150 ml M/10 Ba(MnO4)2 in acidic medium can oxidise what?
150 ml 1 M Fe+
50 ml 1 M FeCro4
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To determine what can be oxidized by a 150 ml M/10 Ba(MnO4)2 solution in acidic medium, we need to understand the characteristics and redox properties of Ba(MnO4)2.
Ba(MnO4)2 is a compound composed of barium cations (Ba2+) and permanganate anions (MnO4-). The permanganate anion is a strong oxidizing agent, meaning it has a high tendency to accept electrons during a redox reaction. In acidic medium, Ba(MnO4)2 dissociates to release MnO4- ions as the active oxidizing species.
MnO4- ions can oxidize substances that have lower reduction potentials, meaning substances that can be easily oxidized by MnO4- ions. Generally, MnO4- ions are capable of oxidizing a wide range of organic and inorganic compounds.
In an acidic medium, MnO4- ions are commonly used to oxidize:
1. Organic compounds: MnO4- can oxidize various organic compounds, such as alcohols, aldehydes, and ketones, to the corresponding carboxylic acids.
2. Inorganic compounds: MnO4- ions can oxidize certain inorganic compounds, including sulfite ions (SO3^2-) to sulfate ions (SO4^2-), iodide ions (I-) to iodine (I2), and iron(II) ions (Fe2+) to iron(III) ions (Fe3+).
It's important to note that the specific compound that Ba(MnO4)2 can oxidize depends on the reaction conditions and the presence of other reagents or substrates. The reactivity and selectivity of MnO4- ions can vary depending on the specific situation.
Therefore, to determine the precise compound that can be oxidized by a 150 ml M/10 Ba(MnO4)2 solution in acidic medium, it is necessary to consider the specific reaction conditions and consult relevant references or experimental data.