Question

Solubility of $AgCl$ will be minimum in
A. $0.001M$ $AgN {O_3}$
B. Pure water
C. $0.01M$ $CaC {l_2}$
D. $0.01M$ $NaCl$

Answer 1

Solubility is an asset referring to the potential for a given substance, the solute, to dissolve in a solvent. It is measured in phrases of the maximum quantity of solute dissolved in a solvent at equilibrium. The ensuing answer is known as a saturated solution.

Complete answer:
The solubility of unsolvable materials can be reduced by the existence of a common ion.
Present in silver chloride are silver ions ($A {g^ + }$) and chloride ions ($C{l^ - }$). $AgCl$ Isn’t always soluble in water.
Silver nitrate (that's soluble) has silver ions in common with silver chloride. But the concentration of the shared ion is small ($0.001M$).
Calcium chloride (additionally soluble) has chloride ions that are not unusual with silver chloride. In $CaC{l_2}$ has moles of common ion ($0.02M$) that decreases solubility very unexpectedly.
And $0.01M$ $NaCl$ is more soluble in $AgCl$ .

So, the correct answer is C.

Additional information:
Certain substances are soluble in all proportions with a given solvent, which include ethanol in water.
This asset is called miscibility.
Under various situations, the equilibrium solubility may be surpassed to offer a so-called supersaturated answer, that is metastable.
The solvent is frequently a solid, which can be a pure material or a combination.
The species that dissolves, the solute, can be a gas, every other liquid, or a strong.
Solubility varies widely, from infinitely soluble together with ethanol in water, to poorly soluble, which includes silver chloride in water.
The time period insoluble is regularly carried out to poorly soluble compounds, though strictly speaking there are only a few cases wherein there is in reality no cloth dissolved.
The manner of dissolving, known as dissolution, is surprisingly honest for covalent materials including ethanol.

Note: The common-ion effect refers back to the decrease in solubility of an ionic precipitate via the addition to the solution of a soluble compound with an ion in common with the precipitate. This behavior is a result of Le Chatelier's principle for the equilibrium response of the ionic association/dissociation