Problem

A 20.00-mL sample of 0.220 M triethylamine, (CH3CH2)3N, is titrated with 0.544 M HCl....

A 20.00-mL sample of 0.220 M triethylamine, (CH₃CH₂)₃N, is titrated with 0.544 M HCl.

(a) Write a balanced net ionic equation for the titration.

(b) How many milliliters of HCl are required to reach the equivalence point?

(c) Calculate at the equivalence point. (Assume that volumes are additive.)

(d) What is the pH at the equivalence point?

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Solutions For Problems in Chapter 14

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