To determine the molarity of the solution, we need to follow these steps:
1. Determine the number of moles of \( KCl \) present:
The formula to compute moles is:
[tex]\[
\text{moles of KCl} = \frac{\text{mass of KCl}}{\text{molar mass of KCl}}
\][/tex]
Given:
- Mass of \( KCl \) = 8.45 g
- Molar mass of \( KCl \) = 74.55 g/mol
Plugging in the values:
[tex]\[
\text{moles of KCl} = \frac{8.45 \text{ g}}{74.55 \text{ g/mol}} \approx 0.1133 \text{ moles}
\][/tex]
2. Calculate the molarity of the solution:
Molarity (\( M \)) is defined as:
[tex]\[
M = \frac{\text{moles of solute}}{\text{liters of solution}}
\][/tex]
Given:
- Moles of \( KCl \) \(\approx 0.1133 \text{ moles}\)
- Volume of the solution = 0.750 L
Using the formula for molarity:
[tex]\[
M = \frac{0.1133 \text{ moles}}{0.750 \text{ liters}} \approx 0.1511 \text{ M}
\][/tex]
So, the calculated molarity of the \( KCl \) solution is approximately 0.151 M.
Hence, the correct answer is:
[tex]\[
0.151 \text{ M}
\][/tex]
