The other answers focus on how FeSO[math]_4[/math] is manufactured (usually H[math]_2[/math]SO[math]_4[/math] and Fe(s)) but I think that this question is asking how the actual FeSO[math]_4[/math] solution is made.
The answer seems obvious, but it is not. Simply adding FeSO[math]_4[/math] to water is not an appropriate way to make a solution of FeSO[math]_4[/math]. To prove this, do the following. Add FeSO[math]_4[/math] to any volume of water and then add a small amount of KSCN. The solution will turn a reddish color, why? Because FeSO[math]_4[/math] immediately begins to disproportionate by the following reaction.
Iron (III) reacts with the SCN- ion to make the FeSCN[math]^{2+}[/math] complex ion which is red. As a consequence, it is well known that FeSO[math]_4[/math] solutions are not stable. To help stabilize this solution we need to force the disproportionation reaction backwards towards the Fe[math]^{2+}[/math] ion. To do this, solutions of FeSO[math]_4[/math] are always made acidic by adding H[math]_2[/math]SO[math]_4[/math] to them (about 3 M H[math]_2[/math]SO[math]_4[/math] ) and a chunk of iron is added to help move the reaction towards the formation of FeSO[math]_4[/math].
So, when we make FeSO[math]_4[/math] solutions, they are acidified with H[math]_2[/math]SO[math]_4[/math] and a chunk of iron is added to help stabilize the solution.
The other answers focus on how FeSO[math]_4[/math] is manufactured (usually H[math]_2[/math]SO[math]_4[/math] and Fe(s)) but I think that this question is asking how the actual FeSO[math]_4[/math] solution is made.
The answer seems obvious, but it is not. Simply adding FeSO[math]_4[/math] to water is not an appropriate way to make a solution of FeSO[math]_4[/math]. To prove this, do the following. Add FeSO[math]_4[/math] to any volume of water and then add a small amount of KSCN. The solution will turn a reddish color, why? Because FeSO[math]_4[/math] immediately begins to disproportionate by the following reaction.
Iron (III) reacts with the SCN- ion to make the FeSCN[math]^{2+}[/math] complex ion which is red. As a consequence, it is well known that FeSO[math]_4[/math] solutions are not stable. To help stabilize this solution we need to force the disproportionation reaction backwards towards the Fe[math]^{2+}[/math] ion. To do this, solutions of FeSO[math]_4[/math] are always made acidic by adding H[math]_2[/math]SO[math]_4[/math] to them (about 3 M H[math]_2[/math]SO[math]_4[/math] ) and a chunk of iron is added to help move the reaction towards the formation of FeSO[math]_4[/math].
So, when we make FeSO[math]_4[/math] solutions, they are acidified with H[math]_2[/math]SO[math]_4[/math] and a chunk of iron is added to help stabilize the solution.
FeSO4 is a soluble salt. So eliminate precipitation.
It is not a group one or ammonium salt so eliminate titration.
We are left with reacting excess metal, base or carbonate with acid. You could react iron hydroxide/oxide/carbonate or just iron metal with sulfuric acid. You would be able to prepare the iron sulfate salt.
FeSO4 is a soluble salt. So eliminate precipitation.
It is not a group one or ammonium salt so eliminate titration.
We are left with reacting excess metal, base or carbonate with acid. You could react iron hydroxide/oxide/carbonate or just iron metal with sulfuric acid. You would be able to prepare the iron sulfate salt.
Because if FeSO⁴ is stored or it is the old one then it reacts with atmospheric oxygen and gets oxidized to form a corrosive brown-yellow coating of basic ferric sulphate, which is an adduct of ferric oxide and ferric sulphate.
Because if FeSO⁴ is stored or it is the old one then it reacts with atmospheric oxygen and gets oxidized to form a corrosive brown-yellow coating of basic ferric sulphate, which is an adduct of ferric oxide and ferric sulphate.
When you heat sulfates, nitrates, phosphates and all other oxoacids salts, the outcome is always that you obtain the metal and the non metal oxides. So, if you heat FeSO, you will obtain FeO and SO3. The first is a salt and the second a gas that will be released in the form of a reddish vapour. If you do this experiment (which you can, it is not dangerous at all) do so in a very ventilated room so you don't inhale the gases.
Using further heating you could even manage to separate Fe and Oxygen, but you would need a hell of a furnace for that. It only occurs at about 5000 K.
When you heat sulfates, nitrates, phosphates and all other oxoacids salts, the outcome is always that you obtain the metal and the non metal oxides. So, if you heat FeSO, you will obtain FeO and SO3. The first is a salt and the second a gas that will be released in the form of a reddish vapour. If you do this experiment (which you can, it is not dangerous at all) do so in a very ventilated room so you don't inhale the gases.
Using further heating you could even manage to separate Fe and Oxygen, but you would need a hell of a furnace for that. It only occurs at about 5000 K.
The compound is also referred to as ferrous sulfate. The name of FeSO4 is Ferrous sulphate as it contains iron and sulphate ions. FeSO4 is ferrous sulphate or iron (II) sulphate.
The compound is also referred to as ferrous sulfate. The name of FeSO4 is Ferrous sulphate as it contains iron and sulphate ions. FeSO4 is ferrous sulphate or iron (II) sulphate.
The metal will react directly with dilute H2SO4 to produce ferrous sulphate & hydrogen gas. Alternatively, you can oxidise iron pyrite FeS2 using water and oxygen (which is the commercial production route):
The metal will react directly with dilute H2SO4 to produce ferrous sulphate & hydrogen gas. Alternatively, you can oxidise iron pyrite FeS2 using water and oxygen (which is the commercial production route):
FeSO4.7H20 is chemical formula of ferrous sulphate heptahydrate..It is also called green vitriol..It is blue green in colour.
On heating, iron(II) sulphate first loses its water of crystallization and the original green crystals are converted into a brown colored anhydrous solid. When further heated, the anhydrous material releases sulphur dioxide and white fumes of sulphur trioxide, leaving a reddish-brown iron(III) oxide.
FeSO4.7H20 is chemical formula of ferrous sulphate heptahydrate..It is also called green vitriol..It is blue green in colour.
On heating, iron(II) sulphate first loses its water of crystallization and the original green crystals are converted into a brown colored anhydrous solid. When further heated, the anhydrous material releases sulphur dioxide and white fumes of sulphur trioxide, leaving a reddish-brown iron(III) oxide.
FeSO4 is green crystals usually their surfaces are covered with the brown Fe2O3 due to oxidation of Fe(II) to Fe(III). So, preparation of a fresh FeSO4 solution involves washing some crystals of ferrous sulphate with some distilled water to remove the the brown Fe2O3, to get the pure green FeSO4 before dissolving it in fresh distilled water with a few drops of Dil H2SO4 to prevent the hydrolysis of ferrous sulphate in solution.
FeSO4 is green crystals usually their surfaces are covered with the brown Fe2O3 due to oxidation of Fe(II) to Fe(III). So, preparation of a fresh FeSO4 solution involves washing some crystals of ferrous sulphate with some distilled water to remove the the brown Fe2O3, to get the pure green FeSO4 before dissolving it in fresh distilled water with a few drops of Dil H2SO4 to prevent the hydrolysis of ferrous sulphate in solution.
The first one is dehydrated salt but the other one is hydrated salt with each mole of feso4 having 7h2o molecules and it is green in colour.
The first one is dehydrated salt but the other one is hydrated salt with each mole of feso4 having 7h2o molecules and it is green in colour.
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The other answers focus on how FeSO[math]_4[/math] is manufactured (usually H[math]_2[/math]SO[math]_4[/math] and Fe(s)) but I think that this question is asking how the actual FeSO[math]_4[/math] solution is made.
The answer seems obvious, but it is not. Simply adding FeSO[math]_4[/math] to water is not an appropriate way to make a solution of FeSO[math]_4[/math]. To prove this, do the following. Add FeSO[math]_4[/math] to any volume of water and then add a small amount of KSCN. The solution will turn a reddish color, why? Because FeSO[math]_4[/math] immediately begins to disproportionate by the following reaction.
3 Fe[math]^{2+} [/math]→ 2 Fe[math]^{3+}[/math] + Fe(s)
Iron (III) reacts with the SCN- ion to make the FeSCN[math]^{2+}[/math] complex ion which is red. As a consequence, it is well known that FeSO[math]_4[/math] solutions are not stable. To help stabilize this solution we need to force the disproportionation reaction backwards towards the Fe[math]^{2+}[/math] ion. To do this, solutions of FeSO[math]_4[/math] are always made acidic by adding H[math]_2[/math]SO[math]_4[/math] to them (about 3 M H[math]_2[/math]SO[math]_4[/math] ) and a chunk of iron is added to help move the reaction towards the formation of FeSO[math]_4[/math].
So, when we make FeSO[math]_4[/math] solutions, they are acidified with H[math]_2[/math]SO[math]_4[/math] and a chunk of iron is added to help stabilize the solution.
The other answers focus on how FeSO[math]_4[/math] is manufactured (usually H[math]_2[/math]SO[math]_4[/math] and Fe(s)) but I think that this question is asking how the actual FeSO[math]_4[/math] solution is made.
The answer seems obvious, but it is not. Simply adding FeSO[math]_4[/math] to water is not an appropriate way to make a solution of FeSO[math]_4[/math]. To prove this, do the following. Add FeSO[math]_4[/math] to any volume of water and then add a small amount of KSCN. The solution will turn a reddish color, why? Because FeSO[math]_4[/math] immediately begins to disproportionate by the following reaction.
3 Fe[math]^{2+} [/math]→ 2 Fe[math]^{3+}[/math] + Fe(s)
Iron (III) reacts with the SCN- ion to make the FeSCN[math]^{2+}[/math] complex ion which is red. As a consequence, it is well known that FeSO[math]_4[/math] solutions are not stable. To help stabilize this solution we need to force the disproportionation reaction backwards towards the Fe[math]^{2+}[/math] ion. To do this, solutions of FeSO[math]_4[/math] are always made acidic by adding H[math]_2[/math]SO[math]_4[/math] to them (about 3 M H[math]_2[/math]SO[math]_4[/math] ) and a chunk of iron is added to help move the reaction towards the formation of FeSO[math]_4[/math].
So, when we make FeSO[math]_4[/math] solutions, they are acidified with H[math]_2[/math]SO[math]_4[/math] and a chunk of iron is added to help stabilize the solution.
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K2Cr2O7 = 294 g/mol
equive weight = 294/6 = 49 in a solution
0.1 N = X/49 / V
1 L???
4.9 g mixed with 1 L water
K2Cr2O7 = 294 g/mol
equive weight = 294/6 = 49 in a solution
0.1 N = X/49 / V
1 L???
4.9 g mixed with 1 L water
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Because if FeSO⁴ is stored or it is the old one then it reacts with atmospheric oxygen and gets oxidized to form a corrosive brown-yellow coating of basic ferric sulphate, which is an adduct of ferric oxide and ferric sulphate.
Thus the brown ring will not be formed.
Because if FeSO⁴ is stored or it is the old one then it reacts with atmospheric oxygen and gets oxidized to form a corrosive brown-yellow coating of basic ferric sulphate, which is an adduct of ferric oxide and ferric sulphate.
Thus the brown ring will not be formed.
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When you heat sulfates, nitrates, phosphates and all other oxoacids salts, the outcome is always that you obtain the metal and the non metal oxides. So, if you heat FeSO, you will obtain FeO and SO3. The first is a salt and the second a gas that will be released in the form of a reddish vapour. If you do this experiment (which you can, it is not dangerous at all) do so in a very ventilated room so you don't inhale the gases.
Using further heating you could even manage to separate Fe and Oxygen, but you would need a hell of a furnace for that. It only occurs at about 5000 K.
When you heat sulfates, nitrates, phosphates and all other oxoacids salts, the outcome is always that you obtain the metal and the non metal oxides. So, if you heat FeSO, you will obtain FeO and SO3. The first is a salt and the second a gas that will be released in the form of a reddish vapour. If you do this experiment (which you can, it is not dangerous at all) do so in a very ventilated room so you don't inhale the gases.
Using further heating you could even manage to separate Fe and Oxygen, but you would need a hell of a furnace for that. It only occurs at about 5000 K.
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The compound is also referred to as ferrous sulfate. The name of FeSO4 is Ferrous sulphate as it contains iron and sulphate ions. FeSO4 is ferrous sulphate or iron (II) sulphate.
The compound is also referred to as ferrous sulfate. The name of FeSO4 is Ferrous sulphate as it contains iron and sulphate ions. FeSO4 is ferrous sulphate or iron (II) sulphate.
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The metal will react directly with dilute H2SO4 to produce ferrous sulphate & hydrogen gas. Alternatively, you can oxidise iron pyrite FeS2 using water and oxygen (which is the commercial production route):
2 FeS2 + 7O2 + 2H2O → 2FeSO4 + 2H2SO4
The metal will react directly with dilute H2SO4 to produce ferrous sulphate & hydrogen gas. Alternatively, you can oxidise iron pyrite FeS2 using water and oxygen (which is the commercial production route):
2 FeS2 + 7O2 + 2H2O → 2FeSO4 + 2H2SO4
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FeSO4.7H20 is chemical formula of ferrous sulphate heptahydrate..It is also called green vitriol..It is blue green in colour.
On heating, iron(II) sulphate first loses its water of crystallization and the original green crystals are converted into a brown colored anhydrous solid. When further heated, the anhydrous material releases sulphur dioxide and white fumes of sulphur trioxide, leaving a reddish-brown iron(III) oxide.
2 FeSO4 → Fe2O3 + SO2 + SO3
Hope it is helpful..
Thank you..
FeSO4.7H20 is chemical formula of ferrous sulphate heptahydrate..It is also called green vitriol..It is blue green in colour.
On heating, iron(II) sulphate first loses its water of crystallization and the original green crystals are converted into a brown colored anhydrous solid. When further heated, the anhydrous material releases sulphur dioxide and white fumes of sulphur trioxide, leaving a reddish-brown iron(III) oxide.
2 FeSO4 → Fe2O3 + SO2 + SO3
Hope it is helpful..
Thank you..
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FeSO4 is green crystals usually their surfaces are covered with the brown Fe2O3 due to oxidation of Fe(II) to Fe(III). So, preparation of a fresh FeSO4 solution involves washing some crystals of ferrous sulphate with some distilled water to remove the the brown Fe2O3, to get the pure green FeSO4 before dissolving it in fresh distilled water with a few drops of Dil H2SO4 to prevent the hydrolysis of ferrous sulphate in solution.
FeSO4 is green crystals usually their surfaces are covered with the brown Fe2O3 due to oxidation of Fe(II) to Fe(III). So, preparation of a fresh FeSO4 solution involves washing some crystals of ferrous sulphate with some distilled water to remove the the brown Fe2O3, to get the pure green FeSO4 before dissolving it in fresh distilled water with a few drops of Dil H2SO4 to prevent the hydrolysis of ferrous sulphate in solution.
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