How the Concentration of Hydrochloric Acid Changes the Rate of the Reaction with Magnesium
Aim
The investigation that I will be doing is to investigate the rate of
reaction between Magnesium and Hydrochloric acid. Factors which will
effect this experiment will be
· The concentration of the acid because as you increase the
concentration of acid you will also increase the change of an
collision so there for speeding up the reaction
· Temperature. As you increase the temperature you will also increase
the rate of the reaction because the particles move around with more
energy so a greater chance of an reaction.
· Surface area. This will also effect the rate of collision because
there is more surface area able to react with the acid so increasing
the chance of an collision
Prediction
I predict that when I increase the concentration of the acid I will
notice an increase in the rate of the reaction. This is because there
is a greater chance of HCl particles reacting with an Mg atoms. This
is because If the concentration of any reactant in a solution is
increased, the rate of reaction is increased. Increasing the
concentration, increases the probability of a collision between
reactant particles because there are more of them in the same volume.
Apparatus
· A gas syringe
· Hydrochloric acid
· Magnesium
· Stop watch
· Beaker
· A flask
· Rubber bung
· Measuring cylinder
Diagram
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Method
1. a measuring cylinder with 50 ml of hydrochloric acid and pour it in
to a flask
2. Add three 2cm strips of magnesium to the flask.
3. attach the rubber bung with the gas syringe to the flask
4. start the stopwatch
5. record the volume of gas every 10 seconds
6. repeat this experiment altering the concentration of the
Hydrochloric acid by adding the following amounts of water
50ml HCl 0ml of water
How am I going to make it a fair test I will use a clean flask for
Investigating the Effect of Concentration on the Rate of Diffusion Aim: To find out if concentration affects the rate of diffusion. Prediction: I predict that the higher the concentration of acid the faster the reaction will be. Hypothesis: Diffusion is the spreading out of a gas or liquid from an area of low concentration to another area where it has a lower concentration until the overall concentrations are balanced. The Hydrochloric acid (HCl) diffuses into the gelatine cube of which contains Sodium Hydroxide (NaOH), which is an alkali. When the Hydrochloric acid combines with the Sodium Hydroxide they form salt and water, which is neutral therefore turning the pink cube to clear.
Investigating How the Concentration of Hydrochloric Acid Affects the Rate of Reaction with Calcium Carbonate
The first step that we took to accomplish our goal was to put on our safety goggles and choose a lab station to work at. We received one 400ml beaker, one polyethylene pipet, two test tubes with hole rubber stoppers, two small pieces of magnesium (Mg), one thermometer and a vial of hydrochloric acid (HCl). We took the 400ml beaker and filled it about 2/3 full of water (H20) that was 18 OC. Then we measured our pieces of Mg at 1.5 cm and determined that their mass was 1.36*10-2 g. We filled the pipet 2/3 full of HCl and poured it into one of the test tubes. Then, we covered the HCl with just enough H2O so that no H2O would be displaced when the stopper was inserted. After inserting the stopper, we placed the Mg strip into the hole, inverted the test tube and placed it in the 400ml beaker. HCl is heavier than H2O, so it floated from the tube, into the bottom of the beaker, reacting with the Mg along the way to produce hydrogen gas (H2). We then measured the volume of the H2, cleaned up our equipment and performed the experiment a second time.
Although this does not directly increase the number of particles, it does increase the number of particles that are available for the H+ ions to react with. This is shown in diagram 1 of appendix 2. The second way to increase the concentration in my experiment is to increase the concentration of the hydrochloric acid. By doing this you increase the number of H+ ions available to react with the calcium carbonate and therefore the number of collisions per second between the two increase.
will result in an increase in the speed of the rate of reaction it has
It is important however to note that the NH4 and K ions are still in
The aim is to find out if changing the concentration of the hydrochloric acid solution has an effect on the time taken for the reaction. The reaction that will take place is: Hydrochloric acid + Calcium Carbonate + Calcium Chloride + Water + Carbon dioxide 2HCl (aq) + CaCo3 (s) CaCL2 (aq) + H2O + CO2 (g). Collision theory - Collisions between reactant particles are needed. for the reaction to take place in order to form a product.
The Effect of Temperature of Hydrochloric Acid on the Rate of Reaction Between Hydrochloric Acid and Magnesium
Rate of Reaction Between Calcium Carbonate and Hydrochloric Acid Plan: In my experiment I will measure the rate of reaction between calcium carbonate and hydrochloric acid. The rate of the reaction is the speed that the reaction takes place so by measuring the rate I will measure the amount of time the reaction takes. Hydrochloric acid is a strong acid that is found in digestive juices in the stomach, it is also used for cleaning metals before they are coated. Calcium carbonate has a few forms including chalk and limestone the main use of these two materials is in the making of concrete, which is used for many things such as buildings. When you put calcium carbonate and hydrochloric acid together they react to form calcium chloride, carbon dioxide and water.
from 10cm to 50cm to make it easier to see the difference in a graph.
The Effect of Concentration of Hydrochloric Acid on the Rate of Reaction with Magnesium Aim: To investigate the effect of concentration of hydrochloric acid on the rate of reaction with magnesium Prediction: As the concentration of the hydrochloric acid increases, so will the rate of reaction Hypothesis: In a reaction, particles of two different reactants react together to form a product. The reaction only takes place on account of two things, if the particles collide, and if the collision has enough 'activation energy'. The two reactant particles, in this case magnesium particles and hydrochloric acid particles, must collide with each other on the correct 'collision course'. If this does not occur then no chemical reaction will take place. The reaction must also have enough energy, this can be affected by temperature, the more heat the particles have the faster they move and so the more energy therefore more chance of successful collisions.
Looking at the table of results above and the graph, it is shown that the higher the temperature got, the shorter the reaction time. The obtained results have been plotted on a line graph of the temperature of hydrochloric acid (y-axis) against reaction time (x-axis). This line graph in fig.2 also clearly shows that as the temperature increases, so does the speed of the reaction, shown by a reduction in the time taken. This corroborates the collision theory, where as the temperature of particles increase, the particles gain more kinetic energy and react with each other upon collision. This is shown as to happen in the hydrochloric acid, where the hydrochloric acid particles collide more with the particles of the magnesium ribbon as the temperature was increased. The above graph shows a gradual sloping curve, which gets steeper at higher temperatures. This shows that the reaction will reach a peak rate of activity as the gaps between the temperature and reaction times continue to decrease. The experiment fulfills the aim and clearly shows that as the temperature of a reaction is increased so does it’s rate of reaction, proving the hypothesis to be correct.
Because there are more molecules, the frequency of successful collisions is greater, and the reactions happen faster. Safety There are a lot of safety issues we must abide by in this experiment. We must remember that the substances we use in this experiment can be very harmful if used the wrong way. When doing this experiment, it may be necessary to wear safety goggles, as things are very unpredictable, and even though it is very unlikely that the solution will come out of the beaker during the experiment, one must still be cautious of spills. We must make sure that coats and bags are all out of the way while doing the experiment.
tube. Add 6 mL of 0.1M HCl to the first test tube, then 0.1M KMnO4 and