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We’re being asked to determine the effect of increasing acidity on the solubility of the following compounds.
For an ionic compound to be more soluble in acidic solution, it must contain a basic ion or be a basic salt.
The acidic ions are usually cations and include:
1. Transition metals with a charge of +2 or higher. Transition metals not satisfying this condition are neutral.
2. Main group metals with a charge of +3 or higher. Main group metals not satisfying this condition are neutral.
3. Amines, which are compounds that contain only N and H (i.e. NH3) or C, N, and H (i.e. CH3NH2)
To determine if an anion is a basic ion, we should add H+ to it.
If the addition of H+ leads to:
1. a weak acid, the anion is basic.
2. a strong acid, the anion is neutral.
Identify the effect of increasing acidity on the solubility of the given compounds.
Drag the appropriate items to their respective bins.
BaCO3, Sr(OH)2, NiBr2, AgI, FeS
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Our tutors have indicated that to solve this problem you will need to apply the Ionic Salts concept. You can view video lessons to learn Ionic Salts. Or if you need more Ionic Salts practice, you can also practice Ionic Salts practice problems.
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Based on our data, we think this problem is relevant for Professor Bakker's class at UA.