A number of ionic compounds, e.g AgCl,Ca{F}_{2},Ba{SO}_{4} are insoluble in water. This is because:ionic compounds do not dissolve in waterwater is not a good ionising solventwater has a high dielectric constantthese molecules have exceptionally high attr (2024)

FAQs

Are a number of ionic compounds insoluble in water? ›

A number of ionic compounds, e.g AgCl,CaF2,BaSO4 are insoluble in water. This is because these molecules have exceptionally high attractive forces in their lattice. Ionic compounds having lattice energy higher than hydration energy are insoluble in water.

Fluoride is very electronegative, and thus the bonding forces between Ca2+ and each fluoride anions are very strong, they are tightly held together in the crystal form. A few water molecules do not have enough strength to get in between and dissolve it.

“Barium sulphate is insoluble in water” for its high lattice energy as well as low hydration energy, which is the ionic compound of these chemical particles.

as we move from left to right in periodic table ionic character decreases , similarly moving from top to bottom it increases ....so out of these Agcl is less ionic (more ionic is Cacl2,Kcl, Bacl2,Agcl).

This is because the ionic forces in those molecules are very high, which creates high lattice energy. Due to high lattice energy, the hydration energy decreases that makes those compounds insoluble in water. Some examples of insoluble ionic compounds are $AgCl,BaS{{O}_{4}},Ca{{F}_{2}}$ etc.

This kind of solution is said saturated and the maximum amount of the salt which can be dissolved is called solubility of the salt. Therefore the solubility of AgCl is 0.0024 grams/liter.

The solubility of fluorides is much less as compared to corresponding chlorides. because of low lattice enthalpy.

Barium sulfate (or sulphate) is the inorganic compound with the chemical formula BaSO₄. It is a white crystalline solid that is odorless and insoluble in water.

B a S O 4 is an ionic compound, yet it is insoluble in water because both B a 2 + and S O 4 2 − are bigger cation stabilizes bigger anion strongly hence B a S O 4 has high lattice enthalpy. For a compound to be soluble, its lattice enthalpy should be low and it should decrease more rapidly than hydration enthalpy.

The lattice enthalpy of BaSO4 is much than its hydration enthalpy and hence it is insoluble in water . But on, the other hand , hydration enthalpy of BeSO4 is much higher than its lattice enthalpy because of small size of Be2+ ions . Therefore , it is highly soluble in water .

Is AgCl more ionic than NaCl? ›

The bond character of Silver chloride is less ionic. The more ionic in character a bond is, the less covalent it will be. A covalent bond shares electrons, and an ionic bond does not share electrons. Thus, Silver chloride is more covalent because it shares its electrons more evenly than the sodium chloride does.

NaCl is soluble freely in water but AgCl is sparingly soluble.

According to the postulates, As we move left to right in a period, the size of the cation decreases and ionic character also decreases. Among $Ag,K,Ca,Ba$ , the compound that is present in the d block is $Ag$ whereas $K,Ca,Ba$ they are all present in s block. Therefore, $AgCl$ is least ionic among the above options.

Water is a polar solvent and has two poles one negative and another positive. The two poles of water have strong forces of attraction towards other charged ions, due to this water breaks the ionic bond by hydrogen bond formation. Therefore, ionic bonds dissolve in water.

Carbonate is a doubly charged negative ion that should form strong electrostatic bonds with metal ions - the doubly charged calcium ion, Ca2+, should form strong ionic bonds, and indeed it does. So, calcium carbonate is insoluble in water.

Sand , Chalk , Benzene ( C 6 H 6 ) , Calcium Sulfate , Barium Sulfate , Strontium sulfate , Lead Sulfate , and many more are insoluble in water.

Ionic compounds often result from reactions between metals and non-metals. Ionic substances conduct electricity when they are in a liquid state or in an aqueous solution.