Answer:
a. To calculate the number of moles of iron(Il) chloride in the given solution, we can use the formula:
moles = concentration (in M) x volume (in L)
First, we need to convert the given volume of 50.0 mL to liters by dividing it by 1000:
50.0 mL ÷ 1000 = 0.050 L
Now, we can plug in the values into the formula:
moles = 0.911 M x 0.050 L
moles = 0.0456
b. Solving for the final concentration, we get:
final concentration = (initial concentration x initial volume) / final volume
final concentration = (0.911 M x 0.0500 L) / 0.250 L
final concentration = 0.182 M
Now that we know the final concentration of the solution, we can use the same formula as before to calculate the number of moles of iron(II) chloride in the diluted solution:
moles = 0.182 M x 0.250 L
moles = 0.0455 mol
c. First, let's calculate the moles of iron(II) chloride in the initial 50.0 mL sample:
moles = concentration x volume (in liters)
moles = 0.911 mol/L x 0.050 L
moles = 0.0456 mol
Next, let's calculate the liters of solution in the final mixture:
liters = 100.0 mL / 1000 mL/L
liters = 0.100 L
Now we can use these values to calculate the molarity of the iron(II) chloride in the final solution:
Molarity = moles / liters
Molarity = 0.0456 mol / 0.100 L
The molarity of iron(II) chloride in the final solution is 0.456 M.