An Investigation to See What Effects the Neutralisation of Acids by Antacids

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An Investigation to See What Effects the Neutralisation of Acids by Antacids

In this experiment I will be looking at what affects the rate of reaction in a chemical reaction between Hydrochloric acid and commercial antacids. I will be looking at one of the Rates of reaction, surface area, to see if a smaller surface area does speed up a reaction.

The reason that I became interested in this experiment is that I have been suffering from terrible indigestion of late and was wondering what would affect the efficiency of the tablets. Indigestion is a common condition caused by excess (or too strong) acid in the stomach, using antacids, usually a salt containing either an earth or alkali metal, always a base, neutralises the acid in the stomach relieving pain.

In chemical reactions atoms are rearranged. This rearrangement (and the reaction) is caused by the collision of atoms. In gases and liquids, contact with solids and with each other millions of collisions occur very second. If all these were successful and caused a reaction then every reaction would be over in a millionth of a second. Because reactions aren't over in such a quick speed one can presume that not all collisions are successful. To be successful a collision has to occur with enough energy and directly. A good analogy for this is bumper cars at a fair ground. A glancing hit does little but a head on collision hurts!
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Several things govern the rate of a reaction.

I predict that as the surface area of one of the reactants (the tablet) increases so will the rates of reaction. This is because of the reasons discussed above.

I set up the apparatus as below and used the equipment safely.

. I broke the tablet into smaller sizes as per the experiment demanded

2. In this experiment I will be using 0.25-M hydrochloric acid because antacid tablets are designed to work in our stomach, in which is hydrochloric acid. I was provided with 2M hydrochloric ...

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