In: Chemistry
How many grams of CaCO3 are required to neutralize 900. mL of stomach acid, which is equivalent to 0.0100 M HCl?
CaCO3 can neutralize stomach acid.
If stomach acid is equivalent to 900ml of 0.01 M HCl
the mmoles of HCl = molarity*volume in ml = 0.01M*900ml = 9 mmoles
The neutralization reaction will be -
CaCO3 + 2HCl -> H2O + CO2 + CaCl2
So, each mole of CaCO3 can neutralize 2 moles of HCl,
so, to neutralize 9 mmoles of HCl we need 9/2 mmoles of CaCO3
9/2 mmoles = 9/2 * 10-3 moles
Molar mass of CaCO3 = molar mass of Ca + molar mass of C + molar mass of O*3
= 40g/mole + 12g/mole + 16g/mole*3 = 100g/mole
So, weight of 9/2 mmoles of CaCO3 = molar mass*moles
= 100g/mole * 9/2 * 10-3 moles = 0.45 g
So, we need 0.45 g of CaCO3 to neutralize the stomach acid.