and got to work. We decided to start with the magnesium in hydrochloric acid first, we measured out 198.5 L of HCl and put it in the foam-cup calorimeter and took initial temperature reading. We then selected a piece of magnesium ribbon and found its mass: 0.01g. This piece was placed in the calorimeter and the lid was shut immediately to prevent heat from escaping. We “swirled” the liquid mixture in the calorimeter to ensure a reaction, and waited for a temperature change. After a few moments, the final temperature was recorded and DT determined.
Magnesium is an important element necessary healthy bones and teeth. The use of all muscles, and nerves convert it into energy for daily living. It is also instrumental in maintaining adequate levels of calcium in the blood. Having a therapeutic magnesium level helps prevent cardiovascular disease and reduces the risk of bone loss. The body of the adult human contains about 2000 mEq of Mg. Half of this amount stays within the skeleton and the other half in soft tissues (Wacker and Parisi 1968). The normal concentration in the blood is somewhere in the ranges of 1.7-2.3 mg/dL (Magnesium, 2013)
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