What is `Cl^(-)` concentration in `2.5 M BaCl_(2)` solution which is 80% dissociated.

Find the Cl^(-) concentration in solution which is obtained by mixing one mole each of BaCl_(2), NaCl and HCl in 500 ml of water.

If 0.5 M methanol undergo selft dissociation like CH_(3) OH hArr CH_(3) O^(-) + H^(+) & if concentration of H^(+) is 2.5 xx 10^(-4) M then calculate % dissociation of methanol

What is the concentration of chloride ion, in molarity, in a solution containing 10.56 gm BaCl_(2). 8H_(2)O per litre of solution ? (Ba = 137)

In a solution total concentration of M^(3+) is 2xx10^(-3) (M) and total concentration of SCN^(-) is 1.51xx10^(-3) (M) and free SCN^(-) concentration = 1xx10^(-5) (M) What is the dissociation constant of the complex M(SCN)^(2+) ?

Van't Hoff factor of 0.1 m aqueous solution of Al_2(SO_4)_3 which undergoes 80% dissociation is

A sample of 1.0g of solid Fe_(2)O_(3) of 80% purity is dissolved in a moderately concentrated HCl solution which is reduced by zinc dust. The resulting solution required 16.7mL of a 0.1M solution of the oxidant. Calculate the number of electrons taken up by the oxidant.

The osmotic pressure of a dilute solution of an compound XY in water is four times that of a solution of 0.01 M BaCl_(2) in water. Assuming complete dissociation of the given ionic compounds in water, the concentration of XY in solution is x xx 10^(–2) mol/L. The numerical value of x is____.