1. 0.1 Molar (M) Sodium Hydroxide Solution:
* This refers to a solution where 0.1 moles of sodium hydroxide (NaOH) are dissolved in 1 liter of water.
* This is the most common interpretation.
2. 0.1 Normal (N) Sodium Hydroxide Solution:
* This refers to a solution where 0.1 equivalents of sodium hydroxide are dissolved in 1 liter of water.
* Since NaOH has one hydroxide ion per molecule, 0.1 N NaOH is equivalent to 0.1 M NaOH.
3. 0.1% (w/v) Sodium Hydroxide Solution:
* This refers to a solution where 0.1 grams of sodium hydroxide are dissolved in 100 ml of water.
* This is a much lower concentration than the previous two examples.
To understand the makeup, let's focus on the most common interpretation (0.1 M NaOH solution):
* Sodium Hydroxide (NaOH): The solute, a white solid.
* Water (H2O): The solvent.
Here's how to prepare a 0.1 M NaOH solution:
1. Calculate the mass of NaOH needed:
* Molecular weight of NaOH = 40 g/mol
* 0.1 moles of NaOH = 0.1 mol * 40 g/mol = 4 g
2. Dissolve the NaOH in water:
* Carefully add 4 g of NaOH to a volumetric flask containing about 800 ml of distilled water.
* Stir until the NaOH is completely dissolved.
* Add more distilled water to bring the total volume up to 1 liter.
Important Safety Note:
* Sodium hydroxide is a strong base and corrosive. Wear appropriate safety gear (gloves, goggles, lab coat) when working with it.
* Always add NaOH to water, never the other way around. This prevents a potentially dangerous exothermic reaction.
Let me know if you have any other questions!
