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:
- Calculate the moles of CuCl2 using its volume and molarity.
- Use the mole ratio from the balanced chemical equation to determine the moles of Na3PO4 needed.
- Calculate the volume of Na3PO4 solution using the required moles and its molarity.
To answer the question, we need to perform these calculations:
- Moles of CuCl2 = 94.2 mL x 0.108 M x (1 L/1000 mL) = 0.010176 moles
- Moles of Na3PO4 needed = 0.010176 moles (1:1 ratio)
- 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.