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Chemistry, 12.12.2019 03:31 ayoismeisjjjjuan
10. a 20.00 ml sample of 0.150 mol/l ammonia (nh3(aq)) is titrated to the equivalence point by 20.0 ml of a solution of 0.150 mol/l of the strong acid hydroiodic acid (hi (
a) write a balanced equation for the titration reaction.
b) what is the ph of the ammonia solution before the titration begins?
c) what is the ph at the equivalence point?
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Answer asap need it by wednesday morning carry out the following calculations on ph and ka of from data. i. calculate the ph of 0.02m hcl ii. calculate the ph of 0.036m naoh iii. calculate the ph of 0.36m ca(oh)2 iv. calculate the ph of 0.16m ch3cooh which has ka = 1.74 x 10-5 mol dm-3 v. calculate ka for weak acid ha which has a ph of 3.65 at 0.30m concentration vi. calculate the ka of a solution made by mixing 15.0 cm3 0.2m ha and 60.0 cm3 0.31m a-. [ph= 3.80] vii. calculate the ph of a solution made by mixing 15.0 cm3 0.1m naoh and 35.0 cm3 0.2m hcooh. [ka = 1.82 x 10-4 m]
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10. a 20.00 ml sample of 0.150 mol/l ammonia (nh3(aq)) is titrated to the equivalence point by 20.0...
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