Question

In: Chemistry

given the five commercial products mentioned in the write up, Tums, Buffered aspirin, milk of Magnesia,...

given the five commercial products mentioned in the write up, Tums, Buffered aspirin, milk of Magnesia, Rolaids and Alka Seltzer, which would you expect to be more effective on mass basis to neutralize stomach acid? Back your reasoning with pertinent calculations.

Solutions

Expert Solution

Antacids are compound that neutralize the stomach acid

Take each tablet in turn - say you start with Tums.

Determine its composition. Then start to work out how much HCl the tablet can neutralise.

You then do this for each tablet in turn.

I will do this using the data of my own tablet:

Molar mass CaCO3 (tums) = 100g/mol
Molar mass MgCO3 = 84 g/mol

680mg CaCO3 =0.680/100 = 6.8*10-3 mol CaCO3
80mg MgCO3 = 0.080/84 = 9.52*10-4mol MgCO3

From your balanced equation you will see that 1 mol CaCO3 reacts with 2mol HCl
6.8*10-3 mol CaCO3 reacts with 2*6.8*10-3 = 1.36*10-2 mol HCl
Likewise, for MgCO3
9.52*10-4 mol MgCO3 reacts with 2*9.52*10-4 = 1.904*10-3 mol HCl

1 tablet will react with (neutralise):
1.36*10-2 + 1.904*10-3 = 1.55*10-2 mol HCl

Molar mass HCl = 36.5g/mol
1.55*10-2mol = 36.5* 1.55*10-2 = 0.566g HCl.

1 of my antacid tablets will neytralise 0.556g HCl

Now you go ahead and do exactly the same for your antacid tablets.

If Tums regular. I found: Active Ingredients: Calcium Carbonate USP (500 mg) (Antacid).

This is a simple exercise:
500mg CaCO3 = 0.500/100= 5.0*10-3mol CaCO3
This will netralise = 1.0*10-2 mol HCl
Molar mass HCl = 36.5g/mol:
1*10-2mol = 0.365 g HCl

Same do with milk of Magnesia( Mg(OH)2),and Alka Seltzer (KHCO3 and NaHCO3)


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