Question
Asked Mar 9, 2020
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Assuming that stomach acid is 0.150 M HCl (density, 1.00 g mL-1), what mass of acid would a 500 mg antacid tablet composed of Na2CO3 neutralize?  (Hint:  The neutralization reactions for Na2CO3 are similar to those written for CaCO3 in the Introduction.)
 
 

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Expert Answer

Step 1

Given,

Molarity of HCl solution = 0.150 M = 0.150 mol/L

Density of HCl solution = 1.00 g/mL

Mass of Na2CO3 = 500 mg = 0.500 g    (1 mg = 0.001 g)

 

Moles of Na2CO3 can be calculated as :

Chemistry homework question answer, step 1, image 1

Step 2

The balanced neutralization reaction of Na2CO3 and HCl can be written as:

Na2CO3 + 2 HCl → 2 NaCl + H2O + CO2

 

From the given reaction, it is evident that :

Chemistry homework question answer, step 2, image 1

Step 3

Volume of HCl required can be calculated as :

Chemistry homework question answer, step 3, image 1

...

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