The standard reduction potentials of Cu2+ and Ag+ in V are +0.34 and +0.80; resp

Question

The standard reduction potentials of Cu2+ and Ag+ in V are +0.34 and +0.80; respectively. Determine the value of E (in V) for the following cell at 25 Degree C. Cu | Cu2+ (1.00 M) || Ag+(0.0010 M) | Ag Given the following information determine which of the following actions would change the measured cell potential. increasing the pH in the cathode compartment lowering the pH in the cathode compartment increasing the tin(II) ion concentration increasing the pressure of hydrogen gas in the hydrogen cell any of these things will change the measured cell potential Consider the following electrochemical cell at 298 K. One compartment contains a 1.00-M solution of silver nitrate. The other compartment contains a saturated solution of silver iodide. Both electrodes are silver and the measured potential is 0.476 V. From this information, determine the molar solubility of silver iodide at 298 K.

Explanation / Answer

18) c = 0.37

19)c = increase Sn(ii) concentration

   Since reduction potential of Hydrogen zero alteriing Hydrogen concentration will not change any effect

20) c = 9.11*10-9

The dissociation equation for AgI is:

AgI (s) <===> Ag+ (aq) + I (aq)

The Ksp expression is:

Ksp = [Ag+] [I]

This is the equation we must solve. First we put in the Ksp value:

Ecell = E - (0.0591 / n) log K

0 = -0.476 - (0.0591/1)log KSP

logKsp = -0.476/0.0591

Ksp = 9.1182*10-9

Ksp = [Ag+][I-]

Solubility of AgI    = KSP/concentration of Ag+

= 9.11*10-9/1

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