Solubility diagram

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[[Image:Solubility diagram for some metal hydroxides.png|thumb|Solubility diagram for some metal hydroxides]]
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[[Image:Solubility diagram for some metal hydroxides.png|Solubility diagram for some metal hydroxides]]
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In the figure a solubility diagram with some of the common metal hydroxides is shown.
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In the figure a solubility diagram for some of the common metal hydroxides is shown.
In the figure the line for each metal ion represents the equilibrium between a 1 M solution of respective metal ion and its hydroxide. On the y-axis the metal ion concentration is given and pH is on the x-axis. At low pH-values the hydroxides are soluble and at higher pH-values the metal ion concentration decreases as the hydroxides are formed. It can be seen that trivalent metal ions can be precipitated at lower pH values compared with the divalent metal ions. Metal ions located close to each other like Fe<sup>2+</sup> and Zn<sup>2+</sup> are difficult to separate and give mixed hydroxide precipitates if both are present during neutralisation. The most difficult metals to precipitate in the diagram are the alkaline earth metals calcium and magnesium.
In the figure the line for each metal ion represents the equilibrium between a 1 M solution of respective metal ion and its hydroxide. On the y-axis the metal ion concentration is given and pH is on the x-axis. At low pH-values the hydroxides are soluble and at higher pH-values the metal ion concentration decreases as the hydroxides are formed. It can be seen that trivalent metal ions can be precipitated at lower pH values compared with the divalent metal ions. Metal ions located close to each other like Fe<sup>2+</sup> and Zn<sup>2+</sup> are difficult to separate and give mixed hydroxide precipitates if both are present during neutralisation. The most difficult metals to precipitate in the diagram are the alkaline earth metals calcium and magnesium.

Revision as of 12:27, 24 August 2007

Solubility diagram for some metal hydroxides

In the figure a solubility diagram for some of the common metal hydroxides is shown.

In the figure the line for each metal ion represents the equilibrium between a 1 M solution of respective metal ion and its hydroxide. On the y-axis the metal ion concentration is given and pH is on the x-axis. At low pH-values the hydroxides are soluble and at higher pH-values the metal ion concentration decreases as the hydroxides are formed. It can be seen that trivalent metal ions can be precipitated at lower pH values compared with the divalent metal ions. Metal ions located close to each other like Fe2+ and Zn2+ are difficult to separate and give mixed hydroxide precipitates if both are present during neutralisation. The most difficult metals to precipitate in the diagram are the alkaline earth metals calcium and magnesium.

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