Test: Solubility Equilibria of Sparingly Soluble Salts - ACT MCQ

Solubility of the product is only applicable to the saturated solutions, whereas an ionic product is applicable to all types of solutions. It is because the formation of a precipitate is dependent on the solubility product.

For the salt A_xB_y, (A_xB_y = xA^y+ + yB^x+), the solubility of a sparingly soluble salt is given by x^x.y^y.s^x+y. K_sp = x^x.y^y.s^x+y, where x = 2 and y = 3; K_sp = 108S5 = 1 x 10^-25. S = 10^-5. The solubility of the salt is given by 10^-5.

Yes, we can predict the solubility of a sparingly soluble salt, for example, consider the reaction; A_xB_y = xA^y+ + yB^x+, the solubility of a sparingly soluble salt is given by x^x.y^y.s^x+y, knowing the values of K_sp, x and y, the solubility of the salt can be calculated.

Solubility product K_sp is defined as the product of the concentrations of the ions of the salt in its standard solution at a given temperature raised to the power of the ions produced by the dissociation of 1 mole of the salt.

Common Ion effect is used in the purification of common salt, salting out of soap and qualitative analysis. In qualitative analysis, Ammonium Hydroxide is added in the presence of Ammonium Chloride to avoid the precipitation of V group radicals.

For the salt A_xB_y, (A_xB_y = xA^y+ + yB^x+), the solubility of a sparingly soluble salt is given by x^x.y^y.s^x+y. K_sp = x^x.y^y.s^x+y, where x = 1 and y = 3; K_sp = 27S⁴, by rearranging, we get solubility denoted by S as (K_sp/27)^1/4.

A salt is soluble if the solubility is greater than 0.1 M. A salt is slightly soluble if the solubility is between 0.01 M and 0.1 M and the salt is sparingly soluble if the solubility is less than 0.01 M.

The concept of solubility product helps in predicting the formation of the precipitate. In general, if the ionic product is greater than the solubility product, the precipitate is formed and if the ionic product is less than the solubility product, the precipitate is not formed.

In the solution of two electrolytes, if the common ions’ concentration (Hydroxide Ion concentration in calcium hydroxide and barium hydroxide solution) is equal, then on mixing there is zero change in the degree of association in both of the electrolytes, such solutions are called isohydric solutions.

Common Ion effect is defined as the separation of the dissociation of a weak electrolyte by the addition of a strong electrolyte having some common ion. Therefore the degree of dissociation of Ammonium hydroxide decreases in the presence of Ammonium Chloride due to common Ion effect.