Can you help me? From a 0.5 M #Na_2CO_3# solution having a volume of 300 ml, prepare a 0.075 M #Na_2CO_3# solution with a volume of 150 ml.
You'd take 22.5 mL of your stock solution and add enough water to get the volume to 150 mL.
This time you're dealing with a classic dilution problem.
The idea behind dilution problems is that the number of moles of solute, which in your case is sodium carbonate, must remain constant after the initial solution is diluted.
Dilutions imply that the number of moles of solute remain constant, but that the total volume of the solution increases. This will cause the solution's molarity to decrease.
So, start by figuring out how many moles of sodium carbonate your target solution must contain.
This means that the sample you take from the stock solution must contain the exact same number of moles of sodium carbonate.
Knowing the molarity of the stock solution, the volume you'd need is
This is equivalent to
This means that if you take 22.5 mL of your stock solution, and add enough water to make the volume out to 150 mL, you'll get your target solution.
The volume of water needed is