1. The problem statement, all variables and given/known data A sample of 5.53g of Mg(OH)2 is added to 25.0mL of 0.200M HNO3. How many moles of Mg(OH)2, HNO3, and Mg(NO3)2 are present after the reaction is complete? 2. Relevant equations M = mol/L 3. The attempt at a solution The balanced equation for the reaction is Mg(OH)2 + 2HNO3 -> Mg(NO3)2 + 2H2O The limiter in this case would be HNO3 and I found that in 0.025L of this solution there is 0.315g of HNO3. What I'm not sure is how to find the moles of each after the reaction is complete. I assume it's with stoichiometry, but I'm not sure how to find the moles of each at the end. I know that there should be 0 moles of HNO3 because it's used up correct? As for the Mg(OH)2, am I suppose to subtract the grams of HNO3 from the 5.53g of Mg(OH)2?