A 100.0 mL sample of 0.10 mol L^-1 Ca(OH)₂ is titrated with 0.10 mol L^-¹ HBr.Determine the pH of the solution after the addition of 300.0 mL HBr. A)1.60 B)1.30 C)1.00 D)12.40 E)1.12

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Quizplus · Accepted Answer

Ca(OH)2 is a strong base and HBr is a strong acid. The reaction is: Ca(OH)2 + 2HBr → CaBr2 + 2H2O. Initially, there are 0.01 mol of OH- ions. Adding 300 mL of 0.10 M HBr gives 0.03 mol of H+. After neutralizing OH-, 0.02 mol of H+ remains in 400 mL solution, giving [H+] = 0.05 M. pH = -log(0.05) = 1.30.

A 1000 ML Sample of 0