0.6 N = 0.6 M, as the equivalence of N (Normality) is equal to the equivalence of M (Molarity) for NaOH (a monoprotic base)

Step 2: Calculate the Amount of NaOH Needed

To prepare a 0.6 M NaOH solution, you will need 0.6 moles of NaOH per liter of solution. The formula for calculating the amount of solute (NaOH) required is:

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Moles of NaOH = Molarity x Volume of Solution in Liters

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For 1 Liter of 0.6 M NaOH solution:

Moles of NaOH = 0.6 M x 1 L = 0.6 moles

Step 3: Weigh the NaOH

Using an analytical balance, accurately weigh out 0.6 moles of NaOH. The molecular weight of NaOH is approximately 40 g/mol. Therefore, you will need:

0.6 moles NaOH x 40 g/mol = 24 grams NaOH

Step 4: Dissolve NaOH in Water

In a clean beaker, add a small amount of distilled water to dissolve the NaOH. Stir or mix until the NaOH is fully dissolved.

Step 5: Transfer to a Volumetric Flask

Quantitatively transfer the dissolved NaOH solution to a 1-liter volumetric flask. Use a funnel to avoid spilling.

Step 6: Add More Distilled Water

Fill the volumetric flask with distilled water up to the calibration mark. Swirl gently to ensure uniform mixing.

Step 7: Obtain a Well-Mixed Solution

By following the above steps, you have prepared 1 liter of 0.6 M NaOH solution. Mix thoroughly to ensure the solution is well-mixed and uniform.

Note: Be cautious when handling NaOH as it is a corrosive substance. Always wear gloves and safety goggles to prevent any potential accidents.