Calculate the number of millilitre of `NH_3 (aq)` solution `(d=0.986 g/mL)` contain `2.5%` by mass `NH_3`, which will be required to precipitate iron as `Fe(OH)_3` in a `0.8g` sample that contains `50% Fe_2O_3`.

Calculate the number of millilitre of NH_(3) (aq) solution (d=0.986g/ml) contain 2.5% by mass NH_(3) , which will be required to precipitate iron as Fe(OH)_(3) in a 0.8 g sample that contains 50% Fe_(2)O_(3) .

The density of NH_(4)OH solution is 0.6g//mL . It contains 34% by weight of NH_(4)OH . Calculate the normality of the solution:

How many millilitres of 0.1 NH_(2)SO_(4) solution will be required for complete reaction with a solution containing 0.125 g of pure Na_(2)CO_(3) ?

The density of a solution containing 7.3% by mass of HCl is 1.2 g/mL. Calculate the molarity of the solution

Ammonia gas is passed into water, yielding a solution of density 0.93 g//cm^(3) and containing 18.6% NH_(3) by weight. The mass of NH3 per cc of the solution is :

12. g of an impure sample of arsenious oxide was dissolved in water containing 7.5 g of sodium bicarbonate and the resulting solution was diluted to 250 mL . 25 mL of this solution was completely oxidised by 22.4 mL of a solution of iodine. 25 mL of this iodine solution reacted with same volume of a solution containing 24.8 g of sodium thiosulphate (Na_(2)S_(2)O_(3).5H_(2)O) in one litre. Calculate teh percentage of arsenious oxide in the sample ( Atomic mass of As=57 )

1.7g of NH_3(g) is present in a 2-L flask. The active mass of NH_3(g) is

Number of Fe atoms in 100 g Haemoglobin if it contains 0.33% Fe. (Atomic mass of Fe. = 56)