When iron (III) hydroxide is mixed with phosphoric acid, iron (II) phosphate precipitate results. Using the equation: Fe(OH)2 (aq) + H3PO4 (aq) → Fe3(PO4)2 (s) + H2O (l) If 3.70g of Fe(OH)2 is treated with 4.75g of phosphoric acid. a. How many grams of Fe3(PO4)2 precipitate can be formed? b. What is the limiting reagent? c. How much of the reactant in excess remains affter the reaction? d. If 3.75g of Fe3(PO4)2 is actually obtained, what is the percent yield?
When iron (III) hydroxide is mixed with phosphoric acid, iron (II) phosphate precipitate results. Using the equation: Fe(OH)2 (aq) + H3PO4 (aq) → Fe3(PO4)2 (s) + H2O (l) If 3.70g of Fe(OH)2 is treated with 4.75g of phosphoric acid. a. How many grams of Fe3(PO4)2 precipitate can be formed? b. What is the limiting reagent? c. How much of the reactant in excess remains affter the reaction? d. If 3.75g of Fe3(PO4)2 is actually obtained, what is the percent yield?
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Chapter4: Chemical Reactions
Section: Chapter Questions
Problem 4.155QP: Phosphoric acid is prepared by dissolving phosphorus(V) oxide, P4O10, in water. What is the balanced...
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When iron (III) hydroxide is mixed with phosphoric acid, iron (II) phosphate precipitate results. Using the equation: Fe(OH)2 (aq) + H3PO4 (aq) → Fe3(PO4)2 (s) + H2O (l)
If 3.70g of Fe(OH)2 is treated with 4.75g of phosphoric acid.
a. How many grams of Fe3(PO4)2 precipitate can be formed?
b. What is the limiting reagent?
c. How much of the reactant in excess remains affter the reaction?
d. If 3.75g of Fe3(PO4)2 is actually obtained, what is the percent yield?
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