The pKsp of AgI is 16-07- If the E- value for Ag-Ag is 0-7991 V- If the E- for the half cell reaction AgI-e- Ag-I- in Volts is 149 -10-x- then what is the value of x-

The expression for the standard emf of the cell is E^0_I^ |AgI|Ag=E^0_Ag^+|Ag+0.0592log K_sp=E^0_Ag^+|Ag 0.0592pKsp=0.7991 0.0592 × 16.07= 0.149 V ...

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Standard XII

Chemistry

Primary Cells

The pKsp of...

Question

The $p K_{s p}$ of AgI is 16.07. If the $E^{\circ}$ value for $A g^{+} / A g$ is 0.7991 V, If the $E^{\circ}$ for the half cell reaction $A g I + e^{-} \to A g + I^{-}$ , in Volts is $149 \times 10^{- x}$ , then what is the value of x?

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Solution

The expression for the standard emf of the cell is
$E_{I^{-} | A g I | A g}^{0} = E_{A g^{+} | A g}^{0} + 0.0592 l o g K_{s p} = E_{A g^{+} | A g}^{0} - 0.0592 p K s p = 0.7991 - 0.0592 \times 16.07 = - 0.149 V$

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Similar questions

Q. The

p K_{s p}

A g I

is 16.07. If the

E^{\circ}

value for

A g^{+} | A g

is 0.7991 V. find the

E^{\circ}

for the half cell recation

A g I / (s) + e^{-} \to A g + I

Given the data $25^{0} C$

A g + I^{-} \to A g I + e^{-}, E^{0} = 0.152 V

A g \to A g^{+} e^{-}, E^{0} = 0.800 V

What is the value of log $K_{s p}$ for AgI?

Q. Given the data at

25^{0} C

A g + I^{-} \to A g I + e^{-}; E^{0} = 0.152 V

A g \to A g^{+} + e^{-}; E^{0} = - 0.800 V

What is the value of log

K_{s p}

for

A g I

(G i v e n : 2.303 R T / F = 0.059 V)

Q. Calculate the solubility product constant of

A g I

from the following values of standard electrode potentials.

E_{A g^{+} / A g}^{\circ} = 0.80 v o l t

and

E_{I / A g I / A g}^{\circ} = - 0.15 v o l t

25^{\circ} C

Q. Given the data at

25^{o}

A g_{(s)} + I_{(a q)} \to A g I_{(s)} + e^{-}, E^{o} = 0.152

A g_{(s)} \to A g_{(a q)}^{+} + e^{-}, E^{o} = - 0.800

What is the value of log

K_{s p}

for AgI?

(W h e r e K_{s p} = solubility product, 2.303 \frac{R T}{F} = 0.059 V)

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The pKsp of AgI is 16.07. If the E∘ value for Ag+/Ag is 0.7991 V, If the E∘ for the half cell reaction AgI+e−→Ag+I−, in Volts is 149×10−x, then what is the value of x?

The expression for the standard emf of the cell is E0I−|AgI|Ag=E0Ag+|Ag+0.0592logKsp=E0Ag+|Ag−0.0592pKsp=0.7991−0.0592×16.07=−0.149V

The $p K_{s p}$ of AgI is 16.07. If the $E^{\circ}$ value for $A g^{+} / A g$ is 0.7991 V, If the $E^{\circ}$ for the half cell reaction $A g I + e^{-} \to A g + I^{-}$ , in Volts is $149 \times 10^{- x}$ , then what is the value of x?

The expression for the standard emf of the cell is
$E_{I^{-} | A g I | A g}^{0} = E_{A g^{+} | A g}^{0} + 0.0592 l o g K_{s p} = E_{A g^{+} | A g}^{0} - 0.0592 p K s p = 0.7991 - 0.0592 \times 16.07 = - 0.149 V$