Question

You are titrating 100.0 mL of 0.0200 M Fe3+ in 1 M HClO4 with a titrant solution of 0.100 M Cu+ to give Fe2+ and Cu2+ (E0 Cu2+/Cu+= 0.161V; E0 Fe3+/Fe2+= 0.767V).

What is the cell potential after pouring 10.0mL of titrant?

Answer #1

Applying Nernst equation:

E_{cell} = E^{o}_{cell} -
(0.0591/n)logQ

= 0.606 - (0.0591/1)log(0.0091)

= 0.485 V

So, answer is 0.485 V

You are titrating 50.00 mL of a 0.161 M formic acid solution
with 0.2949 M sodium hydroxide. Calculate the pH of the solution
after adding 46.94 mL of titrant.

Question1: A 100.0 mL solution of 0.5
M histidine in its tribasic form, A3-, (pKa1
= 1.70, pKa2 = 6.02, pKa3 = 9.08) is titrated
with 1.0 M HCl titrant.
1)calculate the volume of titrant required to reach the second
equivalence point,
2)calculate the pH after the addition of 50.0 mL of titrant,
3)calculate the pH after the addition of 62.0 mL of titrant,
4)calculate the pH after the addition of 75.0 mL of titrant.
Question4: A 100 mL volume...

1- 30.00 mL of sodium sulfite solution are titrated by 45.78 mL
of 0.000983 M potassium dichromate in the presence of sulfuric
acid, generating sulfate and chromium (III) ions. Determine the
balanced net ionic equation for the titration, and calculate the
molarity of the sodium sulfite solution.
2- A voltaic cell is constructed at 25˚C using half cell couples
of Fe3+/Fe2+ with 1.00M/0.100 M concentrations and MnO4 - /Mn2+ at
1.00x10-2 M/1.00x10-4 M concentrations in an acidic solution of
1x10-3...

1. A 100.0-mL sample of 0.500 M sodium hydroxide is titrated
with 0.100 M nitric acid. Calculate the pH before the titration
begins.
2. A 1.0-L buffer solution contains 0.100 mol HCN and 0.100 mol
LiCN. The value of Ka for HCN is 4.9 x 10-10. Because the initial
amounts of acid and conjugate base are equal, the pH of the buffer
is equal to pKa = -log (4.9 x 10-10) = 9.31. Calculate the new pH
after the addition...

Calculate the change in pH when 4.00 mL of 0.100 M HCl(aq) is
added to 100.0 mL of a buffer solution that is 0.100 M in NH3(aq)
and 0.100 M in NH4Cl(aq). (Could you please show work, thank
you!

For the titration of 25 mL of 0.050 M Sn+2 with 0.100 M Fe+3 in
1 M HCl using a Pt electrode and a calomel reference electrode,
what is the potential after 25 mL of titrant has been added?

Consider the following redox reaction between 50. mL of a 0.0500
M Sn2+ solution with 0.100 M Tl3+ if the solution is in a 1.0 M HCl
solution (you can disregard the HCl, it’s acting as an
electrolyte).
1. Write out your balanced reaction ensuring you’re taking into
account the electrons being transferred
2. Determine the volume of thallium needed to reach the
equivalence point.
3. Determine the standard potential of the cell
4. Setup a data table determining the...

1) Balance the reaction Fe2+ + MnO4– → Fe3+ + Mn2+ in acidic
solution. What is the correct coefficient for Fe2+ when the
smallest whole number coefficients are used?
2) Balance the reaction Fe2+ + H2O2 → Fe3+ + H2O in acidic
solution. How many electrons are exchanged when the smallest whole
number coefficients are used?
3) Balance the reaction Cu + HNO3 → Cu2+ + NO in acidic
solution. What is the correct coefficient for NO when the smallest...

.Consider the titration of 100.0 mL of 0.100 M H2NNH2
(Kb=3.0E-6) by 0.200 M HNO3. Calculate the pH of the resulting
solution after the following volumes of HNO3 have been added.
A) 0.0 mL B) 20.0 mL C) 25.0 mL D) 40.0 mL E) 50.0 mL F)100.0
mL

Consider titration of 100.0 mL of 0.100 M H2NNH2 (Kb =
3.5x10^-6) by 0.200 M HNO3? Calculate the pH of the resulting
solution after the following volumes of HNO3 have been added.
0.0 mL
20.0 mL
25.0 mL
40.0 mL
50.0 mL
100.0 ml
Can anyone answer this thouroughly please? Please be sure to
show every step of the math, that us were I tend to get lost. Thank
you!

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