Question

The following galvanic cell has a potential of 0.578 v at 25 degress C: Ag(s) | AgCl(s) | Cl- (1.0 M) | |Ag+ (1.0 M) | Ag(s). Use this information to calculate Ksp for AgCl at 25 degrees C.

**Please answer the following questions:**

**The constant 0.0592 volts combines 2.303, __________
J/mole/K for R, __________ K for temperature, and __________C/mole
for F.**

**The value for the solubility product constant is
___________ (2 significant figures)**

Answer #1

Predict the potential for the following voltaic cell at 25 C:
Cu(s)|CuSO4(0.42 M)||AgNO3(0.46 M)|Ag(s) (answer in volts)

1. AgCl (s) <-> Ag+ (aq) + Cl- (aq) Ksp = 1.8 x 10^-10
Ag+ (aq) + 2S2O3^2- (aq) <-> Ag(S2O3)2^3- Kf = 2.9 x
10^13
Consider the two above equilibria. If sodium thiosulfate
solution were added to a solution containing the silver chloride
equilirbium (first equilibrium above) the silver chloride
equilibrium would shift toward the reactants (TRUE OR FALSE)
2. AgCl (s) <-> Ag+ (aq) +
Cl- (aq) Ksp = 1.8 x 10^-10
Ag+ (aq) + 2S2O3^2- (aq) <->...

What is the cell potential of the following voltaic cell if the
Ksp of Ag2SO4 is 1.4x10−5?
Cu(s) | Cu+(1.0 M) || Ag+(Saturated
Ag2SO4) | Ag(s)
The answer is 0.19 V , please explain how and step by step.

Q. Hg|Hg2Cl2(s), KCl(aq,saturated)||KCl(aq, 0.08 M),
AgCl(s)|Ag
(emf was observed at 0.051 V at room temperature,
Standard potential of the Ag/AgCl electrode with 0.08 M KCl =
0.222 V)
Calculate the activity coefficient of Cl- in 0.08 M
KCl(aq) in the cell.

Given a potential of 0.456 V, for the following electrochemical
cell, what is the concentration of Ag+?
Cu2+(aq) (1.0 M)|Cu(s)||Ag+(aq)|Ag(s)

Pb2+ + 2 e- → Pb (s)
ξo = -0.13 V
Ag+ + 1 e- → Ag (s)
ξo = 0.80 V
What is the voltage, at 298 K, of this voltaic cell starting with
the following non-standard concentrations:
[Pb2+] (aq) = 0.065 M
[Ag+] (aq) = 0.93 M
Use the Nernst equation:
ξ = ξo - (RT/nF) ln Q
First calculate the value of Q, and enter it into the first
answer box. Q is dimensionless.
Then calculate ξ,...

At 25 °C, you conduct a titration of 15.00 mL of a 0.0460 M
AgNO3 solution with a 0.0230 M NaI solution within the following
cell: Saturated Calomel Electrode || Titration Solution | Ag
(s)
For the cell as written, what is the voltage after the addition
of the following volume of NaI solution? The reduction potential
for the saturated calomel electrode is E = 0.241 V. The standard
reduction potential for the reaction
Ag+ + e- --> Ag(s)
is...

1. Calculate the equilibrium constant, K, for the reaction in
the Galvanic Pb-Cu cell. (Report your answer in scientific notation
to three significant figures. Use * for the multiplication sign and
^ to designate the exponent.) Cu+ (aq) + Pb (s) → Cu (s) + Pb2+
(aq) Eocell = 0.647 V
K =
2. For the reaction Mg (s) + Ni2+ (aq) →→
Mg2+ (aq) + Ni (s),
Eocell = 2.629 V.
Calculate the cell potential at T = 50.0oC...

Pb2+ + 2 e- → Pb (s)
ξo = -0.13 V
Ag+ + 1 e- → Ag (s)
ξo = 0.80 V
What is the voltage, at 298 K, of this voltaic cell starting with
the following non-standard concentrations:
[Pb2+] (aq) = 0.109 M
[Ag+] (aq) = 1.01 M
Use the Nernst equation:
ξ = ξo - (RT/nF) ln Q
First calculate the value of Q, and enter it into the first answer
box. Q is dimensionless.
Then calculate ξ,...

For the following cell at 25 Celsius:
Ag+ +e—>Ag(s)=0.80V
Cu2+ +2e—>Cu(s)=0.34V
(Cu(s)|CuCl2(aq)||AgNO3(aq)|Ag(s))
1) what is the equilibrium constant under standard
conditions?
2)what is the cell potential if the concentration of the AgNO3
solution was changed to 0.500 M, and all other conditions remained
the same?
3)Calculate delta Grxn for part 2

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