Specialized cells in the stomach release HCl to aid digestion. If 
they release too much, the excess can be neutralized with 
antacids. A common antacid contains magnesium hydroxide, 
Mg(OH)2, which reacts with the acid to form water and magnesium 
chloride solution. As a government chemist testing commercial 
antacids, you use 0.10 M HCl to simulate the acid concentration in 
the stomach. How many liters of “stomach acid” react with a tablet 
containing 0.10 g of magnesium hydroxide?

Every antacid contains one or more ingredients capable of reactingwith excess stomach acid (HCl). The essential neutralizationproducts are CO2 and/or H2O. Write NET IONIC EQUATIONS to representthe neutralizing action of the following popular antacids. IDENTIFYALL PHASES of the answer

1. Milk of magnesia (magnesium hydroxide)
2. Maalox (magnesium hydroxide, aluminum hydroxide)
3. Rolaids [NaAl(OH)2CO3]

Milk of Magnesia is a suspension of magnesium hydroxide in water. Acommon medicine, it is often used as an antacid because itneutralizes hydrochloric acid in the stomach:
Mg(OH)2(s) + 2 HCl(aq) ? Mg2+(aq) + 2 H2O(l)
Calculate the mass of HCl that is neutralized by 2 g of Mg(OH)2(s)