To produce 3.00 L of a 1.9 M solution of NaOH, how many grams of NaOH must be dissolved?
To determine how many grams of NaOH must be dissolved to produce a 1.9 M solution in 3.00 L of solution, we need to use the formula:
Molarity (M) = moles of solute / liters of solution
First, we need to find the moles of NaOH required. Rearranging the formula, we have:
moles of solute = Molarity × liters of solution
Substituting the given values into the formula:
moles of NaOH = 1.9 M × 3.00 L
Next, we need to convert the moles of NaOH to grams using its molar mass. The molar mass of NaOH is the sum of the atomic masses of sodium (Na), oxygen (O), and hydrogen (H). The atomic masses are:
- Na: 22.99 g/mol
- O: 16.00 g/mol
- H: 1.01 g/mol
The molecular formula of NaOH has one sodium atom, one oxygen atom, and one hydrogen atom. Therefore, the molar mass of NaOH is:
molar mass of NaOH = (1 × atomic mass of Na) + (1 × atomic mass of O) + (1 × atomic mass of H)
Substituting the atomic masses:
molar mass of NaOH = (1 × 22.99 g/mol) + (1 × 16.00 g/mol) + (1 × 1.01 g/mol)
Now, we can calculate the grams of NaOH required using the moles of NaOH and the molar mass:
grams of NaOH = moles of NaOH × molar mass of NaOH
By substituting the previously calculated values, we get the grams of NaOH needed to dissolve in order to produce the desired solution.
How many mols do you want? That is M x L = mols.
Then mol = grams/molar mass.