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Stannous chloride is not dissolving into water
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Stannous chloride is not dissolving into water
Tin chloride $\ce{SnCl2}$ (hydrated or not) is not soluble in pure water. It is quickly hydrolyzed according to : $$\ce{SnCl2 + 2 H2O -> Sn(OH)2 + 2 HCl}$$ and $\ce{Sn(OH)2}$ is insoluble in water. To dissolve $\ce{SnCl2}$, this reaction has to be reversed by adding $\ce{HCl}$ in $5$ M solution. In this case, a clear solution is obtained.
Unfortunately $\ce{SnCl2}$ solutions are easily oxidized by oxygen from the air, and transformed into $\ce{SnCl4}$ plus a basic and not very soluble salt $\ce{Sn(OH)Cl}$, according to : $$\ce{6 SnCl2 + O2 + 2 H2O -> SnCl4 + 4 Sn(OH)Cl}$$ If a pure solution of $\ce{SnCl2}$ is wanted, this reaction can be avoided by adding some metallic tin grains ($\ce{Sn}$), which react and reduce $\ce{SnCl4}$ according to : $$\ce{SnCl4 + Sn -> 2 SnCl2}$$ It should also be mentioned that the solutions of $\ce{SnCl4}$ are also slowly hydrolyzed at high dilution.
Ref.: F. P. Treadwell, Analyse qualitative, Dunod Ed. Paris, 1924.
F. A. Cotton, G. Wilkinson, Advanced Inorganic Chemistry, Interscience Pub., J. Wiley, New York, 1972, p. 330 - 331
Tin chloride $\ce{SnCl2}$ (hydrated or not) is not soluble in pure water. It is quickly hydrolyzed according to : $$\ce{SnCl2 + 2 H2O -> Sn(OH)2 + 2 HCl}$$ and $\ce{Sn(OH)2}$ is insoluble in water. To dissolve $\ce{SnCl2}$, this reaction has to be reversed by adding $\ce{HCl}$ in $5$ M solution. In this case, a clear solution is obtained.
Unfortunately $\ce{SnCl2}$ solutions are easily oxidized by oxygen from the air, and transformed into $\ce{SnCl4}$ plus a basic and not very soluble salt $\ce{Sn(OH)Cl}$, according to : $$\ce{6 SnCl2 + O2 + 2 H2O -> SnCl4 + 4 Sn(OH)Cl}$$ If a pure solution of $\ce{SnCl2}$ is wanted, this reaction can be avoided by adding some metallic tin grains ($\ce{Sn}$), which react and reduce $\ce{SnCl4}$ according to : $$\ce{SnCl4 + Sn -> 2 SnCl2}$$ It should also be mentioned that the solutions of $\ce{SnCl4}$ are also slowly hydrolyzed at high dilution.
Ref.: F. P. Treadwell, Analyse qualitative, Dunod Ed. Paris, 1924.
F. A. Cotton, G. Wilkinson, Advanced Inorganic Chemistry, Interscience Pub., J. Wiley, New York, 1972, p. 330 - 331
Tin chloride $\ce{SnCl2}$ (hydrated or not) is not soluble in pure water. It is quickly hydrolyzed according to : $$\ce{SnCl2 + 2 H2O -> Sn(OH)2 + 2 HCl}$$ and $\ce{Sn(OH)2}$ is insoluble in water. To dissolve $\ce{SnCl2}$, this reaction has to be reversed by adding $\ce{HCl}$ in $5$ M solution. In this case, a clear solution is obtained.
Unfortunately $\ce{SnCl2}$ solutions are easily oxidized by oxygen from the air, and transformed into $\ce{SnCl4}$ plus a basic and not very soluble salt $\ce{Sn(OH)Cl}$, according to : $$\ce{6 SnCl2 + O2 + 2 H2O -> SnCl4 + 4 Sn(OH)Cl}$$ If a pure solution of $\ce{SnCl2}$ is wanted, this reaction can be avoided by adding some metallic tin grains ($\ce{Sn}$), which react and reduce $\ce{SnCl4}$ according to : $$\ce{SnCl4 + Sn -> 2 SnCl2}$$ It should also be mentioned that the solutions of $\ce{SnCl4}$ are also slowly hydrolyzed at high dilution.
Ref.: F. P. Treadwell, Analyse qualitative, Dunod Ed. Paris, 1924.
F. A. Cotton, G. Wilkinson, Advanced Inorganic Chemistry, Interscience Pub., J. Wiley, New York, 1972, p. 330 - 331
Tin chloride $\ce{SnCl2}$ (hydrated or not) is not soluble in pure water. It is quickly hydrolyzed according to : $$\ce{SnCl2 + 2 H2O -> Sn(OH)2 + 2 HCl}$$ and $\ce{Sn(OH)2}$ is insoluble in water. To dissolve $\ce{SnCl2}$, this reaction has to be reversed by adding $\ce{HCl}$ in $5$ M solution. In this case, a clear solution is obtained.
Unfortunately $\ce{SnCl2}$ solutions are easily oxidized by oxygen from the air, and transformed into $\ce{SnCl4}$ plus a basic and not very soluble salt $\ce{Sn(OH)Cl}$, according to : $$\ce{6 SnCl2 + O2 + 2 H2O -> SnCl4 + 4 Sn(OH)Cl}$$ If a pure solution of $\ce{SnCl2}$ is wanted, this reaction can be avoided by adding some metallic tin grains ($\ce{Sn}$), which react and reduce $\ce{SnCl4}$ according to : $$\ce{SnCl4 + Sn -> 2 SnCl2}$$ It should also be mentioned that the solutions of $\ce{SnCl4}$ are also slowly hydrolyzed at high dilution.
Ref.: F. P. Treadwell, Analyse qualitative, Dunod Ed. Paris, 1924.
F. A. Cotton, G. Wilkinson, Advanced Inorganic Chemistry, Interscience Pub., J. Wiley, New York, 1972, p. 330 - 331
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