What is the molarity of CaCl_2 when 1.92 mol of CaCl_2 is dissolved in water to form 515 mL of solution?

• A. 2.69 M
• B. 0.269 M
• C. 3.73 M
• D. 0.373 M

Answer: (C)

Verified step by step guidance

1. Identify the given information: the amount of solute (CaCl_2) is 1.92 mol, and the volume of the solution is 515 mL.
2. Convert the volume from milliliters to liters because molarity is expressed in moles per liter. Use the conversion: \$1\, \text{L} = 1000\, \text{mL}\(, so \)V = \frac{515}{1000} = 0.515\, \text{L}$.
3. Recall the formula for molarity, which is the number of moles of solute divided by the volume of the solution in liters: \(M = \frac{\text{moles of solute}}{\text{liters of solution}}\)
4. Substitute the known values into the molarity formula: \(M = \frac{1.92\, \text{mol}}{0.515\, \text{L}}\)
5. Perform the division to find the molarity, which will give the concentration of CaCl_2 in moles per liter.