2MnO₂ + 3S0₂² +20H3SO, +2MnO + H₂O In the above redox reaction, use oxidation numbers to identify the element oxidized, the element reduced, the oxidizing agent and the reducing agent. Name of the element oxidized: Name of the element reduced: Formula of the oxidizing agent: Formula of the reducing agent:

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2MnO₂ + 350,² + 2OH → 3S0₁² + 2MnO4+H₂O
In the above redox reaction, use oxidation numbers to identify the element oxidized, the element reduced, the oxidizing agent and the reducing agent.
Name of the element oxidized:
Name of the element reduced:
Formula of the oxidizing agent:
Formula of the reducing agent:
Transcribed Image Text:2MnO₂ + 350,² + 2OH → 3S0₁² + 2MnO4+H₂O In the above redox reaction, use oxidation numbers to identify the element oxidized, the element reduced, the oxidizing agent and the reducing agent. Name of the element oxidized: Name of the element reduced: Formula of the oxidizing agent: Formula of the reducing agent:
The concentration of Cu in a solution is determined by titrating it with a 0.1993 M permanganate solution. The balanced net ionic equation for the reaction is:
MnO, (aq) + 5Cu (aq) +8H₂O" (aq) →Mn² (aq) + 5Cu² (aq) + 12H₂O(l)
In one experiment, 15.39 mL of the 0.1993 M permanganate solution is required to react completely with 20.00 ml of the Cu solution. Calculate the concentration of the Cu
solution.
Concentration -
M
Transcribed Image Text:The concentration of Cu in a solution is determined by titrating it with a 0.1993 M permanganate solution. The balanced net ionic equation for the reaction is: MnO, (aq) + 5Cu (aq) +8H₂O" (aq) →Mn² (aq) + 5Cu² (aq) + 12H₂O(l) In one experiment, 15.39 mL of the 0.1993 M permanganate solution is required to react completely with 20.00 ml of the Cu solution. Calculate the concentration of the Cu solution. Concentration - M
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