The balanced chemical equation for the reaction is:
SrCl2(aq) + 2NaF(aq) ⟶ SrF2(s) + 2NaCl(aq)
To find the volume of a 0.550 M NaF solution required to react completely with 675 mL of a 0.680 M SrCl2 solution, we can use the following steps:
1.Calculate the moles of SrCl2 present in 675 mL of a 0.680 M solution:
moles of SrCl2 = (0.680 mol/L) x (0.675 L) = 0.459 mol
2.Use the mole ratio from the balanced chemical equation to calculate the moles of NaF required to react with all of the SrCl2:
moles of NaF = (2 mol NaF / 1 mol SrCl2) x (0.459 mol SrCl2) = 0.918 mol NaF
3.Calculate the volume of a 0.550 M NaF solution required to contain 0.918 moles of NaF:
volume of NaF solution = (0.918 mol) / (0.550 mol/L) = 1.67 L
Therefore, 1.67 L of a 0.550 M NaF solution is required to react completely with 675 mL of a 0.680 M SrCl2 solution.
I hope this helps! Let me know if you have any other questions.