What mass of H2SO4 would be required to react with 0.59 mol of NaOH?
To determine the mass of H2SO4 required to react with a specific amount of NaOH, we need to use the balanced chemical equation for the reaction between NaOH and H2SO4:
2NaOH + H2SO4 -> Na2SO4 + 2H2O
First, find the molar ratio of NaOH to H2SO4 from the balanced equation. In this case, the ratio is 2:1 because the coefficient of NaOH is 2, while the coefficient of H2SO4 is 1.
Next, we'll use the molar ratio to convert the given number of moles of NaOH (0.59 mol) to moles of H2SO4:
0.59 mol NaOH × (1 mol H2SO4 / 2 mol NaOH) = 0.295 mol H2SO4
Now we have the number of moles of H2SO4 required to react with 0.59 mol of NaOH.
Finally, we can calculate the mass of H2SO4 by multiplying the number of moles by its molar mass, which you can find from the periodic table. The molar mass of H2SO4 is approximately 98.09 g/mol.
Mass of H2SO4 = 0.295 mol × 98.09 g/mol = 28.89 g
Therefore, approximately 28.89 grams of H2SO4 would be required to react with 0.59 mol of NaOH.
H2SO4 + 2NaOH ==> Na2SO4 + 2H2O
0.59 mol NaOH x (1 mol H2SO4/2 mol NaOH) = ?