3. Each day, the stomach produces 2.0 L of gastric juice that contains 0.10 M HCl. Phillips Milk of Magnesia is a white-colored, aqueous, mildly alkaline suspension of magnesium hydroxide formulated at 8.0 % (w/v). It would take ________ mL of milk of magnesia to titrate the stomach acid produced in each day. (Mg(OH)2 molar mass = 58.32 g/mol)
To solve this problem, we first need to calculate the amount of HCl in the 2.0 L of gastric juice produced each day.
1. Calculate the amount of HCl in the gastric juice:
2.0 L x 0.10 mol/L = 0.20 mol HCl
2. Next, let's calculate the amount of Mg(OH)2 needed to neutralize the HCl in the gastric juice:
1 mol of HCl reacts with 2 mol of Mg(OH)2 (from the balanced chemical equation)
So, the amount of Mg(OH)2 needed = 0.20 mol HCl x 2 mol Mg(OH)2 / 1 mol HCl = 0.40 mol Mg(OH)2
3. Calculate the mass of Mg(OH)2 needed:
0.40 mol Mg(OH)2 x 58.32 g/mol = 23.33 g Mg(OH)2
4. Finally, let's convert the mass of Mg(OH)2 to volume:
%w/v = (mass of solute / volume of solution) x 100
8.0 % = (23.33 g / volume) x 100
volume = 23.33 g / 8.0 g/mL = 2.92 mL
Therefore, it would take 2.92 mL of milk of magnesia to titrate the stomach acid produced in each day.