Given the reaction: H2SO4 = 2NaOH -> NaSO4 = 2H20.
Determine the # of moles of sulfuric acid id needed to completely react with 2.3 L of 0.5 M of NaOH. Then determine the concentration of the solution if 3.0 L of it are used instead.
4.5
To determine the number of moles of sulfuric acid (H2SO4) needed to completely react with 2.3 L of 0.5 M NaOH, we need to use the balanced equation:
H2SO4 + 2NaOH -> Na2SO4 + 2H2O
We can see that the stoichiometry between H2SO4 and NaOH is 1:2. This means that for every 1 mole of H2SO4, we need 2 moles of NaOH.
First, let's calculate the moles of NaOH present in 2.3 L of 0.5 M solution:
Moles of NaOH = Volume (L) x Concentration (M)
Moles of NaOH = 2.3 L x 0.5 M
Moles of NaOH = 1.15 mol
Since the stoichiometry is 1:2, we need twice the number of moles of H2SO4:
Moles of H2SO4 = 2 x Moles of NaOH
Moles of H2SO4 = 2 x 1.15 mol
Moles of H2SO4 = 2.3 mol
Therefore, 2.3 moles of sulfuric acid are needed to completely react with 2.3 L of 0.5 M NaOH.
Now, let's determine the concentration of the solution if 3.0 L of it are used instead:
Moles of NaOH = Volume (L) x Concentration (M)
Moles of NaOH = 3.0 L x 0.5 M
Moles of NaOH = 1.5 mol
Again, since the stoichiometry is 1:2, we need twice the number of moles of H2SO4:
Moles of H2SO4 = 2 x Moles of NaOH
Moles of H2SO4 = 2 x 1.5 mol
Moles of H2SO4 = 3.0 mol
To determine the concentration, we use the formula:
Concentration (M) = Moles / Volume (L)
Concentration of the solution = 3.0 mol / 3.0 L
Concentration of the solution = 1.0 M
Therefore, the concentration of the solution is 1.0 M when 3.0 L of it are used.