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13 Dec 2019

A 50.0 mL solution of 0.200 M ammonia (pKa of ammonia is 9.24) is titrated by 0.100 M HCl. Calculate the pH of the solution when, A.) the volume of HCl is 20.00 mL B.) the volume of HCl is 100.0 mL

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Jean Keeling
Jean KeelingLv2
17 Dec 2019

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Related questions

An 80 mL sample of 0.200 M ammonia is titrated with 0.100 M HCl. Kb for ammonia is 1.8*10-5. Calculate the pH of the solution at each of the following points of the titration:

a) before the addition of any HCl

b) halfway to the equivalence point

c) at the equivalence point

d) after the addition of 175 mL of 0.100 M HCl

A 50.0-mL sample of a 0.100 M solution of NaCN is titrated by 0.200 M HCl.

Kb for CN− is 2.0×10−5. Calculate the pH of the solution:

  1. Prior to the start of the titration
  2. After the addition of 15.0 mL of 0.200 M HCl
  3. At the equivalence point
  4. After the addition of 30.0 mL of 0.200 M HCl

If 50.0 mL of 0.200 M solution of ammonia are titrated with 0.100 M solution of HNO3, what volume of HNO3 is required to reach the equvalence point? What is the pH at that point?

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