Question

A 50.0-ml sample of H2SO4 is neutralized with NaOH solution having a concentration of 2.00 M. If 35.5 mL of NaOH are required to complete the neutralization, what is the concentration of the sulfuric acid solution? O 2.84 M O 1.41M O 0.710M O 0.355M

Answer 1

To find the concentration of the sulfuric acid solution, we can use the concept of stoichiometry and the volume and concentration of NaOH solution used in the neutralization. The concentration of the sulfuric acid solution is 0.710 M.

Step-by-step explanation:

To find the concentration of the sulfuric acid solution, we can use the concept of stoichiometry and the volume and concentration of NaOH solution used in the neutralization. Here's how:

1. First, let's calculate the moles of NaOH used in the neutralization:

• Moles of NaOH = volume of NaOH solution used × molarity of NaOH
• Moles of NaOH = 35.5 mL × 2.00 M = 71 mol of NaOH

The balanced equation for the neutralization reaction is H2SO4 (aq) + 2NaOH(aq) → Na2SO4 (aq) + 2H2O(l)From the balanced equation, we can see that 1 mole of H2SO4 reacts with 2 moles of NaOH.Therefore, the moles of H2SO4 = moles of NaOH / 2 = 71 mol / 2 = 35.5 mol of H2SO4Now, let's calculate the concentration of the sulfuric acid solution:

• Concentration of H2SO4 = moles of H2SO4 / volume of H2SO4
• Volume of H2SO4 = 50.0 mL = 0.0500 L
• Concentration of H2SO4 = 35.5 mol / 0.0500 L = 710 M

The concentration of the sulfuric acid solution is 0.710 M.