Prepare 0.03 mole fraction solution of NaOH in water

Total volume of solution is 100ml

How to prepare?

You want XNaOH = 0.03. Then

0.03 = mols NaOH/[mols NaOH +(mols H2O-mols NaOH)]
If you let y stand for mols NaOH, this becomes
0.03 = y/[y+(100/18)-y]
Solve for y = mols NaOH. Post your work if you get stuck.

To prepare a 0.03 mole fraction solution of NaOH in water with a total volume of 100 ml, you need to calculate the amount of NaOH needed and then add water to achieve the desired final volume.

First, let's understand what a mole fraction is. The mole fraction of a component in a solution is the ratio of the number of moles of that component to the total number of moles of all components in the solution. In this case, we want to calculate the mole fraction of NaOH.

Given that we want a 0.03 mole fraction of NaOH, it means that NaOH accounts for 0.03 moles out of a total of 1 mole of all components in the solution. Therefore, we can say that 0.03 mole fraction of NaOH is equivalent to 0.03 moles of NaOH.

To calculate the amount of NaOH needed, we can use the formula:

Amount (in moles) = Mole fraction x Total moles

In this case, the mole fraction of NaOH is 0.03 and the total moles will be 0.03 moles as well. Therefore, the calculation is as follows:

Amount of NaOH (in moles) = 0.03 mole fraction x 0.03 moles = 0.0009 moles

Since we know the amount of NaOH in moles, we can use its molecular weight to calculate the actual mass needed. The molecular weight of NaOH is approximately 39.997 grams/mole.

Mass of NaOH (in grams) = Amount of NaOH (in moles) x Molecular weight
Mass of NaOH (in grams) = 0.0009 moles x 39.997 grams/mole ≈ 0.036 grams

Therefore, you will need approximately 0.036 grams of NaOH to prepare the desired solution.

Now, to prepare the solution, you need to dissolve the calculated amount of NaOH (approximately 0.036 grams) in water and then add more water to reach the final volume of 100 ml.