Step 1: Determine the molar mass of sodium sulfate
The molar mass of Na2SO4 is 142.04 g/mol. This means that 1 mole of Na2SO4 weighs 142.04 grams.
Step 2: Calculate the number of moles of sodium sulfate we need
We are aiming to produce 50 g of Na2SO4. To calculate the number of moles, we divide the mass by the molar mass:
Number of moles of Na2SO4 = 50 g / 142.04 g/mol = 0.352 moles
Step 3: Determine the stoichiometry of the reaction
The balanced chemical equation for the reaction between sodium hydroxide (NaOH) and sulfuric acid (H2SO4) to form sodium sulfate is:
2 NaOH + H2SO4 → Na2SO4 + 2 H2O
This equation tells us that for every 2 moles of NaOH and 1 mole of H2SO4 that react, 1 mole of Na2SO4 is produced.
Step 4: Calculate the moles of NaOH and H2SO4 needed
Using the stoichiometry of the reaction, we can determine the number of moles of NaOH and H2SO4 required to produce 0.352 moles of Na2SO4:
- Moles of NaOH needed = 0.352 moles Na2SO4 * (2 moles NaOH / 1 mole Na2SO4) = 0.704 moles NaOH
- Moles of H2SO4 needed = 0.352 moles Na2SO4 * (1 mole H2SO4 / 1 mole Na2SO4) = 0.352 moles H2SO4
Step 5: Convert moles to grams
Now we can convert the moles of NaOH and H2SO4 back to grams:
- Mass of NaOH needed = 0.704 moles NaOH * 40 g/mol (molar mass of NaOH) = 28.16 grams NaOH
- Mass of H2SO4 needed = 0.352 moles H2SO4 * 98.08 g/mol (molar mass of H2SO4) = 34.54 grams H2SO4
Therefore, to produce 50 grams of sodium sulfate (Na2SO4), you will need approximately 28.16 grams of sodium hydroxide (NaOH) and 34.54 grams of sulfuric acid (H2SO4).
