The solubility of Ba_3(AsO_4)_2 (formula weight =690 ) is 6.9 xx 10^(-2) g//100 ml. what is the K_(sp) ?
Calculate the solubility of A_(2)X_(3) is pure water, assuming that neither kind of ion racts with water. The solubility product of A_(2)X_(3),K_(sp)=1.1xx10^(-23)
What is the weight (in g) of Na_(2) CO_(3) (molar mass= 106) present in 250 mL of its 0.2 M solution?
The solubility of AgCl in 0.1M NaCI is (K_(sp) " of AgCl" = 1.2 xx 10^(-10))
Calculate the solubility of A_(2)X_(2) in pure water, assuming that neither kind of ion reacts with water. The solubility product of A_(2)X_(3) , K_(sp)=1.1xx10^(-23) .
The molar solubility of Pbl_(2) in 0.2M Pb(NO_(3))_(2) solution in terms of solubility product, K_(sp)
A solution which remains in equilibrium with undissolved solute is said to be saturated. The concentration of a saturated solution at a given temperature is called solubility. The product of concentration of ions in a saturated solution of an electrolyte at a given temperature, is called solubility product (K_(sp)) . For the electrolyte, A_(x),B_(y),:A_(x),B_(y(s)) rarr xA^(y+)+ y^(Bx-) , with solubility S, the solubility product (K_(sp)) =x^(x)xxy^(y) xx s^(x+y) . While calculating the solubility of a sparingly soluble salt in the presence of some strong electrolyte containing a common ion, the common ion concentration is practically equal to that of strong electrolyte. If in a solution, the ionic product of an clectrolyte exceeds its K_(sp) , value at a particular temperature, then precipitation occurs. The solubility of BaSO_(4) , in 0.1 M BaCl_(2) , solution is (K_(sp) , of BaSO_(4), = 1.5 xx 10^(-9))
NARENDRA AWASTHI-IONIC EEQUILIBRIUM-Assertin-Reason Type Questions
