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Why does sodium sulphate form a white precipitate when barium chloride is added to it? Does this show the presence of ions?
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+ Inorganic chemistry
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Posted by
Ludwig Nijholt
Why does sodium sulphate form a white precipitate when barium chloride is added to it? Does this show the presence of ions?
Because what is important is the formation of insoluble BaSO4 which will prove that there was sulphate in the sample being tested. Chloride or nitrate ions are not relevant therefore it doesn’t matter which is used as long as Barium is the cation in the reagent.
Because what is important is the formation of insoluble BaSO4 which will prove that there was sulphate in the sample being tested. Chloride or nitrate ions are not relevant therefore it doesn’t matter which is used as long as Barium is the cation in the reagent.
This reaction takes advantage of the fact that barium sulfate is highly insoluble to drive what what would otherwise be an equilibrium process. The reaction products will be copper(II) chloride, which remains in solution, and barium sulfate, which precipitates as a white solid. The equation is:
This reaction takes advantage of the fact that barium sulfate is highly insoluble to drive what what would otherwise be an equilibrium process. The reaction products will be copper(II) chloride, which remains in solution, and barium sulfate, which precipitates as a white solid. The equation is:
Most sulfates are water-soluble… calcium sulfate is not so soluble, and barium sulfate is as soluble as a brick…the webz quote [math]K_{sp}=4×10^{-10}[/math] for the barium salt…the which corresponds to a mass solubility of [math]approx ext{4•ppm}[/math] … i.e. [math]4•mg•L^{-1}[/math] …
And we could represent the reaction by the equation…
Most sulfates are water-soluble… calcium sulfate is not so soluble, and barium sulfate is as soluble as a brick…the webz quote [math]K_{sp}=4×10^{-10}[/math] for the barium salt…the which corresponds to a mass solubility of [math]approx ext{4•ppm}[/math] … i.e. [math]4•mg•L^{-1}[/math] …
And we could represent the reaction by the equation…
The barium ion reacts with the sulfate ion to form solid barium sulfate, which precipitates because it's insoluble in water.. The sodium and chloride ions remain dissolved in the solution.
The barium ion reacts with the sulfate ion to form solid barium sulfate, which precipitates because it's insoluble in water.. The sodium and chloride ions remain dissolved in the solution.
There is the possibility that the chloride ion will form a precipitate with metals (silver, lead, mercury, and to a lesser extent copper) and give a false positive result, while nitrates are always soluble.
There is the possibility that the chloride ion will form a precipitate with metals (silver, lead, mercury, and to a lesser extent copper) and give a false positive result, while nitrates are always soluble.
In general, the only ions which are coloured are the transition metals - the reason for that is rather more complex than I feel like going in to this morning. However, since Ba is not a transition metal, and sulphate is also not a coloured ion, the solid that settles out is white.
Remember: If you are not part of the solution, you are part of the precipitate!
In general, the only ions which are coloured are the transition metals - the reason for that is rather more complex than I feel like going in to this morning. However, since Ba is not a transition metal, and sulphate is also not a coloured ion, the solid that settles out is white.
Remember: If you are not part of the solution, you are part of the precipitate!
Because what is important is the formation of insoluble BaSO4 which will prove that there was sulphate in the sample being tested. Chloride or nitrate ions are not relevant therefore it doesn’t matter which is used as long as Barium is the cation in the reagent.
Because what is important is the formation of insoluble BaSO4 which will prove that there was sulphate in the sample being tested. Chloride or nitrate ions are not relevant therefore it doesn’t matter which is used as long as Barium is the cation in the reagent.
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This reaction takes advantage of the fact that barium sulfate is highly insoluble to drive what what would otherwise be an equilibrium process. The reaction products will be copper(II) chloride, which remains in solution, and barium sulfate, which precipitates as a white solid. The equation is:
CuSO4 + BaCl2 → CuCl2 + BaSO4
This reaction takes advantage of the fact that barium sulfate is highly insoluble to drive what what would otherwise be an equilibrium process. The reaction products will be copper(II) chloride, which remains in solution, and barium sulfate, which precipitates as a white solid. The equation is:
CuSO4 + BaCl2 → CuCl2 + BaSO4
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Most sulfates are water-soluble… calcium sulfate is not so soluble, and barium sulfate is as soluble as a brick…the webz quote [math]K_{sp}=4×10^{-10}[/math] for the barium salt…the which corresponds to a mass solubility of [math]approx ext{4•ppm}[/math] … i.e. [math]4•mg•L^{-1}[/math] …
And we could represent the reaction by the equation…
[math]BaCl_{2}(aq) + Na_{2}SO_{4}(aq) longrightarrow BaSO_{4}(s)downarrow+2NaCl(aq)[/math]
…else, the net ionic equation…
[math]Ba^{2+} + SO_{4}^{2-} longrightarrow BaSO_{4}(s)downarrow[/math]
…does this show the presence of ions…?
Most sulfates are water-soluble… calcium sulfate is not so soluble, and barium sulfate is as soluble as a brick…the webz quote [math]K_{sp}=4×10^{-10}[/math] for the barium salt…the which corresponds to a mass solubility of [math]approx ext{4•ppm}[/math] … i.e. [math]4•mg•L^{-1}[/math] …
And we could represent the reaction by the equation…
[math]BaCl_{2}(aq) + Na_{2}SO_{4}(aq) longrightarrow BaSO_{4}(s)downarrow+2NaCl(aq)[/math]
…else, the net ionic equation…
[math]Ba^{2+} + SO_{4}^{2-} longrightarrow BaSO_{4}(s)downarrow[/math]
…does this show the presence of ions…?
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This is a simple reaction.
Barium Chloride(BaCl2) and Aluminum sulphate(Al2(SO4)3) react in a normal condition and form thr following compound-
BaSO4 + AlCl3.
Barium sulphate + aluminum chloride.
I hope i helped.
This is a simple reaction.
Barium Chloride(BaCl2) and Aluminum sulphate(Al2(SO4)3) react in a normal condition and form thr following compound-
BaSO4 + AlCl3.
Barium sulphate + aluminum chloride.
I hope i helped.
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The barium ion reacts with the sulfate ion to form solid barium sulfate, which precipitates because it's insoluble in water.. The sodium and chloride ions remain dissolved in the solution.
The barium ion reacts with the sulfate ion to form solid barium sulfate, which precipitates because it's insoluble in water.. The sodium and chloride ions remain dissolved in the solution.
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The white precipitate is barium sulfate which has a very low solubility in water.
Na2SO4 (aq) + BaCl2 (aq) → BaSO4 (s) + 2 NaCl (aq)
Ba^2+ + SO4^2- → BaSO4
The white precipitate is barium sulfate which has a very low solubility in water.
Na2SO4 (aq) + BaCl2 (aq) → BaSO4 (s) + 2 NaCl (aq)
Ba^2+ + SO4^2- → BaSO4
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while sodium will not displace the barium in BaSO4, the addition of NaCl will increase the solubility of BaSO4 (see graphs below).
while sodium will not displace the barium in BaSO4, the addition of NaCl will increase the solubility of BaSO4 (see graphs below).
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There is the possibility that the chloride ion will form a precipitate with metals (silver, lead, mercury, and to a lesser extent copper) and give a false positive result, while nitrates are always soluble.
There is the possibility that the chloride ion will form a precipitate with metals (silver, lead, mercury, and to a lesser extent copper) and give a false positive result, while nitrates are always soluble.
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In general, the only ions which are coloured are the transition metals - the reason for that is rather more complex than I feel like going in to this morning. However, since Ba is not a transition metal, and sulphate is also not a coloured ion, the solid that settles out is white.
Remember: If you are not part of the solution, you are part of the precipitate!
In general, the only ions which are coloured are the transition metals - the reason for that is rather more complex than I feel like going in to this morning. However, since Ba is not a transition metal, and sulphate is also not a coloured ion, the solid that settles out is white.
Remember: If you are not part of the solution, you are part of the precipitate!
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