100 mL of an aqueous HCl solution with pH = 1.0 is mixed with 400 mL of an aqueous NaOH solution with pH = 12.0 . The resulting mixture is then diluted with water to a final total volume of 1000 mL . The pH of the final diluted solution is:

Question

100 mL of an aqueous HCl solution with pH = 1.0 is mixed with 400 mL of an aqueous NaOH solution with pH = 12.0 . The resulting mixture is then diluted with water to a final total volume of 1000 mL . The pH of the final diluted solution is: (Given 2=0.30 , 3=0.48 )

Quantrex Academy · Accepted Answer

Correct answer: D. 2.22

For HCl solution: pH = 1.0 [ H ⁺] = 10⁻¹ M = 0.1 M Millimoles of H ⁺ = 0.1 M 100 mL = 10 mmol For NaOH solution: pH = 12.0 pOH = 2.0 [ OH ⁻] = 10⁻² M = 0.01 M Millimoles of OH ⁻ = 0.01 M 400 mL = 4 mmol Upon mixing, neutralization occurs: Remaining millimoles of H ⁺ = 10 - 4 = 6 mmol The mixture is diluted to a final total volume of 1000 mL . Final [ H ⁺] = 6 mmol 1000 mL = 6 10⁻³ M pH = - (6 10⁻³) = 3 - 6 = 3 - ( 2 + 3) pH = 3 - (0.30 + 0.48) = 3 - 0.78 = 2.22 Answer: 2.22

100 mL of an aqueous HCl solution with pH = 1.0 is mixed with 400 mL of an aqueous NaOH solution with pH = 12.0 . The resulting mixture is then diluted with water to a final total volume of 1000 mL . The pH of the final diluted solution is: (Given 2=0.30 , 3=0.48 )

Options

Correct answer

Step-by-step solution

More from Ionic Equilibrium