The mass of carbon present in 0.5 mol of K, [Fe(CN)g] is : a. 1.8 g b. 18g c. 3.6 g d. 36 g 2 m

The freezing point of a solution containing 0.1g of K_3[Fe(CN)_6] in 100 g of water. (K_f=1.86 K kg mol^-1) is

The freezing point ( "in"^(@)"C" ) of a solution containing 0.1 g of K_(3)[Fe(CN)_(6)] ( Mol. Wt. 329) in 100g of water ( K_(f)"=1.86 k kg mol"^(-1)) is

The freezing point of a solution containing 0.1g of K_3[Fe(CN)_6] (Mol. Wt. 329) in 100 g of water ( K_f =1.86K kg mol^(−1) ) is:

Calculate the depression in the freezing point of a solution containing 0.1 g of K_(3)[Fe(CN)_(6)] in 100 g of H_(2)O ? (molecular weigth of K_(3)[Fe(CN)_(6)]=329, K_(f)=1.86K " kg mol"^(-1) )

10.1 g of KNO_(3) is dissolved in 500 mL of H_(2) O . Mass of Ba(NO_(3))_(2) that should be added to this solution of get a molality (m) of 0.3 with respect to NO_(3)^(ɵ) ion is (Mw of KNO_(3) = 101 g mol^(-1), Mw of Ba(No_(3))_(2) = 261 g mol^(-1)) a. ~~ 1.3 g b. ~~ 13 g c. ~~ 6.5 g d. ~~ 65 g

10.1 g of KNO_(3) is dissolved in 500 mL of H_(2) O . Mass of Ba(NO_(3))_(2) that should be added to this solution of get a molality (m) of 0.3 with respect to NO_(3)^(ɵ) ion is (Mw of KNO_(3) = 101 g mol^(-1), Mw of Ba(No_(3))_(2) = 261 g mol^(-1)) a. ~~ 1.3 g b. ~~ 13 g c. ~~ 6.5 g d. ~~ 65 g

The freezing point (in ""^(@)C ) for a solution containing 0.1 g of K_(3)[Fe(CN)_(6)] (mol wt 329) in 100 g water (K_(f)=1.86K kg"mol"^(-1)0 is