Question

19. How many mL of 1.50 M NaOH is required to neutralize 275 ml of
0.5 M H₂SO4?

Answer 1

To neutralize 275 mL of 0.5 M H₂SO4, 91.7 mL of 1.50 M NaOH is required.

Step-by-step explanation:

To calculate the volume of NaOH required to neutralize H₂SO4, we need to use the balanced chemical equation between NaOH and H₂SO4. The balanced equation is:

2 NaOH + H₂SO4 -> Na₂SO₄ + 2 H₂O

From the equation, we can see that the ratio of NaOH to H₂SO4 is 2:1. To determine the volume of NaOH, we need to use the equation:

(Volume of NaOH) / (Volume of H₂SO4) = (Molarity of H₂SO4) / (Molarity of NaOH)

Plugging in the values, we have:

(Volume of NaOH) / 275 mL = 0.5 M / 1.50 M

Solving for (Volume of NaOH), we get:

(Volume of NaOH) = (275 mL) * (0.5 M) / (1.50 M)

(Volume of NaOH) = 91.7 mL

Learn more about Neutralization of acids and bases