Final answer:
To calculate the molarity of the resulting NaF solution after dilution, we use the molar mass of NaF to convert the given mass to moles, calculate the initial molarity, then apply the dilution equation. After dilution, the molarity of the NaF solution is 1.075 M.
Step-by-step explanation:
The molarity of a solution can be calculated using the formula: molarity = moles of solute / liters of solution. To find the molarity of the resulting solution after dilution, we can follow these steps. Initially, we have 125.6 g of NaF in 1 L of solution.
First, convert the mass of NaF to moles by using the molar mass of NaF (Na = 22.99 g/mol + F = 19.00 g/mol,
NaF = 41.99 g/mol).
The calculation is 125.6 g NaF x (1 mol NaF / 41.99 g NaF)= 2.991 moles.
Then, the initial molarity (Mi) is 2.991 moles in 1 L which is 2.991 M.
Next, we consider the dilution process. When 180. mL (0.180 L) of the initial solution is diluted to 500 mL (0.500 L), the number of moles of NaF does not change, since only the volume changes. Using the dilution equation (Mi x Vi = Mf x Vf), where Mf is the final molarity and Vf is the final volume, we have 2.991 M * 0.180 L = Mf * 0.500 L.
Therefore, the final molarity (Mf) is (2.991 M * 0.180 L) / 0.500 L = 1.075 M.