Limestone's Reaction With Hydrochloric Acid
Planning the experiment.
This experiment will show how much limestone fizzes when added to
hydrochloric acid.
I will gather the gas released from the fizzing and measure how long
it takes to gather a certain amount of gas.
Burette
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The light blue area represents the hydrochloric acid, and the white
blobs are the limestone. The grey area is the carbon dioxide released
from the HCl and CaCO3 reaction, heading in the direction indicated by
the arrows. The dark blue areas are water.
Using this equipment, I will conduct 5 tests, each one with the same
equipment, the same mass of limestone, the same volume of acid, but in
each test the acid will be a different strength. This keeps it all a
fair test. The 5 acid strengths will be
0.5M, 0.75M, 1.0M, 1.5M, and 2.0M. I will conduct each test twice, so
as to obtain two sets of results for each acid strength. This will
enable me to take averages.
This idea of taking averages will account for any slight mishaps in
the tests, for example, different air temperatures can affect how
quickly the reaction between the CaCO3 and the HCl takes place.
I predict that the stronger the acid is, and the warmer the air is,
the faster the limestone will react with the hydrochloric acid. This
prediction is based mainly upon the collision theory, for this states
that as substances heat up, the molecules and the atoms move around
faster, in this case the acid moves and collides with the limestone
more, causing the reaction to increase in speed. Also, the more
concentrated the acid is, the higher the strength of the reactions
are.
The strategy I choose to take is that of placing the limestone into
the acid, activating the stopwatch, and putting the bung in the top of
the flask as quickly as possible. There will be 50 millilitres of
water in the glass tube. I will allow the carbon dioxide to travel
An Experiment to Find Out How Much Gas is Given Off When Hydrochloric Acid and Marble Chips React
Apparatus: * 1 measuring cylinder * 1 test tube * 1 stop clock * A large gelatine cube containing indicator and NaOH * Hydrochloric acid ranging from 1-3 molars * A scalpel Diagram: Method: * Take the large gelatine cube and cut into 15 equal pieces * Place on piece of the cube into the test tube * Measure out 10mls of HCl in the measuring cylinder * Pour the HCl into the test tube with the gelatine cube and start the clock * Time how long it takes for the pink colour inside the gelatine cube to completely disappear * You will also notice that the cube dissolves slightly * Record your results and repeat this same process 3 times for each molar of acid: § 1 molar § 1.5 molar § 2 molar
Investigating How the Concentration of Hydrochloric Acid Affects the Rate of Reaction with Calcium Carbonate
Investigating the Rate of Reaction Between Marble Chips and Hydrochloric Acid I am investigating the rate of reaction between marble chips (calcium
as: a.. * Temperature * Concentration of acid * Surface area of chalk * Pressure Light intensity (this is a very small effect so it doesn't really. count and I won't take it into account). Whether a catalyst is present (in this experiment there isn't one).
Experiment is to investigate the rate of reaction between hydrochloric acid and calcium carbonate Hydrochloric acid + Calcium Carbonate Þ Calcium Chloride + Water + Carbon Dioxide 2HCl (aq) CaCo3 (s) CaCl2(s) H2O (aq) CO2 (g) There are a number of variables in this experiment and these are listed below as input variables and outcome variables.
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.
My prediction of this experiment is that the results will be a minimum difference of 2-3 ml between each other at the beginning but when it comes down the middle there will be a difference of 4-5ml. This is because I believe that as there is more water at the start of the burette it will slow it down, but when coming down the middle it will go faster.
The product of CaCO3 is formed, “…from the reaction of carbon dioxide with burnt (I) or slaked lime (II)” (Kroker, Rohleder, Tegethoff). Historians and scientists have concluded that the natural element, calcium, was molded into different compounds due to the underwater pressure that collided with the volcanic rocks. In contrast, with high concentrations of carbon dioxide and low pressure, these calcium compounds can also be dissolved. The change in water pressure was due to drastic globate climate changes, and deformations of the seabed. This phenomenon can be hypothesized as the time when the Earth’s plates began shifting and colliding. As time progresses, vast limestone deposits on lakes and oceans (Kroker, Rohleder, Tegethoff). Calcium is not only known the main component for our teeth and bones, but aquatic life also depends on it (i.e. mussels and mollusks). Marble and chalk are also forms of calcium that undergo particular
The amount of hydrochloric acid. 3. The concentration of the hydrochloric acid. 4. The surface area of the calcium carbonate.
If there is not enough energy no reaction takes place. In a solution of 0.5M hydrochloric acid, there are less hydrochloric acid particles compared to that of 2M hydrochloric acid, therefore, there are less particles to react with magnesium particles thus meaning less chance of collisions between the two reactants: [IMAGE] Therefore, as the concentration of the hydrochloric acid is increased, the chances of collisions increase thus giving a faster rate of reaction. Apparatus: Beaker Hydrochloric acid Distilled water Measuring cylinder Pipette Test tubes Test tube rack Diagram: [IMAGE] Method: Measure out 10cm3 of hydrochloric acid, as the concentration requires, for each concentration its composition is: Moles Volume HCl Volume Water 2M 10 cm³ 0 cm³ 1.5M 7.5 cm³ 2.5 cm³ 1M 5 cm³ 5 cm³ 0.5M 2.5 cm³ 7.5 cm³ 0M 0 cm³
The Effect of Temperature on the Rate of Reaction Between Hydrochloric Acid and Calcium Carbonate
Limestone aggregates are produced by the crushing of sedimentary rock precisely limestone, which comprises mostly of calcite (calcium carbonate - СаСО3).
An investigation into how changing one variable influences the rate of reaction between marble chips and dilute Hydrochloric acid
I will have to keep the volume of the acid, the mass and size of the marble chips and the temperature of the acid the same in all my experiments to insure a fair test, because by changing any of the above I will change the conditions and therefore the results will be inaccurate and the rate of reaction will be affected. The products of the reaction between the hydrochloric acid and the magnesium ribbon are calcium chloride, water and carbon dioxide. CaCO3 (s) + 2HCl(aq) CaCl2 (l) + H2O (l) + CO2 (g)