1. Magnesium hydroxide, the active ingredient in milk of magnesia, neutralizes stomach acid, primarily HCl, according to the following reaction: Mg(OH)2(aq) + 2 HCl(aq) ---> 2 H2O(l) + MgCl2(aq) What mass of HCl, in grams, can be neutralized by a dose of milk of magnesia caontaining 3.26g Mg(OH)2? 2. Mass A --> Amount A(in moles) --> Amount B(in moles) --> Mass B 3. The attempt at a solution: 3.26g Mg(OH)2 X 1mol Mg(OH)2 /34.01g Mg(OH)2 X 2 mol HCl/ 1 mol Mg(OH)2 X 36.46g HCl/ 1 molg HCl = 6.99 which is wrong, like I thought it would be. whats the right way to do this?