A concentration cell consists of two half-cells with identical electrodes but different ion concentrations. Consider the following concentration cell (pictured below). M(s) | M*(satd MX) || M*(0.100 M)| M(s) Ecell = 0.417 V At the anode, a metal electrode (M) is placed in a saturated aqueous solution containing ions of the same metal (M) and a halogen (X), MX. At the cathode, a second electrode of the same metal (M) is placed in a solution with [M*] = 0.100 M.The two half-cells are connected by a salt bridge, and the measured cell voltage is 0.417 V. The cell reaction occurring in this concentration cell is Reduction: M*(0.100 M) + e → M(s) Oxidation: M(s) → M*(satd MX) + e From this information, calculate the Ksp of MX. NOTE: You may enter a number in scientific notation as: 6.6E-66 or 6.66*10^-66 or 6.66x10^-66 (DO NOT ADD Spaces) Anode MX(s) MX (sat'd aq) 0.417 Voltmeter Salt bridge KNO,(aq) M Cathode M*(0.100M)
A concentration cell consists of two half-cells with identical electrodes but different ion concentrations. Consider the following concentration cell (pictured below). M(s) | M*(satd MX) || M*(0.100 M)| M(s) Ecell = 0.417 V At the anode, a metal electrode (M) is placed in a saturated aqueous solution containing ions of the same metal (M) and a halogen (X), MX. At the cathode, a second electrode of the same metal (M) is placed in a solution with [M*] = 0.100 M.The two half-cells are connected by a salt bridge, and the measured cell voltage is 0.417 V. The cell reaction occurring in this concentration cell is Reduction: M*(0.100 M) + e → M(s) Oxidation: M(s) → M*(satd MX) + e From this information, calculate the Ksp of MX. NOTE: You may enter a number in scientific notation as: 6.6E-66 or 6.66*10^-66 or 6.66x10^-66 (DO NOT ADD Spaces) Anode MX(s) MX (sat'd aq) 0.417 Voltmeter Salt bridge KNO,(aq) M Cathode M*(0.100M)
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![A concentration cell consists of two half-cells with identical electrodes but different ion concentrations.
Consider the following concentration cell (pictured below).
M(s) | M*(satd MX) || M+ (0.100 M)| M(s) Ecell = 0.417 V
At the anode, a metal electrode (M) is placed in a saturated aqueous solution containing ions of the same metal (M) and a halogen
(X), MX. At the cathode, a second electrode of the same metal (M) is placed in a solution with [M*] = 0.100 M.The two half-cells are
connected by a salt bridge, and the measured cell voltage is 0.417 V. The cell reaction occurring in this concentration cell is
Reduction: M*(0.100 M) + e → M(s)
Oxidation: M(s) → M*(satd MX) + e*
From this information, calculate the Ksp of MX.
NOTE: You may enter a number in scientific notation as: 6.6E-66 or 6.66*10^-66 or 6.66x10^-66 (DO NOT ADD Spaces)
Anode
M
MX(s)
MX (sat'd aq)
0.417
Voltmeter
Salt bridge
KNO3(aq)
Cathode
M+ (0.100M)](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F07d44ac4-a3f5-428d-bcfb-1c7dbd317829%2F2ee6e9b6-bcd1-4810-8a3e-6ab3ea8c21f7%2Fmemslqi_processed.png&w=3840&q=75)
Transcribed Image Text:A concentration cell consists of two half-cells with identical electrodes but different ion concentrations.
Consider the following concentration cell (pictured below).
M(s) | M*(satd MX) || M+ (0.100 M)| M(s) Ecell = 0.417 V
At the anode, a metal electrode (M) is placed in a saturated aqueous solution containing ions of the same metal (M) and a halogen
(X), MX. At the cathode, a second electrode of the same metal (M) is placed in a solution with [M*] = 0.100 M.The two half-cells are
connected by a salt bridge, and the measured cell voltage is 0.417 V. The cell reaction occurring in this concentration cell is
Reduction: M*(0.100 M) + e → M(s)
Oxidation: M(s) → M*(satd MX) + e*
From this information, calculate the Ksp of MX.
NOTE: You may enter a number in scientific notation as: 6.6E-66 or 6.66*10^-66 or 6.66x10^-66 (DO NOT ADD Spaces)
Anode
M
MX(s)
MX (sat'd aq)
0.417
Voltmeter
Salt bridge
KNO3(aq)
Cathode
M+ (0.100M)
Expert Solution
Step 1
In a concentration cell, the electricity is generated due to the potential difference created by the difference in the concentration of both the half-cells.
Given the potential of the concentration cell, Ecell = 0.417 V
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