0
Anions
Cl-, Br-, I-
S2-
OH-, O2-
SO42-
CO32-,PO43-,SO32-
C2H3O2-
NO3-
High Solubility (aq) ≥0.1 mol/L (at SATP)
Most
Group 1, NH4+, Group 2
Group 1, NH4+, Sr2+, Ba2+, Tl+
Most
Group 1, NH4+
Most
All
All group 1 compounds including acids and all ammonium compounds are assumed to have high solubility in water
Low solubility (s) <0.1 mol/L (at SATP)
Ag+, Pb2+, Tl+, Hg22+, (Hg+), Cu+
Most
Most
Ag+, Pb2+, Ca2+, Ba2+, Sr2+, Ra2+
Most
Ag+
None
Wiki User
∙ 13y ago
Wiki User
∙ 12y agoAlmost all the ionic compounds are soluble in water due to polar nature of water. Now coming to your question, if you mean which substances are soluble in ionic compounds, then you must know that ionic compounds are quite good solvent for ionic or polar substances. This is also dependent on your idea of polar compounds and ionic compounds. So from basic principle of 'like dissolve like' polar or ionic substances dissolve polar or ionic substances. Thats it.
Wiki User
∙ 14y agoGrams anhydrous salt in 100 grams water
35.65 at 0 degrees C
38.99 at 100 degrees C
for further information see Perrys Chemical Engineers handbook
Add your answer:
Earn +20 pts
Ph may affect the solubility of ionic compounds?
True
What is the solubility of Covalent bonds?
Solubility of covalent bonds is usually high to low. Solubility for Ionic compounds is usually high.
Are four physical properties of ionic compounds?
brittlenessmeltinghigh solubility in watervery high boiling points
How is the solubility in ionic compounds?
Solublity of the ionic compounds vastly vary from one to another. For example, sodium chloride dissolves very well in water, but barium chloride is almost insoluble.
Are ionic compounds insoluable in water?
No, they usually are soluable. There are solubility tables that make known any that are not soluable. AgCl is an insoluable ionic compound.
Ph may affect the solubility of ionic compounds?
True
What is the solubility of Covalent bonds?
Solubility of covalent bonds is usually high to low. Solubility for Ionic compounds is usually high.
Are four physical properties of ionic compounds?
brittlenessmeltinghigh solubility in watervery high boiling points
How is the solubility in ionic compounds?
Solublity of the ionic compounds vastly vary from one to another. For example, sodium chloride dissolves very well in water, but barium chloride is almost insoluble.
Are ionic compounds insoluable in water?
No, they usually are soluable. There are solubility tables that make known any that are not soluable. AgCl is an insoluable ionic compound.
How does solubility of ionic compounds and gas in water vary with temperature and pressure changes?
Ionic compounds and gases are more soluble in water at higher temperatures. They are more soluble at lower pressures as well.
What is precipitation titration's principle?
Precipitation titrations are based upon reactions that yield ionic compounds of limited solubility.
What are three characteristic properties of iconic compounds?
If you think to ionic compounds:- dissociation in water- good solubility in water- as solids they are insulators- high melting point
Why is solubility of AgCl in AgNO3 is very low?
solubility of an ionic compound decreases in the presence of a common ion. A common ion in the solution, that is common to the ionic compound being dissolved. for example the silver ion in silver nitrate solution is common to the silver in silver chloride. the presence of a common ion must be taken into accounts when determining the solubility of an ionic compounds.
Does pH mean solubility?
Weak soluble ionic compounds do depend greatly on the solution's ph. Not all compounds depend on the pH though because those that have stronger ionic compounds do not need to depend on the ph.
How lattice energy affect solubility?
A high hydration energy gives an increased solubility.
How does dipolar nature of water molecule make it an effective solvent for ionic compounds like salt?
according to the "Like dissolves like" in solubility, ionic compounds like salt, the polar materials, can be dissolved in similar polar nature water molecule.
