Question

The solubility product of $AgCl$ under standard conditions of temperature is given by:
A. $1.6\times {{10}^{-5}}$
B. $1.5\times {{10}^{-2}}$
C. $3.6\times {{10}^{-6}}$
D. $1.5\times {{10}^{-10}}$

Answer 1

Hint: Solubility product depends on the number of ions formed in a reaction at equilibrium. At standard state a salt will for equal amount of ions. Thus silver chloride will for equal amount of silver cation and chloride ion.

Complete Step by Step Answer:
Solubility product of a species is defined as the product of the concentration of the cation and anion formed from a species at equilibrium. At this stage the coefficients before the ions exist as a power to the concentration of the corresponding cation and anion.

Silver chloride dissociate at equilibrium as follows:
$AgCl\rightleftharpoons A{{g}^{+}}+C{{l}^{-}}$
Thus Silver chloride dissociates into one silver cation and one chloride anion at equilibrium.
Thus solubility product is given as follows:
$K_{sp}=(S)\times S$; where $Ksp$ is defined as the solubility product and $S$ is defined as the solubility for the cation and anion.

When silver chloride dissociates in water at standard state it forms an equal amount of silver ion and chloride ion. Thus one mole of silver chloride dissociates to give one mole of silver cation and one mole of chloride ion. At standard state the value of the solubility product of silver chloride is $1.5\times {{10}^{-10}}$.
Thus the correct option is D.

Note: The chemical name of $BaS{{O}_{4}}$ is barium sulphate. It is an ionic compound. It dissociates into the corresponding ions in solution state. It is a white colored solid and it is insoluble in water.