`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 `:-`
At a certain temperature, the solubility of the salt A_(x)B_(y) is S moles per litre. The general expression for the solubility product will be
The solubility of electrolytes MX_(1),MX_(2) and MX_(3) is 1xx10^(-3) moles per litre. Hence their respective solubility products are :
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.
What is the molar mass of diacidic organic Lewis base (B) , if 12g of its chloroplatinate salt (BH_2 PtCI_6) on ignition produced 5g residue of Pt ?
18g of glucose (molar mass 180gmol^-1) is present in 500cm^3 of its aqueous solution. What is the molarity of the solution? What additional data is required if the molality of the solution is also required to be calculated?
STATEMENT-1: Solubility of sparingly soluble salt decreases due to common ion effect. STATEMENT-2: Solubility product constant does not depend on common ion effect.
25.3 g of sodium carbonate Na_2CO_3 is dissolved in enough water to make 250 ml of solution. If sodium carbonate dissociated completely, molar concentration of sodium ion, Na^+ and carbonate ions , CO_3^(2-) are respectively (Molar mass of Na_2CO_3=106gmol^-1) .
2.5 litre of 1 M NaOH solution are mixed and another 3 litre of 0.5 M NaOH solution. Then the molarity of the resulting solution is
NARENDRA AWASTHI-IONIC EEQUILIBRIUM-Assertin-Reason Type Questions
