Solve the problem below and upload a picture of your written work: Calcium carbonate is often used as an
antacid. Your stomach acid is composed of HCI at a pH of 1.5. If you ate toooo much Turkey and need to
neutralize 15.0 mL of stomach acid, how many grams of calcium carbonate would you need to take?

 

Given, pH = 1.5

We know that

pH = -log[H+]

1.5 = -log[H+]

[H+] = 10^-1.5

[H+] = 0.0316 M

HCl dissociate into H+ and Cl-

HCl --> H+ + Cl-

Concentration of H+ = concentration of HCl

Concentration of HCl = 0.0316 M

Given volume = 15.0 mL = 15.0*10^-3 L = 0.015 L

Mole of HCl = Molarity*Volume

Mole of HCl = 0.0316 M* 0.015 L

Mole of HCl = 0.000474 mol

Balance reaction

CaCO3 + 2HCl --> CaCl2 + H2O + CO2

2 mole of HCl react with 1 mole of Calcium carbonate (CaCO3)

0.000474 mole of HCl react with 1/2(*0.000474 mol) of CaCO3

Mole of CaCO3 react = 0.000237 mol

Molar mass of CaCO3 = 100.0869 g/mol

Mass of CaCO3 needed = mole* molar mass

Mass of CaCO3 needed = 0.000237 mol*100.0869 g/mol

Mass of CaCO3 needed = 0.0237 g