Sure, let's go through the solution step by step.
### Step 1: Calculate the volume of the solution in liters.
First, we need to convert the given volume from milliliters (mL) to liters (L) because molarity is expressed in moles per liter (mol/L).
Given:
- Volume of the solution = 450 mL
To convert from mL to L, we use the conversion factor [tex]\(1 \text{ L} = 1000 \text{ mL}\)[/tex]:
[tex]\[ \text{Volume in liters} = \frac{450 \text{ mL}}{1000} = 0.45 \text{ L} \][/tex]
### Step 2: Calculate the number of moles of FeCl_2 in the solution.
We are given the mass of FeCl_2 and its molar mass. The molar mass tells us how many grams constitute one mole of FeCl_2.
Given:
- Mass of FeCl_2 = 225 g
- Molar mass of FeCl_2 = 126.75 g/mol
To find the number of moles, we use the formula:
[tex]\[ \text{Number of moles} = \frac{\text{Mass}}{\text{Molar mass}} \][/tex]
So the number of moles of FeCl_2 is:
[tex]\[ \text{Number of moles of FeCl}_2 = \frac{225 \text{ g}}{126.75 \text{ g/mol}} \approx 1.775 \text{ moles} \][/tex]
### Step 3: Calculate the molarity of the solution.
Molarity (M) is defined as the number of moles of solute per liter of solution.
From the previous steps, we have:
- Number of moles of FeCl_2 = 1.775 moles
- Volume of the solution in liters = 0.45 L
Using the formula for molarity:
[tex]\[ \text{Molarity} = \frac{\text{Number of moles}}{\text{Volume in liters}} \][/tex]
[tex]\[ \text{Molarity} = \frac{1.775 \text{ moles}}{0.45 \text{ L}} \approx 3.945 \text{ M} \][/tex]
### Summary of Results:
- Volume of the solution: [tex]\(0.45\)[/tex] L
- Number of moles of FeCl_2: [tex]\(1.775\)[/tex] moles
- Molarity of the solution: [tex]\(3.945\)[/tex] M
So, the molar concentration of the FeCl_2 solution is approximately [tex]\(3.945\)[/tex] M, and the solution contains approximately [tex]\(1.775\)[/tex] moles of FeCl_2.
