Question

Consider the reaction below H₂SO4 + 2 NaOH ---> NaSO₄ + 2 H₂O How many mL of a .75 M solution is required to completely react with 150 mL of a .18 M solution of H₂SO₄

a.) 36 mL
b.) 27 mL
c.) 72 mL
d.) 63 mL"

Answer 1

To completely react with 150 mL of a 0.18 M solution of H₂SO₄, you would need 72 mL of a 0.75 M solution of NaOH.

Step-by-step explanation:

To find the volume of a 0.75 M solution of NaOH needed to react with 150 mL of a 0.18 M solution of H₂SO₄, we can use the balanced chemical equation provided. From the equation, we can see that the ratio of NaOH to H₂SO₄ is 2:1, meaning that 2 moles of NaOH react with 1 mole of H₂SO₄. First, we need to calculate the number of moles of H₂SO₄ by multiplying its concentration (0.18 M) by its volume (150 mL or 0.150 L): 0.18 M * 0.150 L = 0.027 mol of H₂SO₄ Since the mole ratio is 2:1, we need 2 moles of NaOH for every 1 mole of H₂SO₄. Therefore, we need 2 * 0.027 mol = 0.054 mol of NaOH. Next, we can calculate the volume of the 0.75 M NaOH solution using the moles and concentration: 0.054 mol / 0.75 M = 0.072 L or 72 mL Therefore, 72 mL of a 0.75 M NaOH solution is required to completely react with 150 mL of a 0.18 M solution of H₂SO₄.