Solution of ethanolamine is titrated with hydrochloric acid

Reference no: EM13695636

Question- The compound ethanolamine, HOCH2CH2NH2, is a weak base. If 49.5 mL of a 0.029 M solution of ethanolamine is titrated with 0.100 M hydrochloric acid.

1) What would be the PH at the beginning of this titration? (Kb=3.1*10^-5)

2) How many mL of HCL will be needed to reach the equivalence point?

3) What would be the pH at the equivalence point?

4) What would be the pH when 10 more mL of hydrochloric acid was added past the equivalence point?

Please show all work in so far as possible. I am in reality struggling with understanding titration problems

Reference no: EM13695636

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