100 ml of 0.1 M HCl and 100 ml of 0.1 M HOCN are mixed . What is the concentration of .. OCN ^(-).. , and pH of the solution ? (K_a=1.2 xx 10^(-6) )
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 molar solubility of Fe(OH)_2 (K_(sp) =8.0 xx 10^(-16) ) at pH 13.0 ?
What is the pH of a solution obtained by dissolving 0.0005 mole of the strong electrolyte, calcium hydroxide, Ca(OH)_(2) , to form 100 ml of a saturated solution (aqueous)? (K_(w)=1.0xx10^(-14) "mole"^(2) "litre"^(-2))
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) .
Calculate the concentration of silver ion, if water is saturated with AgCNS (K_(sp) =1 xx 10^(-12)) and AgBr (K_(sp) = 5 xx 10^(-13) ).
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
