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The pH of Ba(OH)_(2) solution is 13 . The number millimoles of Ba(OH)_(2) present in 10 ml of solution would be

A solution of Ba(OH)_(2) is standardized with potassium acid phthalate (abbreviated KHP), KHC_(8)H_(8)O_(4) (M=204). If 1.530 g of KHP is titrated with 34.50 mL of the Ba(OH)_(2) solution, what is the molarity of Ba(OH)_(2) ?

The amount of H_2 S required to precipitate 1.69 g BaS from BaCl_2 solution is (Atomic weight Ba=137, S = 32 and H = 1) :

An aqueous solution contains an unknown concentration of Ba^(2+) . When 50 mL of a 1 M solution of Na_(2)SO_(4) is added, BaSO_(4 ) just begins to precipitate. The final volume is 500 mL. The solubility product of BaSO_(4) is 1xx10^(–10) . What is the original concentration of Ba^(2+) ?

A solution was prepared by dissolving 0.0005 mol of Ba(OH)_(2) in 100 mL of the solution. If the base is assumed to ionise completely, the pOH of the solution will be

The pH of an aqueous solution of Ba(OH)_(2) is 10 . If the K_(sp) of Ba(OH)_(2) is 1xx10^(-9) , then the concentration of Ba^(2+) ions in the solution in mol L^(-1) is