Titration of an Antacid (Lab Report Sample)
The lab report involves determining the concentration calcium carbonate in an antacid tablet using back titration.source..
CH 111 – Introduction to Inorganic and Organic ChemistryLab 7 – Exp. 478 – Titration of an Antacid
In this lab we are going to determine the amount of HCl one antacid tablet can neutralize. We are going to utilize a titration to perform this analysis, however we cannot do the standard titrations we have done the previous 2 labs. Instead we will be performing something called a back titration.
A back titration involves adding an excess of one of the reactants in the neutralization reaction, and then titrating back the excess amount added. This is necessary because the antacid tablet is insoluble in water, so in order to get the ions in solution we must first react the antacid (Calcium Carbonate (CaCO3)) with excess HCl, according to reaction 1 below. Some of the HCl will be neutralized by the CaCO3, but the excess will remain in the flask. The excess HCl will then be titrated with NaOH, just as we did in Exp. 5 according to reaction 2 below. Since we will know the exact amount of HCl added, we can determine the amount of HCl that that was not neutralized by the antacid. We can then determine the amount of HCl that was neutralized by the antacid.
1 2049145119136002 HCl (aq) + CaCO3 (s) CaCl2 (aq) + H2O (aq) + CO2 (g)
2 20540781204060HCl (aq) + NaOH (aq) NaCl (aq) + H2O (aq)
1 What was the mass of the tablet in the video?
2 What was the concentration of the NaOH in the video? (Normal is the same as Molar in this example.)
3 How many mL of distilled water did he add?
No amount of water was added to the samples.
4 How many drops of phenolphthalein were added?
5 Why does HCl need to be added to the tablet in the beginning of the experiment?
The HCl is added to neutralize the CaCO3
Mass of Antacid Tablet (g)
Molarity HCl (M)
Volume HCl Added to Tablet (mL)
Molarity NaOH (M)
Volume NaOH initial (mL)
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