What is the mass in grams of sodium sulfate would you weigh to prepare to a 100mL solution of 0.2 M NaHSO4 ?(molar mass=120 g/mole)
(100 mL / 1000 mL) * 0 .2 = 0.02 mol needed
0.02 mol * (120 g / mol) = ?
Note to Cj and Damon.
You can't make a solution of NaHSO4 by weighing out Na2SO4 and dropping it into water.
To calculate the mass of sodium sulfate (Na2SO4) needed to prepare a 100 mL solution of 0.2 M NaHSO4, you need to follow these steps:
Step 1: Determine the molar mass of Na2SO4.
The molar mass of Na2SO4 is given as 120 g/mol.
Step 2: Calculate the number of moles of NaHSO4 required.
To do this, use the equation: moles = molarity x volume.
moles = 0.2 mol/L x 0.1 L (100 mL = 0.1 L)
moles = 0.02 moles
Step 3: Use the stoichiometry of Na2SO4 and NaHSO4 to find the mass of Na2SO4.
From the balanced equation:
2 NaHSO4 → Na2SO4 + H2SO4
we see that the stoichiometric ratio of NaHSO4 to Na2SO4 is 2:1.
This means that for every 2 moles of NaHSO4, we will have 1 mole of Na2SO4.
Since we have 0.02 moles of NaHSO4 (as calculated in Step 2), we divide it by 2 to get the moles of Na2SO4 needed:
moles of Na2SO4 = 0.02 moles / 2 = 0.01 moles
Step 4: Calculate the mass of Na2SO4.
To find the mass, we multiply the moles of Na2SO4 by its molar mass:
mass = moles x molar mass
mass = 0.01 moles x 120 g/mol = 1.2 grams
Therefore, to prepare a 100 mL solution of 0.2 M NaHSO4, you would need to weigh 1.2 grams of sodium sulfate (Na2SO4).