You are titrating 100.0 mL of 0.0200 M Fe3 in 1 M HClO4 with 0.100 M...

You are titrating 100.0 mL of 0.0200 M Fe3 in 1 M HClO4 with 0.100 M Cu to give Fe2 and Cu2 using Pt and saturated Ag | AgCl electrodes to find the endpoint. d) Calculate the values of E for the cell when the following volumes of the Cu titrant have been added: (Activity coefficients may be ignored as they tend to cancel when calculating concentration ratios.) 1.50mL 10.0mL 18.0mL 20.0mL 21.0mL 40.0mL

Expert Solution

queen_honey_blossom answered 2 years ago

You are titrating 25.00 mL of a 0.100 M solution of a weak acid with a...

You are titrating 25.00 mL of a 0.100 M solution of a weak acid with a 0.250 M solution of potassium hydroxide. Assume the pKa of the weak acid is 5.6. A. What is the pH after adding 3.0 mL of 0.250 M potassium hydroxide? B. What is the pH at the midpoint of the titration? C. What is the pH at the equivalence point of the titration?

Ascorbic asic (0.0100 M) was added to 10.0 mL of 0.0200 M Fe3+ at pH =...

Ascorbic asic (0.0100 M) was added to 10.0 mL of 0.0200 M Fe3+ at pH = 0.30, and the potential was monitored with Pt and saturated Ag/AgCl electrodes. Dehydroascorbic acid + 2H+ + 2e- --> ascorbic acid + H2O (Eo = 0.390 V) Using Eo = 0.767 V for the Fe3+/Fe2+ couple, calculate the cell voltage when 5.0, 10.0, and 15.0 mL of ascorbic acid have been added. Correct answers are: 0.570 V, 0.307 V, and 0.184 V but not...

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.

1) Consider the titration of 50.0 mL of 0.200 M HClO4 by 0.100 M NaOH. Complete...

1) Consider the titration of 50.0 mL of 0.200 M HClO4 by 0.100 M NaOH. Complete the table with answers to the following questions: What is the pH after 35.5 mL of NaOH has been added? At what volume (in mL) of NaOH added does the pH of the resulting solution equal 7.00?

Consider the titration of 100.0 mL of 0.0200 M H3PO4 with 0.121 M NaOH. Calculate the...

Consider the titration of 100.0 mL of 0.0200 M H3PO4 with 0.121 M NaOH. Calculate the milliliters of base that must be added to reach the first, second, and third equivalence points.

Consider the titration of 100.0 mL of 0.100 M HCN by 0.100 M KOH at 25°C....

Consider the titration of 100.0 mL of 0.100 M HCN by 0.100 M KOH at 25°C. Ka for HCN = 6.2×10-10. Part 1 Calculate the pH after 0.0 mL of KOH has been added. pH = Part 2 Calculate the pH after 50.0 mL of KOH has been added. pH = Part 3 Calculate the pH after 75.0 mL of KOH has been added. pH = Part 4 Calculate the pH at the equivalence point. pH = Part 5 Calculate...

Consider the titration of 40.0 mL of 0.200 M HClO4 by 0.100 M KOH. Calculate the...

Consider the titration of 40.0 mL of 0.200 M HClO4 by 0.100 M KOH. Calculate the pH of the resulting solution after the following volumes of KOH have been added. a. 0.0 mL d. 80.0 mL b. 10.0 mL e. 100.0 mL c. 40.0 mL answers are A) 0.699 B) 0.854 C) 1.301 D) 7.00 E) 12.15 I would just like to know how to do the work please and tbank you

Consider the titration of 50.0 mL of a 0.0200 M solution of butanoic acid with 0.100...

Consider the titration of 50.0 mL of a 0.0200 M solution of butanoic acid with 0.100 M NaOH. First, calculate the equivalence point (Ve). Then, calculate the pH at the following points along the titration curve. Assume fractions are exact numbers and ignore activities for all calculations in this problem. A) VNaOH= 0.000 mL B) VNaOH= 1/2Ve C) VNaOH= 4/5Ve D) VNaOH= Ve E) VNaOH= 3/2Ve

You prepare an equilibrium mixture by combining 4.00 mL 0.00129 M Fe3+ with 0.100 mL 0.00582...

You prepare an equilibrium mixture by combining 4.00 mL 0.00129 M Fe3+ with 0.100 mL 0.00582 M SCN-. What is [Fe3+]o for this mixture? Enter the numerical value to 3 significant figures, without units. (You may enter the value using E-format scientific notation, e.g., 1.23×10-4 would be entered as 1.23E-4 -- no spaces, capital E.)

5) A 100.0 mL sample of 0.18 M HClO4 is titrated with 0.27 M LiOH. Determine...

5) A 100.0 mL sample of 0.18 M HClO4 is titrated with 0.27 M LiOH. Determine the pH of the solution a) before the addition of any LiOH. b) after the addition of 30.0 mL of LiOH. c) after the addition of 50.0 mL of LiOH. d) after the addition of 66.67 mL of LiOH (this is the equivalence point). e) after the addition of 75.0 mL of LiOH.

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