These are two big questions pretaining to a lab ...(I know it's alot but bear with me) I need help.
If you know how to solve these plaese show all of your work, thanks!!!
1) During the pH lab, you saw a demonstration in which hydochloric acid was added to a mixure containing ice, water, universal indicator, and Milk of Magnesia (MOM) is a saturated solution of Mg(OH)2, a fairly insoluble base with molar solubility of 1.317x10^-4 M. Write an equilibrium equation and solubility product expression for Mg(OH)2, and calculate the Ksp.
2) When the aqueous HCl was in the demo described in #2 (above), the solution color changed from purple to red/pink immedietly becuase the solution changed from pH=10 to pH=4. If 30.00 mL of Milk of Magneisa (MOM) is taken as an antacid to neutralize excess 1.50 M HCl (aq) in the stomach, how many mL of acid will be neutralized. The density of MOM is 1.14 g/mL and the solution is 7.26% Mg(OH)2 by mass.
If you know how to solve these plaese show all of your work, thanks!!!
1) During the pH lab, you saw a demonstration in which hydochloric acid was added to a mixure containing ice, water, universal indicator, and Milk of Magnesia (MOM) is a saturated solution of Mg(OH)2, a fairly insoluble base with molar solubility of 1.317x10^-4 M. Write an equilibrium equation and solubility product expression for Mg(OH)2, and calculate the Ksp.
2) When the aqueous HCl was in the demo described in #2 (above), the solution color changed from purple to red/pink immedietly becuase the solution changed from pH=10 to pH=4. If 30.00 mL of Milk of Magneisa (MOM) is taken as an antacid to neutralize excess 1.50 M HCl (aq) in the stomach, how many mL of acid will be neutralized. The density of MOM is 1.14 g/mL and the solution is 7.26% Mg(OH)2 by mass.