Problem: A solution containing several metal ions is treated with dilute HCl; no precipitate forms. The pH is adjusted to about 1, and H2S is bubbled through. Again, no precipitate forms. The pH of the solution is then adjusted to about 8. Again, H2S is bubbled through. This time a precipitate forms. The filtrate from this solution is treated with (NH4)2HPO4. No precipitate forms.Which of these metal cations are either possibly present or definitely absent: Al3+, Na+, Ag+, Mg2+?

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FREE Expert Solution

We have to determine if any of the ions, Al3+, Na+, Ag+ or Mg2+, is either present or absent in the solution.

In qualitative analysis, we can separate metal ions through precipitation reactions.

Metal ions are classified into 5 groups based on their solubility and type of anion they form a precipitate with.

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Problem Details

A solution containing several metal ions is treated with dilute HCl; no precipitate forms. The pH is adjusted to about 1, and H2S is bubbled through. Again, no precipitate forms. The pH of the solution is then adjusted to about 8. Again, H2S is bubbled through. This time a precipitate forms. The filtrate from this solution is treated with (NH4)2HPO4. No precipitate forms.

Which of these metal cations are either possibly present or definitely absent: Al3+, Na+, Ag+, Mg2+?

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Our tutors have indicated that to solve this problem you will need to apply the Solubility Rules concept. You can view video lessons to learn Solubility Rules. Or if you need more Solubility Rules practice, you can also practice Solubility Rules practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor All Professors' class at HCC.