the density of a certain aqueous solution is 1.17g/ml, and the solution is 3.57% by mass NaOH. how many mL of this solution would you need to use in order to prepare 100.0 mL of .150 M NaOH solution?
Convert percent NaOH to molarity of the NaOH solution, then use M x mL = M x mL.
For a 3.57% solution, you will have 3.57 g NaOH in 100 grams solution. g/molar mass = moles NaOH and use density to convert 100 g solution to volume, then M = moles/L.
To solve this problem, we need to know the relationship between the concentration of a solution and the amount of solute and solvent used.
First, let's calculate the mass of the NaOH in the .150 M NaOH solution. The molar mass of NaOH is 22.99 g/mol + 16.00 g/mol + 1.01 g/mol = 40.00 g/mol (approx).
We can use the formula:
mass (g) = volume (L) × concentration (mol/L) × molar mass (g/mol)
Rearranging the formula, we get:
volume (L) = mass (g) / (concentration (mol/L) × molar mass (g/mol))
We want to prepare a 100.0 mL solution with a concentration of .150 M NaOH. Let's calculate the mass of NaOH required:
mass (g) = volume (L) × concentration (mol/L) × molar mass (g/mol)
mass (g) = 0.100 L × 0.150 mol/L × 40.00 g/mol
Now, let's calculate the mass of the solution we need to use to obtain this amount of NaOH. We know that the solution is 3.57% NaOH by mass and has a density of 1.17 g/mL.
mass of solution (g) = mass of NaOH (g) / (% NaOH by mass)
mass of solution (g) = (0.100 L × 0.150 mol/L × 40.00 g/mol) / 0.0357
Finally, let's calculate the volume of the solution in mL:
volume of solution (mL) = mass of solution (g) / density of solution (g/mL)
volume of solution (mL) = [(0.100 L × 0.150 mol/L × 40.00 g/mol) / 0.0357] / 1.17
Now, you can calculate the final answer by plugging in the numbers into the formula.