Evaluating the Antacids Efficiency

Sophomore (College 2nd year) ・Chemistry ・APA ・4 Sources

Excess acids in the belly causes a number of problems and ailments. These include heart burns and acid reflux which are cured the use of antacid drugs. The antacids play a key role of neutralizing the acid thereby leading to a impartial pH at the stomach. The neutral pH is vital on the grounds that it does not erode the walls of the stomach. Antacids have three frequent ingredients which react differently with the belly acids. These include magnesium hydroxide (Mg(OH)2), Sodium hydrogen carbonate (NaHCO3), and Calcium carbonate (CaCO3) (Edwards & Ball, 2014).

In determination of the efficacy of each of the antacids, 0.88M Acetic acid is used as the acid. In the presence of Bogen’s universal indicator, the progress of the reaction is precisely monitored over a wide range of pH (indicated by several colour ass shown, figure 1). The equivalence point is achieved when the moles of the acid are equal to that of the base.

Considering NaHCO3, the vigorous ingredient in it, Alka-Seltzer reacts with acetic acid forming Sodium ethanoate, carbon (IV) oxide and water (Jakaria et al., 2015).

NaHCO3 (aq) + CH3COOH (aq) ‑‑‑‑‑‑‑‑‑‑‑‑‑‑‑‑‑> CH3COONa (aq) + CO2 (g) + H2O (l)

For Calcium carbonate, the products include calcium acetate, water, and carbon dioxide. The reaction is (Timberlake, 2015);

CaCO3 (l) + 2CH3COOH (aq) ‑‑‑‑‑‑‑‑‑‑‑‑‑‑‑‑‑> Ca (CH3COO)2 (aq) + CO2 (g) + H2O (l)

On the other hand, Magnesium hydroxide reacts with acetic acid to give a suspension which is considered milk of magnesium. This is indicated by the equation below (Jacob et al., 2016);

Mg(OH)2 (aq) + 2CH3COOH­­­­­­­­­­­­­­­­­­­­­ (aq) ‑‑‑‑‑‑‑‑‑‑‑‑‑‑‑‑‑> Mg (CH3COO)2 (aq) + H2O (l)

The process is repeated using Tums and Rolaids instead of Alka-Seltzer.

Reagents and Apparatus used

The reagents and apparatus used include Bogen’s universal indicator, milk of magnesia, roll of Tum or Rolaids, 2 pack of Alka-Seltzer syringe, balance, plastic cup, 50ml Graduated cylinder, water, and a sheet of paper (Timberlake, 2015).


The experiment was done in three activities using Alka-Seltzer, Milk of magnesia, and Tum using defined steps. Using a large plastic cup weigh 5g of acetic acid and add 20mL of tap water and stir gently. This is followed by 5 drops of Bogen’s universal indicator. One tablet of Alka-Seltzer is weighed and the mass recorded in the table and added to the solution. The tablet is dissolved and the colour of solution recorded (for yellow colour the volume of 0mL is recorded for volume of NaOH). 10mL of 1M NaOH was transferred and filled to the syringe and initial volume recorded. 0.1mL is added from the syringe till the orange colour persists. Once the equivalent point is reached, the final volume of 1M NaOH was recorded in the table. The total volume of NaOH used was calculated, the solution was disposed and experiment repeated using the second tablet (Timberlake, 2015). Moles of acetic acid that was used in each trial was calculated and recorded using the relationship;

Volume of acetic acid= Mass/Density x 1000

Moles= volume x concentration

Also, moles of NaOH that was used in each trial was calculated using,

Moles = volume/1000 x concentration.

Moles of NaHCO3 for each trial was calculated using,

Furthermore, neutralization capacity of each trial was calculated using,

The procedure was repeated using Tums (activity 2) and milk of magnesia (activity 3). Several readings were also recorded in the respective activities.

Moles of CaCO3 used in each trial was calculated using, and the data was filled in table 2.

For moles of Magnesium hydroxide, its moles was calculated and recorded using,

Finally, the neutralization capacity for each trial using tums and milk magnesia was calculated and recorded using,

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