a neutralization reaction, 50.00 mL of 0.8190 M phosphoric acid reacts with 2.485 g of magnesium hydroxide producing magnesium phosphate and water. How much of the excess reactant remains after the limiting reactant is completely consumed?
In a neutralization reaction, 50.00 mL of 0.8190 M phosphoric acid reacts with 2.485 g of magnesium hydroxide producing magnesium phosphate and water.
How much of the excess reactant remains after the limiting reactant is completely consumed?
Given : molarity of H3PO4 = 0.8190 M
Volume of solution = 50 ml
Mass of Mg(OH) 2 = 2.485 gram
To find : remaining mass of excess reactant.
Solution. As we know that, in a reaction A reactant which has less number of moles will be a limitting reactant and while a reactant which has more number of moles compare to another reactant that will be excess reactant.
And the molarity is the ratio of number of moles of solute and volume of solution.
While mole Is the ratio of mass of substance and molar mass of that substance.
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