Given a 1.00 M solution of NaOH, describe how you would prepare 500 mL of 0.05 M NaOH solution. You have a 500 mL volumetric flask and a graduated cylinder.
I have been trying to figure this question out for over an hour now. I cant seem to place the given numbers into any equation in the text, and I was home sick from school but still have to take this take home test. Please help me.
Use the dilution formula.
To prepare a 500 mL solution of 0.05 M NaOH from a 1.00 M NaOH solution, you need to dilute the original solution by adding water.
Here's how you can do it step by step:
1. Determine the volume of the original 1.00 M NaOH solution needed to make the desired 0.05 M NaOH solution. We can use the formula:
C1V1 = C2V2
Where:
C1 = concentration of the original solution (1.00 M)
V1 = volume of the original solution needed
C2 = desired concentration (0.05 M)
V2 = final volume of the solution (500 mL)
Rearranging the formula, we get:
V1 = (C2 * V2) / C1
V1 = (0.05 M * 500 mL) / 1.00 M
V1 = 2.5 mL
So, you need 2.5 mL of the 1.00 M NaOH solution.
2. Take the graduated cylinder and measure 2.5 mL of the 1.00 M NaOH solution.
3. Transfer that 2.5 mL of the 1.00 M NaOH solution into the 500 mL volumetric flask.
4. Fill the volumetric flask with water until it reaches the calibration mark (500 mL).
5. Carefully mix the solution by swirling the flask gently until the NaOH is completely dissolved in water.
Now, you have prepared a 500 mL solution of 0.05 M NaOH.
Note: It is important to be accurate and precise when measuring the volume of the 1.00 M NaOH solution using the graduated cylinder. Additionally, ensure thorough mixing of the solution in the volumetric flask to attain a homogenous mixture.