Question

In: Chemistry

Question 5. Suppose titration of 100.00 mL mixture of 0.0500 M in Br- + 0.08 M...

Question 5. Suppose titration of 100.00 mL mixture of 0.0500 M in Br- + 0.08 M Cl-   with 0.4000 M AgNO3 with (AgNO3 completely dissolves, AgCl and AgBr are sparingly soluble)

  1. (3 pts) Which specie precipitates first? And why?
  2. (3 pts) What is the volume of AgNO3 necessary at the first equivalence point?
  3. (3 pts) What is the most significant source of Ag+ at the first equivalence point for calculation of pAg? and why?
  4. (3 pts) What is the pAg at the first equivalence point?
  5. (3 pts) What is the volume of AgNO3 necessary to reach the second end point?

Solutions

Expert Solution

Here is the Solution:

Thanks! :-)

queen_honey_blossom answered 2 years ago
Next > < Previous

Related Solutions

5. For the titration of 50.00 mL of 0.0500 M Ce4+ with 0.1000 M Fe2+ in...
5. For the titration of 50.00 mL of 0.0500 M Ce4+ with 0.1000 M Fe2+ in the presence of 1 M H2SO4, please calculate the system potential while 3.00 mL of Fe2+ is added. Ce4+ + e <==> Ce3+, E0 = + 1.44 V (in 1 M H2SO4) Fe3+ + e <==> Fe2+, E0 = + 0.68 V (in 1 M H2SO4). Answer is 1.49 V 5b)  In the above titration, what's the electrode potential after 28.90 mL of Fe2+ is...
For the titration of 40.0 mL of 0.0100 M Sn2 by 0.0500 M Tl3 in 1...
For the titration of 40.0 mL of 0.0100 M Sn2 by 0.0500 M Tl3 in 1 M HCl, using Pt and Ag | AgCl electrodes: (c) What are the two Nernst equations for the cell voltage? The potential for the Ag | AgCl electrode is 0.197 V.] (d) What is the value of E at the following volumes of added Tl3 ? 1.0mL 4.0mL 7.9mL 8.0mL 8.1mL 13mL
For the titration of 40.0 mL of 0.0100 M Sn2 by 0.0500 M Tl3 in 1...
For the titration of 40.0 mL of 0.0100 M Sn2 by 0.0500 M Tl3 in 1 M HCl, using Pt and Ag | AgCl electrodes: (c) What are the two Nernst equations for the cell voltage? The potential for the Ag | AgCl electrode is 0.197 V.] (d) What is the value of E at the following volumes of added Tl3 ? 1.0mL 4.0mL 7.9mL 8.0mL 8.1mL 13mL
For the titration of 35.0 mL of 0.0100 M Sn2 by 0.0500 M Tl3 in 1...
For the titration of 35.0 mL of 0.0100 M Sn2 by 0.0500 M Tl3 in 1 M HCl, using Pt and Ag | AgCl electrodes: (a) What is the balanced titration reaction? (b) What are the two half-reactions that occur at the indicator electrode? (c) What is the value of E at the following volumes of added Tl3 ? 1 mL 3.5 mL 6.9 mL 7 mL 7.1 mL 12 mL
For the titration of 40.0 mL of 0.0100 M Sn2 by 0.0500 M Tl3 in 1...
For the titration of 40.0 mL of 0.0100 M Sn2 by 0.0500 M Tl3 in 1 M HCl, using Pt and Ag | AgCl electrodes: (c) What are the two Nernst equations for the cell voltage? The potential for the Ag | AgCl electrode is 0.197 V.] (d) What is the value of E at the following volumes of added Tl3 ? 1.0mL 4.0mL 7.9mL 8.0mL 8.1mL 13mL
19. a. For the titration of 50.00 mL of 0.0500 M Fe2+ with 0.1000 M Ce4+...
19. a. For the titration of 50.00 mL of 0.0500 M Fe2+ with 0.1000 M Ce4+ in the presence of 1 M H2SO4, please calculate the system potential after 2.25 mL of Ce4+ is added . Ce4+ + e ÍÎ Ce3+, E0 = + 1.44 V (in 1M H2SO4) Fe3+ + e ÍÎ Fe2+, E0 = + 0.68 V (in 1M H2SO4). They got Esystem = 0.62 V. b)  For the same titration as in question (a), what’s the system potential...
Consider the titration of 25.0 mL of 0.0500 M Sn2+ with 0.100 M Fe3+ in 1...
Consider the titration of 25.0 mL of 0.0500 M Sn2+ with 0.100 M Fe3+ in 1 M HCl to give Fe2+ and Sn4+, using a Pt and calomel electrodes. (a) write a balanced titration reaction (b) write two half-reactions fo the indicator electrode (c) write two Nerst equations for the cell voltage (d) calculate E at the following volumes of Fe3+: 1.0, 12.5, 24.0, 25.0, 26.0, and 30.0 mL. Sketch the titration curve.
Consider the titration of 50.0 mL of 0.0500 M Cu+ with 0.1000 M Fe3+ to give...
Consider the titration of 50.0 mL of 0.0500 M Cu+ with 0.1000 M Fe3+ to give Cu2+ and Fe2+ using Pt and standard H+/H2 reference electrode to find the end point. The standard electrode potentials are E0Cu+/Cu2+=0.161 V and E0Fe2+/Fe3+=0.767 V. Calculate the actual electrode potential, E, at the following volumes of Cu2+ (i) 15, (ii) 25, and (iii) 26 mL
In an acid base titration experiment, 50.0 ml of a 0.0500 m solution of acetic acid...
In an acid base titration experiment, 50.0 ml of a 0.0500 m solution of acetic acid ( ka =7.5 x 10^-5) was titrated with a 0.0500 M solution of NaOH at 25 C. The system will acquire this pH after addition of 20.00 mL of the titrant: Answer is 4.581 Please show all work
Consider the titration of 50.0 mL of 0.0500 M C2H5NH2 (a weak base; Kb = 0.000640)...
Consider the titration of 50.0 mL of 0.0500 M C2H5NH2 (a weak base; Kb = 0.000640) with 0.100 M HIO4. Calculate the pH after the following volumes of titrant have been added: (a) 0.0 mL pH =   (b) 6.3 mL pH =   (c) 12.5 mL pH =   (d) 18.8 mL pH =   (e) 25.0 mL pH =   (f) 30.0 mL pH =  
ADVERTISEMENT
Subjects
ADVERTISEMENT
Latest Questions
ADVERTISEMENT