Short Answer TypeHow does the concept of solubility product help in predicting the ionising and precipitating nature of a salt?
Knowing the solubility product of a salt, it is possible to predict that on mixing the solutions of its ions, a precipitate will be formed or not. For the precipitation to occur, its ionic product should exceed its solubility product. Therefore, to predict the precipitation reaction, we just calculate the ionic product of the ions and find out whether it is greater than Ksp or not. If
Ionic product > Ksp, precipitation occurs;
Ionic product < Ksp, no precipitation occurs.
Ionic product = Ksp, the solution is just saturated and no precipitation occurs.
The solubility of Ag2CrO4 at 298K is 6·6 × 10–5 moles/litre. Find its solubility product.
The solubility of CaF2 in water at 298K is 1·7×10–3 gram per 100 cm3. Calculate the solubility product of CaF2 at 298K.
Calculate the molar solubility of Ni(OH)2 in 0·10M NaOH. The ionic product of Ni(OH)2 is 2·0 × 10–15.
At a certain temperature, the solubility product of AgCl is 1 × 10–10, calculate the solubility of AgCl in g/litre.
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