Why does ionic radius affect solubility?

Compounds with small ions are less soluble than compounds with large ions. Small ions are closer to each other, so they have strong attractive forces. It is more difficult for the water to break them apart, so they are less soluble. The solubility increases as the size of the halide ion increases.

How does solubility differ for ionic salts?

Ionic compounds are most soluble in polar solvents like water, because the ions of the solid are strongly attracted to the polar solvent molecules. Ionic compounds are less soluble is solvents that contain a common ion.

How does charge affect ionic radius?

In general, ionic radius decreases with increasing positive charge. As the charge on the ion becomes more positive, there are fewer electrons. In general, ionic radius increases with increasing negative charge. As the charge on the ion becomes more negative, there are more electrons.

Why ionic radius decreases down the group?

As you move down a column or group, the ionic radius increases. Ionic radius decreases moving from left to right across a row or period. More protons are added, but the outer valence shell remains the same, so the positively charged nucleus draws in the electrons more tightly.

Does solubility increase with ionic strength?

The basic principle illustrated is that in the absence of a com- mon ion, the solubility of an electrolyte increases as ionic strength increases.

Why some ionic compounds are less soluble than others?

Generally, ionic compounds whose component ions have larger charge magnitudes are less soluble because the ions are attracted too much to dissociate. A soluble compound will dissociate because of the attractions with the surrounding water molecules are strong enough to separate the ions.

Why does solubility decrease with a common ion?

If you have a solution and solute in equilibrium, adding a common ion (an ion that is common with the dissolving solid) decreases the solubility of the solute. This is because Le Chatelier’s principle states the reaction will shift toward the left (toward the reactants) to relieve the stress of the excess product.

Why do smaller particles dissolve faster than larger ones?

The disjoining pressure of small particles is greater than that of large particles, so small particles have a higher interfacial solubility. Due to their higher differential concentration, thinner diffusion layer,27 and increased surface area, small particles dissolve faster (Figure 8A).

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