In a 0.5 molal solution KCl, KCl is 50% dissociated. The freezing point of solution will be ( K_(f) = 1.86 K kg mol^(-1) ):
0.2 m aqueous solution of a weak acid is 20% dissociated. The boiling point of this solution is (K_(b) of water= 0.52Km^-1)
In a 0.2 molal aqueus solution of a weak acid HX the degree of dissociation is 0.25. The freezing point of the solution will be nearest to: ( K_(f)=1.86 K kg "mol"^(-1) ) a) -0.26^(@)C b) 0.465^(@)C c) -0.48^(@)C d) -0.465^(@)C
An aqueous solution of urea has a freezing point of -0.515^(@)C . Predict the osmotic pressure (in atm) of the same solution at 37^(@)C .
An aqueous solution freezes at 1.186^(@)C ( K_(f)=1.86,K_(b)=0.512 ). What is the elevation in boiling point?
An aqueous solution freezes at 272.07K, while pure water freezes at 273K. Determine the molality of the solution. (given K_f for water= 1.86K/m
When 36.0 g of a solute having the empirical formula CH_(2)O is dissovled in 1.20 kg of water, the solution freezes at -0.93^(@)C . What is the moleculer formula of the solute ? ( K_(f) = 1.86^(@)C kg mol^(-1) )
A certain non-volatile electrolyte contain 40% carbon, 6.7% hydrogen and 53.3% oxygen.An aqueous solution containing 5% by mass of the solute boils at 100.15^(@) C. Determine molecular formula of the compound( K_(b) =0.51^(@)C//m ):
1 . 5 of Ba (NO_(3))_(2) dissolved in 100 g of water shows a depression in freezing point equal to 0 . 28^(@)C . What is the percentage dissociation of the salt ? ( K_(f) for water = 1 . 86 K/m and molar mass of Ba (NO_(3))_(2) = 261.)
NARENDRA AWASTHI-DILUTE SOLUTION-Level 3 - Match The Column
