Solubility Product Constant

This question has statement I and Statement II. Of the four choices given after the Statements, choose the one that best describes the two Statements. Statement-I: Solubility of sparingly soluble salt decreases due to common ion effect. Statement-II: Solubility product constant does not depend on common ion effect.

A very dilute saturated solution of a sparingly soluble salt A_(3)B_(4) has a vapour pressure of 20mm of Hg at temperature T, while pure water exerts a pressure of 20.0126mm Hg at the same temperature. Calculate the solubility product constant of A_(3)B_(4) at the same temperature.

Solubility products constants (K_(sp)) of salts of types MX, MX_2,M_3X at temperature T are 4xx 10^(-8) 3.2 xx 10^(-14) and 27 xx 10 ^(-15) respectively. Solubility ("moldm" ^(-3) ) of the salts at temperature T are in the order :

Consider a sturated solution of silver chloride that is in contact with solid silver chloride. The solubility equilibrium can be represented as AgCl(s)hArrAg^(+)(aq.)+Cl^(-)(aq.)," "K_(sp)=[Ag^(+)(aq.)][Cl^(-)(aq.)] Where K_(sp) is clled the solubility product constant or simply the solubility product. In general, the solubility product of a compound is the product of the molar concentrations of the constituent ions, each raised to the power of its stoichiometric coefficient in the equilibrium equation. For concentrations of ions that do not necessarliy correpond to equilibrium conditions we use the reaction quotient (Q) which is clled the ion or ionic prodect (Q) to predict whether a precipitate will from. Note that (Q) has the same for as K_(sp) are QltK_(sp) Unsaturated solution Q=K_(sp) Saturated solution Qgt_(sp) Supersaturated solution, precipitate will from Determine the molar solubility of MgF_(2) from its solubility product K_(sp)=4xx10^(-9) :

For any sparingly soluble salt [M(NH_(3))_(4)Br_(2)] H_(2)PO_(2) Given: lambda_(M(NH_(3))_(4)Br_(2)^(+))^(@) = 400 Sm^(2) - mol^(-1) . lambda_(H_(2)PO_(2)^(-))^(@) = 100 Sm^(2) -mol^(-1) Specific resistance of saturated [M(NH_(3))_(4)Br_(2)] H_(2)PO_(2) solution is 200 Omega-cm If solubility product constant of the above salt is 10^(-x) . What will be the value of x .

Calculation of Solubility and Solubility Product from Molar Conductivity