Describe how you would prepare 25.0ml of a 1.00 M NaOH solution.
To prepare 25.0 ml of a 1.00 M NaOH solution, you will need to follow a step-by-step procedure. Here's how you can do it:
Step 1: Calculate the amount of NaOH required.
Since you want to prepare a 1.00 M solution, it means you need 1.00 mole of NaOH per liter (1000 ml) of solution. Therefore, for 25.0 ml, you will need 1/40th of that amount (since 25 ml is 1/40th of 1000 ml), which is 0.025 moles.
Step 2: Determine the molar mass of NaOH.
The molar mass of NaOH can be calculated by adding the atomic masses of the individual elements:
Sodium (Na) = 22.99 g/mol
Oxygen (O) = 16.00 g/mol
Hydrogen (H) = 1.01 g/mol
So, the molar mass of NaOH is 22.99 g/mol + 16.00 g/mol + 1.01 g/mol = 39.99 g/mol.
Step 3: Calculate the mass of NaOH required.
To calculate the mass, you multiply the number of moles by the molar mass:
Mass = Moles × Molar mass = 0.025 moles × 39.99 g/mol = 0.99975 grams.
Step 4: Dissolve the calculated mass of NaOH in a solvent.
Carefully weigh 0.99975 grams of NaOH using a balance, and add it to a container. The container should have enough volume to accommodate the final solution volume.
Step 5: Add distilled water and mix.
Add distilled water to the container and mix well until the NaOH is completely dissolved. Continue adding water until the final volume reaches 25.0 ml. Make sure to stir the solution thoroughly so that the NaOH is evenly distributed.
Step 6: Adjust the final volume and concentration (if needed).
Use a graduated cylinder or pipette to measure the final volume accurately. If the volume is slightly off, you can add more distilled water to adjust it precisely to 25.0 ml. Then, verify the concentration of NaOH using a suitable analytical method, like titration, to ensure it is 1.00 M.
Remember to take proper safety precautions, such as wearing protective gloves and goggles, as NaOH is caustic and can cause burns.