$. . . {N a}_{3} {P O}_{4} (a q) + . . . {M g ({N O}_{3})}_{2} (a q) \to . . . {{M g}_{3} ({P O}_{4})}_{2} (s) + . . . N a {N O}_{3} (a q)$
Equal volumes of 0.10 M sodium phosphate and 0.10 M magnesium nitrate are mixed in a container according to the above unbalanced reaction equation. Which of the following statements is true regarding the reaction?

When the reaction is complete, the concentrations of both magnesium and phosphate are essentially 0.

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Magnesium nitrate is the limiting reactant.

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Sodium phosphate is the limiting reactant.

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Since nitrate ion is a spectator ion, the concentration of nitrate ion in the final solution will be the same as in the original magnesium nitrate solution.

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{N a}_{3} {P O}_{4}

and

{M g ({N O}_{3})}_{2}

react in a 1:1 ratio.

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Solution

The correct option is A Magnesium nitrate is the limiting reactant.
The unbalanced chemical reaction is
${N a}_{3} {P O}_{4} (a q) + {M g ({N O}_{3})}_{2} (a q) \to {{M g}_{3} ({P O}_{4})}_{2} (s) + N a {N O}_{3} (a q)$
The balanced chemical equation is
$2 {N a}_{3} {P O}_{4} (a q) + 3 {M g ({N O}_{3})}_{2} (a q) \to {{M g}_{3} ({P O}_{4})}_{2} (s) + 6 N a {N O}_{3} (a q)$
Equal volumes of 0.10 M sodium phosphate and 0.10 M magnesium nitrate are mixed in a container. This corresponds to equal number of moles of both species.
From the balanced chemical equation, we can see that 3 moles of magnesium nitrate reacts with 2 moles of sodium phosphate. However only 2 moles of magnesium nitrate will be present for 2 moles of sodium phosphate.
Hence, Magnesium nitrate is the limiting reactant and sodium phosphate is the excess reactant.

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Similar questions

. . . {N a}_{3} {P O}_{4} (a q) + . . . {M g ({N O}_{3})}_{2} (a q) \to . . . {{M g}_{3} ({P O}_{4})}_{2} (s) + . . . N a {N O}_{3} (a q)

Equal volume of 0.10 M sodium phosphate and 0.10 M magnesium nitrate are mixed in a container according to the above unbalanced reaction equation. After the completion of the reaction, what is the concentration of sodium ions in the solution?

{N a}_{3} {P O}_{4} (a q) + {M g ({N O}_{3})}_{2} (a q) \to

{{M g}_{3} ({P O}_{4})}_{2} (s) + N a {N O}_{3} (a q)

Equal volumes of 0.10 M sodium phosphate and 0.10 M magnesium nitrate are mixed according to the unbalanced reaction equation above. Which of the following statements is true regarding the reaction?

Q. Equal volumes of

0.1

{A g N O}_{3}

and

0.2

N a C l

solutions are mixed. The concentration of nitrate ion in the resultant mixture will be:

Equal volumes of 0.1M $A g N O_{3}$ and 0.2 M NaCl are mixed together. The concentration of nitrate ions in the resulting mixture is:

Q. A small piece of silver is placed in a solution containing both magnesium nitrate and copper (II) nitrate. Which one of the following occurs?

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...Na3PO4(aq)+...Mg(NO3)2(aq)→...Mg3(PO4)2(s)+...NaNO3(aq)Equal volumes of 0.10 M sodium phosphate and 0.10 M magnesium nitrate are mixed in a container according to the above unbalanced reaction equation. Which of the following statements is true regarding the reaction?