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28 Sep 2019
Suppose 100.0 mL of a 0.03750 M solution of the strong baseBa(OH)2 is titrated with a 0.4540M solution of the strong acidHClO4. The neutralization reaction is
BA(OH)2 (aq) + 2HClO4(aq) ---> Ba(ClO4)2(aq) + 2H2O(l)
Compute the pH of the titration solution before any acid is added,when the titration is 1.00 mL short of the equivalence point, whenthe titration is at the equivalence point, and when the titrationis 1.00 mL past the equivalence point. (Note: each mole of Ba(OH)2gives two moles of OH- in solution.)
Suppose 100.0 mL of a 0.03750 M solution of the strong baseBa(OH)2 is titrated with a 0.4540M solution of the strong acidHClO4. The neutralization reaction is
BA(OH)2 (aq) + 2HClO4(aq) ---> Ba(ClO4)2(aq) + 2H2O(l)
Compute the pH of the titration solution before any acid is added,when the titration is 1.00 mL short of the equivalence point, whenthe titration is at the equivalence point, and when the titrationis 1.00 mL past the equivalence point. (Note: each mole of Ba(OH)2gives two moles of OH- in solution.)
papayaprofessorLv10
12 Oct 2022
9 Oct 2022
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Elin HesselLv2
28 Sep 2019
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