How many liters of concentrated 18 M HCl is needed to prepare 225 L of a .66 M solution? 75 L 8.3 L 0.23 L 1.5 L

## Step 1<br />The problem involves the concept of molarity and dilution in chemistry. Molarity (M) is a measure of the concentration of a solute in a solution, defined as the number of moles of solute per liter of solution.<br /><br />## Step 2<br />The formula for dilution is given by \(M_1V_1 = M_2V_2\), where \(M_1\) and \(V_1\) are the molarity and volume of the concentrated solution, and \(M_2\) and \(V_2\) are the molarity and volume of the diluted solution.<br /><br />## Step 3<br />In this problem, we are given:<br />- \(M_1 = 18\) M (concentration of the concentrated HCl solution)<br />- \(M_2 = 0.66\) M (desired concentration of the diluted HCl solution)<br />- \(V_2 = 225\) L (volume of the diluted HCl solution)<br /><br />## Step 4<br />We need to find \(V_1\), the volume of the concentrated HCl solution needed.<br /><br />## Step 5<br />Using the dilution formula, we rearrange to solve for \(V_1\):<br />### \(V_1 = \frac{M_2 \times V_2}{M_1}\)<br /><br />## Step 6<br />Substituting the given values:<br />### \(V_1 = \frac{0.66 \times 225}{18}\)<br /><br />## Step 7<br />Calculating this gives us the volume of the concentrated HCl solution needed to prepare 225 L of a 0.66 M solution.