A hand book states that the solubility of `RNH_(2)` (g) in water at 1 atm and `0^(@)`C is 22.41 volumes of `RNH_(2)`(g) per volume of water. `(pK_(b) of RNH_(2)=4)` Find the max. pOH that can be attained by dissolving `RNH_(2)` in water:
The Henry's constant for solubility of N_(2) gas in water at 298K is 1.0xx10^(5) atm. The mole fraction of N_(2) in air is 0.8 . The number of moles of N_(2) from air dissolved in 10 moles of water at 298K and 5 atm pressure is :
A sample of gas has a volume of 0.2 L, measured at 1 atm pressure and 0^@ C. At the same pressure but at 273^@ C, its volume becomes
A sample of gas has a volume of 0.2 lit measured at 1 atm pressure and 0^@C . At the same pressure, but at 273^@C , its volume will become
The equilibrium constant for the ionisation of RNH_(2(g)) in water as RNH_(2(g)) + H_(2)O_((l)) hArr "RNH"_(3(aq))^(+) + OH_((aq))^(-) is 8 xx 10^(-6) at 25^(@) C . Find the pH of a solution at equilibrium when pressure of RNH_(2(g)) is 0.5 bar.
The vapour pressure of water at 23^(@)C is 19.8 mm. 0.1 mole of glucose is dissolved in 178.2 g of water. What is the vapour pressure (in mm) of the resultant solution?
0.32 g of N_2 H_4 is dissolved in water and made up to one litre. If K_b of N_2 H_4 is 4 xx 10^(-6) M, calculate the fraction of N_2 H_4 that has reacted with water in the solution.
Molecular mass of SrF_2 , is 125.6. Solubility of SrF, in water is 1.2 xx 10^(-2) g L^(-1) . Calculate the solubility product of SrF_2
NARENDRA AWASTHI-IONIC EEQUILIBRIUM-Assertin-Reason Type Questions
