If a chemist titrates 300.0 mL of H2SO4 with a 3.0 M solution of NaOH and requires only 3.4 mL of the base to reach the endpoint, what is the concentration of the sulfuric acid?
See your post above. I worked that earlier.
To find the concentration of sulfuric acid, we need to use the balanced chemical equation for the reaction between sulfuric acid (H2SO4) and sodium hydroxide (NaOH):
H2SO4 + 2NaOH -> Na2SO4 + 2H2O
By looking at the equation, we can see that one mole of sulfuric acid reacts with two moles of sodium hydroxide.
First, let's calculate the number of moles of NaOH used in the reaction.
Moles of NaOH = Volume of NaOH solution (in L) x Concentration of NaOH (in mol/L)
Moles of NaOH = 3.4 mL ÷ 1000 (to convert mL to L) x 3.0 M
Next, since the reaction ratio is 1:2 for H2SO4:NaOH, the moles of sulfuric acid can be calculated:
Moles of H2SO4 = (Moles of NaOH) ÷ 2
Now, we need to find the concentration of sulfuric acid in Molarity (M).
Concentration of H2SO4 (in M) = Moles of H2SO4 ÷ Volume of H2SO4 (in L)
Volume of H2SO4 = 300.0 mL ÷ 1000 (to convert mL to L)
By plugging in the values, we can calculate the concentration of sulfuric acid:
Moles of NaOH = (3.4 mL ÷ 1000) x 3.0 M = 0.0102 mol
Moles of H2SO4 = 0.0102 mol ÷ 2 = 0.0051 mol
Volume of H2SO4 = 300.0 mL ÷ 1000 = 0.3 L
Concentration of H2SO4 = 0.0051 mol ÷ 0.3 L ≈ 0.017 M
So, the concentration of sulfuric acid is approximately 0.017 M.