1
answer
0
watching
214
views
11 Dec 2019
Consider the titration of a 24.0-mL sample of 0.175 M CH3NH2 with 0.150 M HBr. (The value of Kb for CH3NH2 is 4.4Ã10â4.)
Part A)Determine the
pH at 4.0 mL of added acid.
Part B)Determine the
pH at one-half of the equivalence point.
Part C)Determine the
pH at the equivalence point.
Part D) Determine the
pH after adding 6.0 mL of acid beyond the equivalence point.
Consider the titration of a 24.0-mL sample of 0.175 M CH3NH2 with 0.150 M HBr. (The value of Kb for CH3NH2 is 4.4Ã10â4.)
Part A)Determine the
pH at 4.0 mL of added acid.
Part B)Determine the
pH at one-half of the equivalence point.
Part C)Determine the
pH at the equivalence point.
Part D) Determine the
pH after adding 6.0 mL of acid beyond the equivalence point.
Hubert KochLv2
13 Dec 2019