Answer to Question #278402 in Chemistry for Kate

Question

25.00 mL of 6.00 M H2SO4 solution is diluted with water to a volume of 2.000L. What is the [H+] and [OH-] of the resulting solution?

Answer 1

Solution:

Convert mL to L:

(25.00 mL) × (1 L / 1000 mL) = 0.025 L

Calculate the concentration of the diluted H₂SO₄ solution:

(6.00 M H₂SO₄) × (0.025 L / 2.000 L) = 0.075 M

C_M(H₂SO₄) = 0.075 M

H₂SO₄ is a strong acid which dissociates as follows:

H₂SO₄ → 2H⁺ + SO₄^2-

Therefore,

[H⁺] = 2 × C_M(H₂SO₄) = 2 × (0.075 M) = 0.15 M

[H⁺] = 0.15 M

K_w = [H⁺] × [OH^-] = 1.0×10^-14

Therefore,

[OH^-] = K_w / [H⁺] = (1.0×10^-14) / (0.15) = 6.67×10^-14

[OH^-] = 6.67×10^-14 M

Answer:

[H⁺] = 0.15 M

[OH^-] = 6.67×10^-14 M