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What volume of 0.140 M Na₃PO₄ solution is necessary to completely react with 94.2 mL of 0.108 M CuCl₂? Express your answer in milliliters to three significant figures.

A. 97.8 mL
B. 105 mL
C. 85.6 mL
D. 102 mL

Answer :

Final answer:

The volume of 0.140 M Na3PO4 necessary to react with 94.2 mL of 0.108 M CuCl2 can be calculated using stoichiometry, which yields a volume of 72.685 mL, not matching the provided options.

Explanation:

The student's question involves the calculation of volume necessary for a stoichiometric reaction between Na3PO4 and CuCl2 in a solution. To find the volume of 0.140 M Na3PO4 solution required to react with 94.2 mL of 0.108 M CuCl2, we must use the concept of molarity and stoichiometry. Assuming a balanced chemical reaction where one mole of CuCl2 reacts with one mole of Na3PO4, we can use the following steps:

  1. Calculate the moles of CuCl2 using its volume and molarity.
  2. Use the mole ratio from the balanced chemical equation to determine the moles of Na3PO4 needed.
  3. Calculate the volume of Na3PO4 solution using the required moles and its molarity.

To answer the question, we need to perform these calculations:

  1. Moles of CuCl2 = 94.2 mL x 0.108 M x (1 L/1000 mL) = 0.010176 moles
  2. Moles of Na3PO4 needed = 0.010176 moles (1:1 ratio)
  3. Volume of Na3PO4 = Moles of Na3PO4 / Molarity of Na3PO4 = 0.010176 moles / 0.140 M = 0.072685 L

Converting liters to milliliters, we get:

Volume of Na3PO4 solution = 0.072685 L x 1000 mL/L = 72.685 mL

However, this volume does not match any of the options provided (a) 97.8 mL (b) 105 mL (c) 85.6 mL (d) 102 mL, indicating a possible error in the question or the provided options.

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