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Question- A. Calculate the pH at the equivalence point for the titration of 0.160 M Methylamine with 0.160 M HCl. The Kb of methlylamine is 5.0 x 10^-4.
B. Calculate the pH of the resulting solution if 19.0 mL of 0.190 M HCl is added to:
1. 24.0 mL of 0.190 M NaOH...what is pH?
2. 29.0 mL of 0.240 M NaOH...what is pH?
Hello Experts please provide me the detailed computation for above question
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the equivalence point i know you need to use [A-]= moles of HA/(vol water added+vol NaOH added) and believe moles of HA=5.39x10^-3
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