A 25.00 mL solution of 0.100 M CH3NH2 is titrated with 0.1331 M HCl. What is...

A 25.00 mL solution of 0.100 M CH3NH2 is titrated with 0.1331 M HCl. What is the pH at the equivalence point of the titration? Species (K values) CH3NH2 (Kb = 3.74x10-4) CH3NH3+ (Ka = 2.70x10-11)

Expert Solution

queen_honey_blossom answered 2 years ago

25.00 mL 0.100 M CH3NH2 is titrated with 0.100 M HCl. Calculate the pH of this...

25.00 mL 0.100 M CH3NH2 is titrated with 0.100 M HCl. Calculate the pH of this the titration solution after the addition of a) 12.5 mL and b) 25.00 mL of the titrant has been added. Based on these pH values, select an appropriate indicator for the titration from table at the end of lecture notes for Chapter 16.

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