How would you prepare 50.00 mL of 0.25 Molar NaCl from 2.00 Molar NaCl?
Use the dilution formula
c1v1 = c2v2
c = concn
v = volume
To prepare 50.00 mL of 0.25 Molar NaCl from a 2.00 Molar NaCl solution, you will need to perform a dilution. Dilution is the process of reducing the concentration of a solute in a solution by adding more solvent.
To calculate the amount of the 2.00 Molar NaCl solution required for the dilution, you can use the equation: C1V1 = C2V2, where C1 is the initial concentration, V1 is the initial volume, C2 is the final concentration, and V2 is the final volume.
In this case, C1 = 2.00 Molar, V1 is the unknown volume of the 2.00 Molar NaCl solution, C2 = 0.25 Molar, and V2 = 50.00 mL.
Rearranging the equation, you have V1 = (C2 * V2) / C1:
V1 = (0.25 Molar * 50.00 mL) / 2.00 Molar
V1 = 6.25 mL
Therefore, to prepare 50.00 mL of 0.25 Molar NaCl using a 2.00 Molar NaCl solution, you will need to measure out 6.25 mL of the 2.00 Molar NaCl solution and then add enough solvent (such as water) to reach a final volume of 50.00 mL.