The solubility of electrolytes MX_(1),MX_(2) and MX_(3) is 1xx10^(-3) moles per litre. Hence their respective solubility products are :
A_(3)B_(2) is a sparingly soluble salt with molar mass M(gmol_(-)) and solubility x gm litre_(-1) , the ratio of the molar concentration of B^(3-) to the solubilty product of the salt is :-
Discuss the applications of calculation of solubility product of a sparingly soluble salt.
At a certain temperature the equilibrium constant K_(c) is 0.25 for the reaction A_(2)(g)+B_(2)(g)hArrC_(2)(g)+D_(2)(g) If we take 1 mole of each of the four gases in a 10 litre container ,what would be equilibrium concentration of A_(2) (g)?
Arrhenius studies the effect of temperature on the rate of a reaction and postulted that rate constant varies with temperature exponentially as k=Ae^(E_(a)//RT) . Thuis method is generally used for finding the activation energy of a reaction. Keeping temperature constant, the effect of catalyst on the activation energy has also been studied. The pre-exponetial factor in the Arrhenius equation of a first order reaction has the unit : a) mol L^(-1)s^(-1) b) L mol^(1)s^(-1) c) s^(-1) d) dimensionless
Which of the following statements regarding the compound A_(x)B_(y) is /are correct?
STATEMENT-1: Sparingly soluble salts AB and XY_(2) with the same solubility product, will have different solubility. STATEMENT-2: Solubiluty of sparingly soluble salt depend upon solubility product.
NARENDRA AWASTHI-IONIC EEQUILIBRIUM-Assertin-Reason Type Questions
