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28 Sep 2019
Consider a titration of 33.8 mL of 1.64 M solution ofaqueous ammonia [Kb(NH3) = 1.8x10^-5] with a 1.24 M solution ofhydrochloric acid. Calculate:
a) The pH of the aqueous ammonia solution before thetitration,
b) The pH of the solution at half-equivalencepoint,
c) The pH after 7.5 mL of HCL were added.
d) The pH of the solution at the equivalencepoint.
e) The pH of the solution when 1.00 mL of the HClhave been added after the equivalence point was reached.
If you could please show me each step I would greatlyappreciate it.
Consider a titration of 33.8 mL of 1.64 M solution ofaqueous ammonia [Kb(NH3) = 1.8x10^-5] with a 1.24 M solution ofhydrochloric acid. Calculate:
a) The pH of the aqueous ammonia solution before thetitration,
b) The pH of the solution at half-equivalencepoint,
c) The pH after 7.5 mL of HCL were added.
d) The pH of the solution at the equivalencepoint.
e) The pH of the solution when 1.00 mL of the HClhave been added after the equivalence point was reached.
If you could please show me each step I would greatlyappreciate it.
Collen VonLv2
28 Sep 2019