`105 mL` of pure water at `4^(circ)C` saturated with `NH_(3)` gas yielded a solution of density `0.9g mL^(-1)` and containing `30%NH_(3)` by mass. Find out the volume of `NH_(3)` solution resulting and the volume of `NH_(3)` gas at `4^(circ)C` and `775 mm` of `Hg`, which was used to saturate water.

105 mL of pure water at 4^oC is saturated with NH_3 gas yielding a solution of density 0.9gmL^(−1) and containing 30% NH_3 by mass. The volume (in litres) of NH_3 gas at 4^oC and 775 mm of Hg.

180 ml of pure water at 4^(@)C is saturated with NH_(3) gas, yielding a solution of density 0.8 gram/ml and containing NH_(3) (40% by weight ). (a) Volume of NH_(3) solution. (b) Volume of NH_(3) gas present in saturated solution. (c ) Volume of NH_(3) gas at 115^(@)C and 950 mm of Hg in saturated solution.

HCl gas is passed into water, yielding a solution of density 1.095 g mL^(-1) and containing 30% HCl by weight. Calculate the molarity of the solution.

HCl gas is passed into water, yielding a solution of density 1.095 g mL^(-1) and containing 30% HCl by weight. Calculate the molarity of the solution.

HCl gas is passed into water, yielding a solution of density 1.095 g ml^(-1) and containing 30% HCl by weight. 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 :

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 :

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 :

100 gm water is saturated with glucose to form a solution of density X gm//ml and contains 50% gulcose, by mass. If the volume of solution formed is 100 ml, the value of X is: