9:30 AM Mon Nov 18 < Document Home Insert Draw Layout Review View Refere ii Select Objects 2-Calculate the equilibrium concentration of Ag+(aq) i.e. [Ag+(aq)]eq, when 0.15M of AgNO3(aq) were treated with excess ammonia [NH3(aq)] = 0.85 M? Rf = [CM] X. [CL-WCM] W ล 60% об Draw with Touch 3-Find the equilibrium conc of [Cu2+(aq)] eq after it complexes to 0.03M dien from a starting conc of [Cu2+(aq)] o = 0.012M? (Kf = 3.5 x 1019) mmm 4- A 25 mL Ca2+(aq) solution of [Ca2+(aq)] = 0.025M buffered at pH = 9 is titrated with [EDTA(aq)] = 0.025M. Calculate the concentration of Ca2+(aq) ions at the equivalence point [Ca2+(aq)]ep? 5-(i)Check the detection limit of ferric ions concentration [Fe3+(aq)] at the equivalence point when 25 mL of 0.014 M Fe3+(aq) was titrated with 0.018 M of EDTA. (ii)Determine the unknown concentration of an analyte of ferric ions [Fe3+(aq)] ions in a 25 mL sample buffered at pH = 2? The standardized solution of EDTA is [EDTA]s = 0.016M and a volume of EDTA titrant consumed during titration is 16.50 mL. wwwwww
9:30 AM Mon Nov 18 < Document Home Insert Draw Layout Review View Refere ii Select Objects 2-Calculate the equilibrium concentration of Ag+(aq) i.e. [Ag+(aq)]eq, when 0.15M of AgNO3(aq) were treated with excess ammonia [NH3(aq)] = 0.85 M? Rf = [CM] X. [CL-WCM] W ล 60% об Draw with Touch 3-Find the equilibrium conc of [Cu2+(aq)] eq after it complexes to 0.03M dien from a starting conc of [Cu2+(aq)] o = 0.012M? (Kf = 3.5 x 1019) mmm 4- A 25 mL Ca2+(aq) solution of [Ca2+(aq)] = 0.025M buffered at pH = 9 is titrated with [EDTA(aq)] = 0.025M. Calculate the concentration of Ca2+(aq) ions at the equivalence point [Ca2+(aq)]ep? 5-(i)Check the detection limit of ferric ions concentration [Fe3+(aq)] at the equivalence point when 25 mL of 0.014 M Fe3+(aq) was titrated with 0.018 M of EDTA. (ii)Determine the unknown concentration of an analyte of ferric ions [Fe3+(aq)] ions in a 25 mL sample buffered at pH = 2? The standardized solution of EDTA is [EDTA]s = 0.016M and a volume of EDTA titrant consumed during titration is 16.50 mL. wwwwww
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter18: Principles Of Chemical Reactivity: Entropy And Free Energy
Section: Chapter Questions
Problem 44PS
Related questions
Question
![9:30 AM Mon Nov 18
< Document
Home
Insert
Draw Layout Review
View
Refere
ii Select Objects
2-Calculate the equilibrium concentration of Ag+(aq) i.e. [Ag+(aq)]eq,
when 0.15M of AgNO3(aq) were treated with excess ammonia [NH3(aq)] =
0.85 M?
Rf =
[CM]
X. [CL-WCM] W
ล 60%
об
Draw with Touch
3-Find the equilibrium conc of [Cu2+(aq)] eq after it complexes to 0.03M
dien from a starting conc of [Cu2+(aq)] o = 0.012M? (Kf = 3.5 x 1019)
mmm
4- A 25 mL Ca2+(aq) solution of [Ca2+(aq)] = 0.025M buffered at pH = 9 is
titrated with [EDTA(aq)] = 0.025M. Calculate the concentration of Ca2+(aq)
ions at the equivalence point [Ca2+(aq)]ep?
5-(i)Check the detection limit of ferric ions concentration [Fe3+(aq)] at the
equivalence point when 25 mL of 0.014 M Fe3+(aq) was titrated with 0.018
M of EDTA.
(ii)Determine the unknown concentration of an analyte of ferric ions
[Fe3+(aq)] ions in a 25 mL sample buffered at pH = 2? The standardized
solution of EDTA is [EDTA]s = 0.016M and a volume of EDTA titrant
consumed during titration is 16.50 mL.
wwwwww](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fad79f50e-fcfc-4bdb-91e6-16851ff55aa9%2F62cdc5f0-e74a-47d9-97ee-347023827655%2F72z3tdo_processed.jpeg&w=3840&q=75)
Transcribed Image Text:9:30 AM Mon Nov 18
< Document
Home
Insert
Draw Layout Review
View
Refere
ii Select Objects
2-Calculate the equilibrium concentration of Ag+(aq) i.e. [Ag+(aq)]eq,
when 0.15M of AgNO3(aq) were treated with excess ammonia [NH3(aq)] =
0.85 M?
Rf =
[CM]
X. [CL-WCM] W
ล 60%
об
Draw with Touch
3-Find the equilibrium conc of [Cu2+(aq)] eq after it complexes to 0.03M
dien from a starting conc of [Cu2+(aq)] o = 0.012M? (Kf = 3.5 x 1019)
mmm
4- A 25 mL Ca2+(aq) solution of [Ca2+(aq)] = 0.025M buffered at pH = 9 is
titrated with [EDTA(aq)] = 0.025M. Calculate the concentration of Ca2+(aq)
ions at the equivalence point [Ca2+(aq)]ep?
5-(i)Check the detection limit of ferric ions concentration [Fe3+(aq)] at the
equivalence point when 25 mL of 0.014 M Fe3+(aq) was titrated with 0.018
M of EDTA.
(ii)Determine the unknown concentration of an analyte of ferric ions
[Fe3+(aq)] ions in a 25 mL sample buffered at pH = 2? The standardized
solution of EDTA is [EDTA]s = 0.016M and a volume of EDTA titrant
consumed during titration is 16.50 mL.
wwwwww
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