Calculate the pH at the equivalence point in the titration of
20.00 mL of a 0.100...
Calculate the pH at the equivalence point in the titration of
20.00 mL of a 0.100 M solution of CH3NH2 (Kb for CH3NH2 = 4.4 ×
10-4) with a 0.200 M HCl solution. (The reaction products are
CH3NH3+ and Cl-)
What is the pH at the equivalence point for the titration of
25.00 mL 0.100 M CH3CH2CH2CO2- with 0.1848 M HCl? Species (K
values) CH3CH2CH2CO2H (Ka = 1.14E-5) CH3CH2CH2CO2- (Kb =
2.63x10-10
A) What is the pH at the equivalence point in the titration of a
15.6 mL sample of a 0.312 M
aqueous hypochlorous acid solution with a
0.302 M aqueous barium hydroxide
solution?
pH = ___
B) When a 18.2 mL sample of a
0.426 M aqueous hypochlorous acid
solution is titrated with a 0.458 M aqueous
barium hydroxide solution, what is the pH at the
midpoint in the titration?
pH = ___
What is the pH at the equivalence point in the titration of of a
29.5 mL sample of a 0.460 M aqueous hydroflouric acid solution with
a 0.358 M aqueous sodium hydroxide solution?
pH - ___
What is the pH at the equivalence point in the titration of a
22.6 mL sample of a 0.457 M
aqueous hypochlorous acidsolution with a
0.311 M aqueous barium hydroxide
solution?
pH =