How many total moles of KNO_(3) must be dissolved in water to make 1.5 liters of a 2.0 M solution? square

To find the total moles of $KNO_{3}$ needed to make a 1.5-liter solution with a concentration of 2.0 M, we can use the formula:<br /><br />\[ \text{Molarity (M)} = \frac{\text{moles of solute}}{\text{liters of solution}} \]<br /><br />Given:<br />- Molarity (M) = 2.0 M<br />- Volume (V) = 1.5 liters<br /><br />We need to find the moles of solute (KNO₃).<br /><br />Rearranging the formula to solve for moles of solute:<br /><br />\[ \text{moles of solute} = \text{Molarity (M)} \times \text{Volume (V)} \]<br /><br />Substituting the given values:<br /><br />\[ \text{moles of solute} = 2.0 \, \text{M} \times 1.5 \, \text{L} \]<br /><br />\[ \text{moles of solute} = 3.0 \, \text{moles} \]<br /><br />Therefore, 3.0 moles of $KNO_{3}$ must be dissolved in water to make 1.5 liters of a 2.0 M solution.