Sodium hypochlorite (NaClO) can act as both an oxidizing agent and a reducing agent.
When the solution of sodium hypochlorite is heated, it undergoes disproportionation (self-redox) to become sodium chloride (reduction) and sodium chlorate (oxidation). 3NaClO(aq) → 2NaCl(aq) + NaClO₃(aq) OR: 3ClO⁻(aq) → 2Cl⁻(aq) + ClO₃⁻(aq)
Sodium hypochlorite (NaClO) can act as both an oxidizing agent and a reducing agent.
When the solution of sodium hypochlorite is heated, it undergoes disproportionation (self-redox) to become sodium chloride (reduction) and sodium chlorate (oxidation). 3NaClO(aq) → 2NaCl(aq) + NaClO₃(aq) OR: 3ClO⁻(aq) → 2Cl⁻(aq) + ClO₃⁻(aq)
Calcium hypochlorite is a toxic substance as is its sister Sodium hypochlorite. Both of these are bleach. The only difference is that Calcium hypochlorite doesn’t smell as much like bleach.
If you are intending to use this as a treatment for COVID-19, DON’T. It is poison. A vaccine is here NOW. There are treatments for patients who have COVID-19. Hang tight, help is almost at your door!
Calcium hypochlorite is a toxic substance as is its sister Sodium hypochlorite. Both of these are bleach. The only difference is that Calcium hypochlorite doesn’t smell as much like bleach.
If you are intending to use this as a treatment for COVID-19, DON’T. It is poison. A vaccine is here NOW. There are treatments for patients who have COVID-19. Hang tight, help is almost at your door!
+1. Work it out like this with the oxidation states:
Ca always has +2 in its compounds;
O always has -2 (unless it is part of a peroxide or a superoxide, very rare).
The sum of the oxidation numbers in a neutral compound must always be zero, therefore you can set a simple, straightforward equation whose unknown value you will solve for is the oxidation number of Cl:
+1. Work it out like this with the oxidation states:
Ca always has +2 in its compounds;
O always has -2 (unless it is part of a peroxide or a superoxide, very rare).
The sum of the oxidation numbers in a neutral compound must always be zero, therefore you can set a simple, straightforward equation whose unknown value you will solve for is the oxidation number of Cl:
Simply put, an oxidising agent is a substance that looks to remove electrons from the substance it is reacting with (i.e oxidise it/increase its oxidation state). A reducing agent by contrast looks to add electrons to its reactant (i.e reduce it/reduce its oxidation state). In each case, the opposite occurs to the agent itself (an oxidising agent is reduced and gains one or more electrons, a reducing agent is oxidised and loses one or more electrons).
Simply put, an oxidising agent is a substance that looks to remove electrons from the substance it is reacting with (i.e oxidise it/increase its oxidation state). A reducing agent by contrast looks to add electrons to its reactant (i.e reduce it/reduce its oxidation state). In each case, the opposite occurs to the agent itself (an oxidising agent is reduced and gains one or more electrons, a reducing agent is oxidised and loses one or more electrons).
Yes. Chlorine is in the +1 oxidation state in the hypochlorite ion (ClO*-). Since the chlorine is easily reduced to the -1 state, the hypochlorite ion acts as an oxidizing agent (i.e., in order to be reduced, the chlorine in the +1 oxidation state must cause something to be oxidized).
Yes. Chlorine is in the +1 oxidation state in the hypochlorite ion (ClO*-). Since the chlorine is easily reduced to the -1 state, the hypochlorite ion acts as an oxidizing agent (i.e., in order to be reduced, the chlorine in the +1 oxidation state must cause something to be oxidized).
Ca(ClO)2. This is the chemical name of calcium hypochlorite.
Ca(ClO)2. This is the chemical name of calcium hypochlorite.
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Sodium hypochlorite (NaClO) can act as both an oxidizing agent and a reducing agent.
When the solution of sodium hypochlorite is heated, it undergoes disproportionation (self-redox) to become sodium chloride (reduction) and sodium chlorate (oxidation).
3NaClO(aq) → 2NaCl(aq) + NaClO₃(aq)
OR: 3ClO⁻(aq) → 2Cl⁻(aq) + ClO₃⁻(aq)
Sodium hypochlorite (NaClO) can act as both an oxidizing agent and a reducing agent.
When the solution of sodium hypochlorite is heated, it undergoes disproportionation (self-redox) to become sodium chloride (reduction) and sodium chlorate (oxidation).
3NaClO(aq) → 2NaCl(aq) + NaClO₃(aq)
OR: 3ClO⁻(aq) → 2Cl⁻(aq) + ClO₃⁻(aq)
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Calcium hypochlorite is a toxic substance as is its sister Sodium hypochlorite. Both of these are bleach. The only difference is that Calcium hypochlorite doesn’t smell as much like bleach.
If you are intending to use this as a treatment for COVID-19, DON’T. It is poison. A vaccine is here NOW. There are treatments for patients who have COVID-19. Hang tight, help is almost at your door!
Calcium hypochlorite is a toxic substance as is its sister Sodium hypochlorite. Both of these are bleach. The only difference is that Calcium hypochlorite doesn’t smell as much like bleach.
If you are intending to use this as a treatment for COVID-19, DON’T. It is poison. A vaccine is here NOW. There are treatments for patients who have COVID-19. Hang tight, help is almost at your door!
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+1. Work it out like this with the oxidation states:
Ca always has +2 in its compounds;
O always has -2 (unless it is part of a peroxide or a superoxide, very rare).
The sum of the oxidation numbers in a neutral compound must always be zero, therefore you can set a simple, straightforward equation whose unknown value you will solve for is the oxidation number of Cl:
+2 + 2x + 2×(-2) = 0
x = +1
+1. Work it out like this with the oxidation states:
Ca always has +2 in its compounds;
O always has -2 (unless it is part of a peroxide or a superoxide, very rare).
The sum of the oxidation numbers in a neutral compound must always be zero, therefore you can set a simple, straightforward equation whose unknown value you will solve for is the oxidation number of Cl:
+2 + 2x + 2×(-2) = 0
x = +1
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Simply put, an oxidising agent is a substance that looks to remove electrons from the substance it is reacting with (i.e oxidise it/increase its oxidation state). A reducing agent by contrast looks to add electrons to its reactant (i.e reduce it/reduce its oxidation state). In each case, the opposite occurs to the agent itself (an oxidising agent is reduced and gains one or more electrons, a reducing agent is oxidised and loses one or more electrons).
Simply put, an oxidising agent is a substance that looks to remove electrons from the substance it is reacting with (i.e oxidise it/increase its oxidation state). A reducing agent by contrast looks to add electrons to its reactant (i.e reduce it/reduce its oxidation state). In each case, the opposite occurs to the agent itself (an oxidising agent is reduced and gains one or more electrons, a reducing agent is oxidised and loses one or more electrons).
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You might try sodium sulphite.
You might try sodium sulphite.
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Yes. Chlorine is in the +1 oxidation state in the hypochlorite ion (ClO*-). Since the chlorine is easily reduced to the -1 state, the hypochlorite ion acts as an oxidizing agent (i.e., in order to be reduced, the chlorine in the +1 oxidation state must cause something to be oxidized).
Yes. Chlorine is in the +1 oxidation state in the hypochlorite ion (ClO*-). Since the chlorine is easily reduced to the -1 state, the hypochlorite ion acts as an oxidizing agent (i.e., in order to be reduced, the chlorine in the +1 oxidation state must cause something to be oxidized).
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Yes, in cold water it gives Ca+2, Cl-, OCl- ions.
Yes, in cold water it gives Ca+2, Cl-, OCl- ions.
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