# Problem: 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.

###### FREE Expert Solution

For this problem, we're asked to a) Balance the equation for the complete neutralization of Mg(OH)2 with H3POand b) Calculate the mass in g of Mg3(PO4)2 formed in this reaction

We need to do the following steps:

Step 1: Write 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 H3PO(using molarity and the given volume)

Step 3: Based on the balanced chemical equationdo a mole-to-mole comparisonto 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

97% (303 ratings) ###### Problem Details

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.