If 211 mL of water is added to 5.00 mL of 3.24 M NaCl solution, what is the concentration of the new solution? ___ M Your answer should be rounded to two significant figures. Do not include units in your answer.

To solve this problem, we need to understand that the number of moles of NaCl will remain constant before and after the addition of water.

1. First, we calculate the initial number of moles of NaCl in the 5.00 mL solution. We use the formula: moles = Molarity * Volume(L). The volume should be in liters, so we convert 5.00 mL to 0.00500 L.

   moles of NaCl = 3.24 M * 0.00500 L = 0.0162 moles

2. Then, we add 211 mL of water to the solution, which increases the total volume of the solution. We add the initial volume of the NaCl solution (5.00 mL) to the volume of water added (211 mL) to get the total volume.

   Total volume = 5.00 mL + 211 mL = 216 mL = 0.216 L

3. Finally, we calculate the new molarity (concentration) of the solution using the formula: Molarity = moles / Volume(L).

   New Molarity = 0.0162 moles / 0.216 L = 0.075 M

So, the concentration of the new solution is 0.075 M.

Rounded to two significant figures, the answer is 0.075.