How does cation affect solubility?
If the water molecules have a greater attraction to the ions than ions have for each other, then the compound will be soluble in water. Compounds with small ions are less soluble than compounds with large ions. It is more difficult for the water to break them apart, so they are less soluble.
Which cations are always soluble?
If we look at the solubility rules, we will notice that there are three main cations that are always soluble in water. This means that a compound containing one of these three cations will always be soluble in water. The three cations are sodium, potassium and ammonium ions.
Which cation is soluble in water?
The solubility of ionic compounds in water at 25°C, in general: All compounds of the ammonium ion (NH4+) are soluble. All compounds of Alkali metal (Group 1, or, Group IA) cations, are soluble. All nitrates are soluble.
What affects the solubility of an ionic compound?
The solubilities of ionic compounds are affected by solute-solvent interactions, the common ion effect, and temperature. Strong solute-solvent attractions increase solubility of ionic compounds.
How does ion concentration affect solubility?
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.
Are Group 2A cations soluble?
Salts of the Group 2A metals are less soluble in water than those of Group 1A because of the higher charge densities on the 2+ cations; nevertheless, many Group 2A salts are at least moderately soluble.
Is francium soluble in water?
Nearly all francium salts are water-soluble.
What cations and anions are always soluble?
Group 1A and ammonium cations are soluble with no exceptions. Nitrate and acetate anions are soluble with no exceptions. Chlorides, bromides, and iodides are generally soluble except with those that are paired with silver, mercury(II), and lead(II) cations.
What are the solubility rules for ionic compounds?
| Solubility Rules for Ionic Compounds in Water | |
|---|---|
| Rule 1: | Compounds of NH4+ and group 1A metal ions are soluble. |
| Rule 2: | Compounds of NO3–, ClO4–, ClO3– and C2H3O2– are soluble. |
| Rule 3: | Compounds of Cl –, Br – and I – are soluble except those of Ag+, Cu+, Tl+, Hg22+ and Pb2+. |