Consider the titration of 25.00 mL of 0.0100 M Sn2+ by 0.0500 M Tl3+ in 1.0...
Consider the titration of 25.00 mL of 0.0100 M Sn2+ by 0.0500 M Tl3+ in 1.0 M HCl, using Pt and saturated calomel electrodes to find the end point. Read the textbook (Quantitative Chemical Analysis, 9th Ed. Daniel Harris, page 375-378).
Sn2+ + Tl3+ → Sn4+ + Tl+
A) Find the net cell voltage E (v) when 1.80 mL of Tl3+ is consumed.
B) Calculate the volume (mL) of Tl3+ used at the equivalence point.
C) Find the net cell voltage E (v) at the equivalence point.
D) Find the net cell voltage E (v) when 5.90 mL of Tl3+ is consumed.
Homework Answers
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Consider the titration of 25.00 mL of 0.0100 M Sn2+
by 0.0500 M Tl3+ in 1.0...
Consider the titration of 25.0 mL of 0.01000 M Sn2+ by 0.0500 M Tl3+ in 1...
Consider the titration of 25.0 mL of 0.01000 M Sn2+
by 0.0500 M Tl3+ in 1 M HCl, using Pt and saturated
calomel electrodes to find the endpoint.
a.) Write the balanced titration reaction.
b.) Write two different half-reactions for the indicator
electrode.
c.) Write two different Nernst equations for the cell
voltage.
d.) Calculate E at the following volumes of Tl3+:
1.00, 2.50, 4.90, 5.00, 5.10, and 10.0 mL.
(This is problem 3 in Chapter 15 from Eigth Edition...
5. Consider the titration of 25.0 mL of 0.0100 M Sn2 by 0.0500 M Ti Pt and saturated calomel electrodes to find the end point. (total 15 pt) M HCI, using (c) Write two different Nernst equations for...
5. Consider the titration of 25.0 mL of 0.0100 M Sn2 by 0.0500 M Ti Pt and saturated calomel electrodes to find the end point. (total 15 pt) M HCI, using (c) Write two different Nernst equations for the cell voltage. (3 pt) (d) Calculate E at the following volumes of TI: 1.0, 2.5,4.9,5.0,5.1, and 10.0 mL. (6 pt)
5. Consider the titration of 25.0 mL of 0.0100 M Sn2 by 0.0500 M Ti Pt and saturated calomel electrodes to...
ans A C B how ? 14. Consider the titration of 25.00 mL of 0.0500 M...
ans A C B how ?
14. Consider the titration of 25.00 mL of 0.0500 M Sn2+ with 0.100 M Fe3+ in 1 M HCl to give Fe2+ and Sn4+, using Pt and saturated calomel electrodes SCE l Sn4+, Sn2+, Fe3+, Fe3 | Pt(s) The titration reaction: 2Fe3 + Sn2+Snt+ 2Fe2+ The two half-reactions for the indicator electrode: Fe3+e Sn 2e Sn2+ Indicate the two Nernst equations for the cell voltage. E 0.732 V E 0.139 V Fe2+ IFe2 log...
Мар You are performing a titration of 25.0 mL of 0.0100 M Sn4 in 1 M HCI with 0.0500 M Ag* to give Sn2 anu 3+ Ags using...
Мар You are performing a titration of 25.0 mL of 0.0100 M Sn4 in 1 M HCI with 0.0500 M Ag* to give Sn2 anu 3+ Ags using a Pt indicator electrode and a saturated calomel electrode (SCE) as the reference electrode. A) Write the balanced titration reaction B) Complete the two half-reactions that occur at the indicator electrode (shown is their corresponding reduction potential) Sn E 0.139 V 3+ Ag® Eo 1.90 V C) Choose the two different expressions...
Redox titration between Sn2 + 0.2 M 20 ml and Cr2O7 ^ -2 0.0006 M in...
Redox titration between Sn2 + 0.2 M 20 ml and Cr2O7 ^ -2 0.0006 M in 1 M H2So4 solution at all times Sn4+ + 2e >> Sn2+ E (v) = 0.154 Cr2O7^-2 + 14H + 6e>> 2Cr3 + 7H2O E (v) = 1.33 1.initial point 2.Before equivalence point 100 ml and 200 ml 3. Equivalent point 4.After equivalent point
Calculate the potential when 25.00 mL of 0.0750 M Cut is titrated with 12.50 mL of...
Calculate the potential when 25.00 mL of 0.0750 M Cut is titrated with 12.50 mL of 0.150 M Fe3+ in the presence of 1 M HCl, using Pt and saturated calomel electrodes to find the end point. Fe3 Fe E+0732 v Fe3t +e Fe2+ E0.732v Cu2+ +eCut E +0.161 V a +0.401 V 0 b. +0.206 V +1.124v d. +0.157 V
3. (20 points) Consider the titration of 25.0 mL of 0.05 M Sna' with 0.100 M...
3. (20 points) Consider the titration of 25.0 mL of 0.05 M Sna' with 0.100 M Fell in 1 M HCl to give Fe2+ and Sn" using Pt and calomel electrodes. a) Write a balanced titration reaction. b) Write two half-reactions for the indicator electrode. c) Write two Nernst equations for the cell voltage d) Calculate E at the following volumes of Fe3+: 1.0, 5.0, 10.0, 12.5, 17.5, 20.0, 24.0, 25.0, 26.0 and 30.0 mL. Make the titration curve graph.
Consider the titration of 30.0 mL of 0.20 M nitrous acid by adding 0.0500 M aqueous...
Consider the titration of 30.0 mL of 0.20 M nitrous acid by adding 0.0500 M aqueous ammonia to it. The pH at the equivalence point is _____. (Note: This is the titration of a weak acid with a weak base.) (a) greater than 7 (b) equal to 7 (c) less than 7 (d) cannot be determined without more data (not including Ka and Kb) (e) is impossible to predict
PH Ht! B C mL of titrating reagent in buret → 9. For the titration of 100.0 mL of 0.0500 M NH...
ANSWER NUMBER 9 ONLY
SHOW ALL WORK
pH Ht! B C mL of titrating reagent in buret → We were unable to transcribe this image9. For the titration of 100.0 mL of 0.0500 M NH, with 0.100 M HCI, the curve will look different he diagram on the other side of this page (see your answer to question 7). Considering the than t points to be in corresponding places to the curve presented for question 8, calculate parts a-f from...
You are titrating 100.0 mL of 0.0400 M Fe2+ in 1 M HCIO4 with 0.100 M...
You are titrating 100.0 mL of 0.0400 M Fe2+ in 1 M HCIO4 with 0.100 M Ce4+ to give Fe3+ and Ce3+ using Pt and calomel electrodes to find the endpoint. (a) Write the balanced titration reaction. > (b) Complete the two half reactions for the Pt electrode. Ce té E° = 1.70 V Fe +e = E° = 0.767 V [Fe2+11 1 - 0.241 E= 0.767 – 0.05916) (c) From the list in the column at the right, select...
Consider the titration of 25.0 mL of 0.01000 M Sn2+
by 0.0500 M Tl3+ in 1 M HCl, using Pt and saturated
calomel electrodes to find the endpoint.
a.) Write the balanced titration reaction.
b.) Write two different half-reactions for the indicator
electrode.
c.) Write two different Nernst equations for the cell
voltage.
d.) Calculate E at the following volumes of Tl3+:
1.00, 2.50, 4.90, 5.00, 5.10, and 10.0 mL.
(This is problem 3 in Chapter 15 from Eigth Edition...
5. Consider the titration of 25.0 mL of 0.0100 M Sn2 by 0.0500 M Ti Pt and saturated calomel electrodes to find the end point. (total 15 pt) M HCI, using (c) Write two different Nernst equations for the cell voltage. (3 pt) (d) Calculate E at the following volumes of TI: 1.0, 2.5,4.9,5.0,5.1, and 10.0 mL. (6 pt)
5. Consider the titration of 25.0 mL of 0.0100 M Sn2 by 0.0500 M Ti Pt and saturated calomel electrodes to...
ans A C B how ?
14. Consider the titration of 25.00 mL of 0.0500 M Sn2+ with 0.100 M Fe3+ in 1 M HCl to give Fe2+ and Sn4+, using Pt and saturated calomel electrodes SCE l Sn4+, Sn2+, Fe3+, Fe3 | Pt(s) The titration reaction: 2Fe3 + Sn2+Snt+ 2Fe2+ The two half-reactions for the indicator electrode: Fe3+e Sn 2e Sn2+ Indicate the two Nernst equations for the cell voltage. E 0.732 V E 0.139 V Fe2+ IFe2 log...
Мар You are performing a titration of 25.0 mL of 0.0100 M Sn4 in 1 M HCI with 0.0500 M Ag* to give Sn2 anu 3+ Ags using a Pt indicator electrode and a saturated calomel electrode (SCE) as the reference electrode. A) Write the balanced titration reaction B) Complete the two half-reactions that occur at the indicator electrode (shown is their corresponding reduction potential) Sn E 0.139 V 3+ Ag® Eo 1.90 V C) Choose the two different expressions...
Calculate the potential when 25.00 mL of 0.0750 M Cut is titrated with 12.50 mL of 0.150 M Fe3+ in the presence of 1 M HCl, using Pt and saturated calomel electrodes to find the end point. Fe3 Fe E+0732 v Fe3t +e Fe2+ E0.732v Cu2+ +eCut E +0.161 V a +0.401 V 0 b. +0.206 V +1.124v d. +0.157 V
3. (20 points) Consider the titration of 25.0 mL of 0.05 M Sna' with 0.100 M Fell in 1 M HCl to give Fe2+ and Sn" using Pt and calomel electrodes. a) Write a balanced titration reaction. b) Write two half-reactions for the indicator electrode. c) Write two Nernst equations for the cell voltage d) Calculate E at the following volumes of Fe3+: 1.0, 5.0, 10.0, 12.5, 17.5, 20.0, 24.0, 25.0, 26.0 and 30.0 mL. Make the titration curve graph.
ANSWER NUMBER 9 ONLY
SHOW ALL WORK
pH Ht! B C mL of titrating reagent in buret → We were unable to transcribe this image9. For the titration of 100.0 mL of 0.0500 M NH, with 0.100 M HCI, the curve will look different he diagram on the other side of this page (see your answer to question 7). Considering the than t points to be in corresponding places to the curve presented for question 8, calculate parts a-f from...
You are titrating 100.0 mL of 0.0400 M Fe2+ in 1 M HCIO4 with 0.100 M Ce4+ to give Fe3+ and Ce3+ using Pt and calomel electrodes to find the endpoint. (a) Write the balanced titration reaction. > (b) Complete the two half reactions for the Pt electrode. Ce té E° = 1.70 V Fe +e = E° = 0.767 V [Fe2+11 1 - 0.241 E= 0.767 – 0.05916) (c) From the list in the column at the right, select...
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