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urce from Cengage Learning - Google Chrome /ilm/takeAssignment/takeCovalentActivity.do?locator-assignment-take&takeAssignmentSessionLo; (Review Topics) Use the References to access important values if needed for this question. Each of the insoluble salts below are put into 0.10 M hydrobromic acid solution. Do you expect their solubility to be more, less, or about the same as in a pure water solution ? Clear All . lead iodide More soluble than in pure water. silver bromide Similar solubility as in pure water calcium carbonate Less soluble than in pure water calcium fluoride Previous Next

Explanation / Answer

Solubility of any salt increases with ionic strength of the solution provided that there is no common ion and concentration less than 1 M because there are ionic interactions between the solute ions and the solvent ions, which allow more dissolution because only free ions enter into expression for the solubility product equilibrium constant. From mathematical point of view, in higher ionic strength solutions, activity coefficients for calcium and sulfate become smaller, and hence concentrations must be larger to maintain a constant solubility product at equilibrium.

Also, Solubility decreases in the presence of common ion because of Le - Chatlier Principle which cause the reaction to go in direction of undissociated salt as a result of increasing the concentration of common ion.

So, out of four salts given, only AgBr has common ion with HBr and hence its solubility will be less than pure water. Whereas all the other three salts will have more solubility in 0.10 M HBr than pure water.

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