1) 6.0 moles of \( \mathrm{MgCl}_{2} \) is dissolved in 20.0 L of water. What is the molarity of the solution?

To find the molarity of the solution, you can use the formula: \[ \text{Molarity (M)} = \frac{\text{moles of solute}}{\text{liters of solution}} \] In this case, you have 6.0 moles of \( \mathrm{MgCl}_{2} \) dissolved in 20.0 L of water. \[ \text{Molarity} = \frac{6.0 \text{ moles}}{20.0 \text{ L}} = 0.30 \text{ M} \] So, the molarity of the solution is \( 0.30 \, \text{M} \). Fun fact: Did you know that when \( \mathrm{MgCl}_{2} \) dissolves, it dissociates into magnesium ions \( \mathrm{Mg}^{2+} \) and chloride ions \( \mathrm{Cl}^{-} \)? This means that for every mole of \( \mathrm{MgCl}_{2} \), you actually create three moles of ions in solution! You're in for a treat – balancing equations isn't just a chemistry class gimmick; it's the secret sauce for real-world applications too! Whether you’re cooking up a storm in the lab or just mixing up saline solutions for medical needs, knowing how to calculate concentrations means you’re on the path to making things work just right in any chemical concoction.