Assuming that stomach acid is 0.100M HCl, how many grams of acid will be neutral

Question

Assuming that stomach acid is 0.100M HCl, how many grams of acid will be neutralized by a Maalox antacid tablet that contains 0.500 g of CaCO_3 ? If you want to increase the pH of the stomach from 1.00 to 2.00 using an antacid tablet, how many grams of CaCO_3 will be required to change the pH value? Assume the acid is HCl and you have a 1.00L stomach volume. Magnesium hydroxide, Mg(OH)_2 is another active ingredient of some antacids. How does Mg(OH)_2 work to relieve the pain caused by excess stomach acid? Write the equation for this acid-base-neutralization reaction. An antacid tablet was dissolved in 26.00mL of 0.650M HCl. The excess acid was back-titrated with exactly 11.34mL of 1.05M NaOH. The average weight of a tablet is 0.834g. The tablet came from a bottle of 150 tablets that cost $3.99. Calculate the moles of HCl neutralized by the tablet. Calculate the mass effectiveness of the antacid. Calculate the cost effectiveness of the antacid.

Explanation / Answer

Q2

HCl = 0.1 M

find grams of acid fo aalox antacid table

m = 0.5 g of CaCO3

mol = mass/MW = 0.5/100.0869 = 0.004995 mol of CaCO3

so.

2HCl + CaCO3 = CaCl2 + H2O + CO2

s...

ratio is 2:1 so 2 mol of HCl react with 1 mol of antacid

0.004995 mol of antacid require --> 2x0.004995 = 0.00999 mol of HCL

so..

M = mol /V

V = mol/M = 0.00999 / 0.1 = 0.0999 Liters = 0.00999 *10^3 = 9.99 mL of about 10 mL of acid

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