For this problem, we're asked to a) Balance the equation for the complete neutralization of Mg(OH)2 with H3PO4 and b) Calculate the mass in g of Mg3(PO4)2 formed in this reaction
We need to do the following steps:
Step 1: Write a balanced chemical equation for the reaction.
Step 2: Calculate the # of moles for Mg(OH)2 (mass to mole using molar mass) and # of moles for H3PO4 (using molarity and the given volume)
Step 3: Based on the balanced chemical equation, do a mole-to-mole comparison, to determine the limiting reactant
Recall that the limiting reactant or limiting reagent is the compound that determines the maximum amount of product obtained in a chemical reaction.
The limiting reactant is the one that shows a smaller product yield (or smaller # of moles), while the excess reactant is that one that shows a greater product yield.
Step 4: Calculate the mass in g (mole to mass using its molar mass) of Mg3(PO4)2 formed from the moles of the limiting reactant
Consider 5.83g of Mg(OH)2 (s) reacted with 500.ml of 0.100M H 3PO4 .
a) Balance the equation for complete neutralization.
b) Calculate how many grams of Mg 3(PO4)2 are formed in this reaction.
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What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Solution Stoichiometry concept. You can view video lessons to learn Solution Stoichiometry. Or if you need more Solution Stoichiometry practice, you can also practice Solution Stoichiometry practice problems.