How would I make a 0.25M solution of sodium bisulfite?
Weigh a sample of NaHSO3 equal to 0.25 moles (moles = grams/molar mass), place the solid in a 1L volumetric flask, add some water and swirl until all of the solid has dissolved, then make to the mark with distilled water. Mix thoroughly. That will give you 0.25moles in 1 L which is 0.25 M.
Thanks DrBob!!!
To make a 0.25M solution of sodium bisulfite, you need to know the molar mass of sodium bisulfite and the desired volume of the solution. Here's how you can calculate it:
1. Determine the molar mass of sodium bisulfite (NaHSO3).
- Sodium (Na): 22.99 g/mol
- Hydrogen (H): 1.01 g/mol
- Sulfur (S): 32.07 g/mol
- Oxygen (O): 16.00 g/mol (there are 3 oxygen atoms in sodium bisulfite)
Add up the molar masses: 22.99 + 1.01 + 32.07 + (16.00 x 3) = 104.06 g/mol
2. Calculate the number of moles of sodium bisulfite needed:
Moles = Molarity x Volume (in liters)
Moles = 0.25 M x Volume (in liters)
Let's assume you want to make 500 mL (0.5 L) of the solution:
Moles = 0.25 M x 0.5 L = 0.125 mol
3. Calculate the mass of sodium bisulfite needed:
Mass = Moles x Molar mass
Mass = 0.125 mol x 104.06 g/mol
Mass = 13.01 g
Therefore, to make a 0.25M solution of sodium bisulfite, you would need to dissolve 13.01 grams of sodium bisulfite in a sufficient amount of solvent (usually water) to make a final volume of 500 mL.