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
Homework Answers
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Redox titration between Sn2 + 0.2 M 20 ml and Cr2O7 ^ -2 0.0006
M in...
Calculate the electrode potential at 25ºC of the Cr3+, Cr2O7 2- electrode at pH 1 and...
Calculate the electrode potential at 25ºC of the Cr3+, Cr2O7 2- electrode at pH 1 and pH 3 in a solution 0.01 M in both Cr3+, Cr2O7 2-, on the assumption that all activity coefficients are unity. The electrode reaction and corresponding standard electrode potential are as follows: Cr2 O7^2+ + 14H+ + 6e- <-> 2Cr3+ + 7H2O Eº=1.33
help me find the molarity of Sn2+ Redox Titration in Acidic Medium 504 Total 2. Push...
help me find the molarity of
Sn2+
Redox Titration in Acidic Medium 504 Total 2. Push Slider Up to Add a Volume of K2Cr2O7 Volume of K2Cr2O7 Oxidizing Agent KMnO4 K2Cr2O7 Reducing Agent Fe2+ Sn2+ S2032- Reaction 1. Select the 40.52 ml 40.5 ml 3. After Titration, Calculate and Enter Molarity of Sn2+ Molarity of K2Cr2O7 51100 M M OK - Dropwise 3Sn2+ + Cr202-7+ 14H+ 3Sn4+ + 2 Cr3+ + 7H2O Repeat Volume of Sn2+ 25.00 ml Reset
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...
In a titration experiment, 12.6 mL of an aqueous HCl solution was titrated with 0.2 M...
In a titration experiment, 12.6 mL of an aqueous HCl solution was titrated with 0.2 M NaOH solution. The equivalence point in the titration was reached when 9.6 mL of the NaOH solution was added. What is the molarity of the HCl solution?
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...
1. Consider the titration of 50.0 mL of 0.200 M HNO3 with 0.100 M NaOH solution....
1. Consider the titration of 50.0 mL of 0.200 M HNO3 with 0.100 M NaOH solution. What volume of NaOH is required to reach the equivalence point in the titration? a. 25.0 mL b. 50.0 mL c. 1.00 × 10^2 mL d. 1.50 × 10^2 mL 2. Consider the following acid–base titrations: I) 50 mL of 0.1 M HCl is titrated with 0.2 M KOH. II) 50 mL of 0.1 M CH3COOH is titrated with 0.2 M KOH. Which statement...
1 in a certain titration 10.7 ml of 0 205 M NaOH was consumed to bitrate...
1 in a certain titration 10.7 ml of 0 205 M NaOH was consumed to bitrate 20.0 mL of H.SO solution a) White balanced molecular equation of the acid base reaction. 2 pts hi Calculate the moles of NaOH consumed (Show calculations with units at each stage 2 pts and answer with correct sia fig and with units 1 pt) • 200 MOON c) Calculate the moles of H2SO4 present in the sample. (Show calculations with units at each stage...
(1) Determine the pH during the titration of 58.4 mL of 0.386 M hypochlorous acid (Ka...
(1) Determine the pH during the titration of 58.4 mL of 0.386 M hypochlorous acid (Ka = 3.5×10-8) by 0.386 M NaOH at the following points. (a) Before the addition of any NaOH (b) After the addition of 15.0 mL of NaOH (c) At the half-equivalence point (the titration midpoint) (d) At the equivalence point (e) After the addition of 87.6 mL of NaOH (2) Determine the pH during the titration of 39.1 mL of 0.369 M ethylamine (C2H5NH2 ,...
Consider the titration of a 27.0 −mL sample of 0.170 M CH3NH2 with 0.155 M HBr....
Consider the titration of a 27.0 −mL sample of 0.170 M CH3NH2 with 0.155 M HBr. Determine each of the following. Part A the initial pH Express your answer using two decimal places. pH = SubmitMy AnswersGive Up Part B the volume of added acid required to reach the equivalence point V = mL SubmitMy AnswersGive Up Part C the pH at 6.0 mL of added acid Express your answer using two decimal places. pH = SubmitMy AnswersGive Up Part...
Consider the titration of a 34.0 mL sample of 0.170 M HBr with 0.205 M KOH....
Consider the titration of a 34.0 mL sample of 0.170 M HBr with 0.205 M KOH. Determine each of the following: a. the initial pH Express your answer using three decimal places. pH = ??? b. the volume of added base required to reach the equivalence point Express your answer in milliliters. V = ??? c. the pH at 10.6 mL of added base Express your answer using three decimal places. p H = ??? d. the pH at the...
help me find the molarity of
Sn2+
Redox Titration in Acidic Medium 504 Total 2. Push Slider Up to Add a Volume of K2Cr2O7 Volume of K2Cr2O7 Oxidizing Agent KMnO4 K2Cr2O7 Reducing Agent Fe2+ Sn2+ S2032- Reaction 1. Select the 40.52 ml 40.5 ml 3. After Titration, Calculate and Enter Molarity of Sn2+ Molarity of K2Cr2O7 51100 M M OK - Dropwise 3Sn2+ + Cr202-7+ 14H+ 3Sn4+ + 2 Cr3+ + 7H2O Repeat Volume of Sn2+ 25.00 ml Reset
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...
1 in a certain titration 10.7 ml of 0 205 M NaOH was consumed to bitrate 20.0 mL of H.SO solution a) White balanced molecular equation of the acid base reaction. 2 pts hi Calculate the moles of NaOH consumed (Show calculations with units at each stage 2 pts and answer with correct sia fig and with units 1 pt) • 200 MOON c) Calculate the moles of H2SO4 present in the sample. (Show calculations with units at each stage...
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