Final answer:
After dividing the initial 1.00 M NaCl solution into two equal parts, the molarity remains 1.00 M in both the original and the new beaker because the concentration, which is the ratio of moles to volume, is unchanged.
Step-by-step explanation:
You have asked about the molarity of NaCl solution after splitting it between two beakers. Originally, you have 100 mL of a 1.00 M NaCl solution. Molarity is defined as the number of moles of solute per liter of solution (mol/L). Since molarity is an intensive property, it does not change when you divide the solution into parts as long as no extra solute or solvent is added.
When you take 50 mL of your initial 1.00 M NaCl solution and pour it into another beaker, you are essentially dividing the total number of moles present in the original solution in half, but the volume that they occupy is also halved. Therefore, the concentration of the NaCl remains 1.00 M in both beakers. This is because the number of moles of NaCl remains constant in each portion and the volume is also proportionally reduced.
In terms of calculations, the original solution has 0.100 moles of NaCl (since 1.00 M means 1.00 mol/L and you have 0.100 L or 100 mL). When you take half of that volume (50 mL or 0.050 L), you also take half of the moles, which is 0.050 moles. But since you have also halved the volume, the molarity remains the same:
Number of moles in 50 mL = (1.00 mol/L) × 0.050 L = 0.050 moles
Molarity = Number of moles / Volume (in liters) = 0.050 moles / 0.050 L = 1.00 M
Thus, the molarity of the NaCl solution in each of the two beakers is 1.00 M after you pour 50 mL into another beaker.